{"id":14165,"date":"2020-11-30T08:52:55","date_gmt":"2020-11-30T03:22:55","guid":{"rendered":"https:\/\/cbselibrary.com\/?p=14165"},"modified":"2020-11-30T11:43:18","modified_gmt":"2020-11-30T06:13:18","slug":"physical-chemical-properties-group-1-elements","status":"publish","type":"post","link":"https:\/\/cbselibrary.com\/physical-chemical-properties-group-1-elements\/","title":{"rendered":"Physical and Chemical Properties of Group 1 Elements"},"content":{"rendered":"<h2><strong>Physical and Chemical Properties of Group 1 Elements<\/strong><\/h2>\n<p><strong>Group 1 Elements: The Alkali Metals<\/strong><\/p>\n<p>The elements in Group 1 are:<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109607\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-1.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 1\" width=\"377\" height=\"56\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-1.png 377w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-1-300x45.png 300w\" sizes=\"(max-width: 377px) 100vw, 377px\" \/><br \/>\nThese elements are known as <strong>alkali metals.<\/strong><\/p>\n<h3><strong>Physical Properties of Group 1 Elements<\/strong><\/h3>\n<p><strong>1.<\/strong> Table shows some properties of Group 1 elements.<\/p>\n<table style=\"height: 216px;\" border=\"2\" width=\"781\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"66\"><strong>Element<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"58\"><strong>Proton number<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"63\"><strong>Nucleon number<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"59\"><strong>Density (g cm<sup>-3<\/sup>)<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"68\"><strong>Hardness (Brinell)<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"60\"><strong>Melting point (\u00b0C)<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"57\"><strong>Boiling point (\u00b0C)<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"57\"><strong>Atomic radius (nm)<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"116\"><strong>Electro<br \/>\nnegativity<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Lithium<\/td>\n<td style=\"text-align: center;\" width=\"58\">3<\/td>\n<td style=\"text-align: center;\" width=\"63\">7<\/td>\n<td style=\"text-align: center;\" width=\"59\">0.53<\/td>\n<td style=\"text-align: center;\" width=\"68\">0.06<\/td>\n<td style=\"text-align: center;\" width=\"60\">181<\/td>\n<td style=\"text-align: center;\" width=\"57\">1347<\/td>\n<td style=\"text-align: center;\" width=\"57\">0.15<\/td>\n<td style=\"text-align: center;\" width=\"116\">1.0<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Sodium<\/td>\n<td style=\"text-align: center;\" width=\"58\">11<\/td>\n<td style=\"text-align: center;\" width=\"63\">23<\/td>\n<td style=\"text-align: center;\" width=\"59\">0.97<\/td>\n<td style=\"text-align: center;\" width=\"68\">0.07<\/td>\n<td style=\"text-align: center;\" width=\"60\">98<\/td>\n<td style=\"text-align: center;\" width=\"57\">886<\/td>\n<td style=\"text-align: center;\" width=\"57\">0.19<\/td>\n<td style=\"text-align: center;\" width=\"116\">0.9<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Potassium<\/td>\n<td style=\"text-align: center;\" width=\"58\">19<\/td>\n<td style=\"text-align: center;\" width=\"63\">39<\/td>\n<td style=\"text-align: center;\" width=\"59\">0.86<\/td>\n<td style=\"text-align: center;\" width=\"68\">0.04<\/td>\n<td style=\"text-align: center;\" width=\"60\">64<\/td>\n<td style=\"text-align: center;\" width=\"57\">774<\/td>\n<td style=\"text-align: center;\" width=\"57\">0.23<\/td>\n<td style=\"text-align: center;\" width=\"116\">0.8<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Rubidium<\/td>\n<td style=\"text-align: center;\" width=\"58\">37<\/td>\n<td style=\"text-align: center;\" width=\"63\">85<\/td>\n<td style=\"text-align: center;\" width=\"59\">1.53<\/td>\n<td style=\"text-align: center;\" width=\"68\">0.03<\/td>\n<td style=\"text-align: center;\" width=\"60\">39<\/td>\n<td style=\"text-align: center;\" width=\"57\">688<\/td>\n<td style=\"text-align: center;\" width=\"57\">0.25<\/td>\n<td style=\"text-align: center;\" width=\"116\">0.8<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Caesium<\/td>\n<td style=\"text-align: center;\" width=\"58\">55<\/td>\n<td style=\"text-align: center;\" width=\"63\">133<\/td>\n<td style=\"text-align: center;\" width=\"59\">1.87<\/td>\n<td style=\"text-align: center;\" width=\"68\">0.02<\/td>\n<td style=\"text-align: center;\" width=\"60\">28<\/td>\n<td style=\"text-align: center;\" width=\"57\">678<\/td>\n<td style=\"text-align: center;\" width=\"57\">0.26<\/td>\n<td style=\"text-align: center;\" width=\"116\">0.7<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Francium<\/td>\n<td style=\"text-align: center;\" width=\"58\">87<\/td>\n<td style=\"text-align: center;\" width=\"63\">223<\/td>\n<td style=\"text-align: center;\" width=\"59\">2.40<\/td>\n<td style=\"text-align: center;\" width=\"68\">?<\/td>\n<td style=\"text-align: center;\" width=\"60\">27<\/td>\n<td style=\"text-align: center;\" width=\"57\">677<\/td>\n<td style=\"text-align: center;\" width=\"57\">0,29<\/td>\n<td style=\"text-align: center;\" width=\"116\">0.7<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong>2. General physical properties of Group 1 elements:<\/strong><\/p>\n<ul>\n<li style=\"list-style-type: none;\">\n<ul>\n<li>Alkali metals are <strong>grey solids<\/strong> with <strong>shiny silvery surfaces<\/strong> when freshly cut.<\/li>\n<li>These surfaces <strong>turn dull<\/strong> when exposed to air.<\/li>\n<li>This is because alkali metals are <strong>very reactive.<\/strong> They react rapidly with oxygen and water vapour in the air when exposed.<\/li>\n<\/ul>\n<\/li>\n<li>Alkali metals are <strong>soft solids<\/strong> and can be <strong>easily cut.<\/strong><\/li>\n<li>Alkali metals have <strong>low densities<\/strong> as compared to heavy metals such as iron and copper.<\/li>\n<li>Alkali metals are <strong>good conductors<\/strong> of <strong>heat<\/strong> and <strong>electricity.<\/strong><\/li>\n<li>Alkali metals have <strong>low melting<\/strong> and <strong>boiling points<\/strong> as compared to heavy metals such as copper and iron.<\/li>\n<\/ul>\n<p>Table compares the melting and boiling points of potassium (an alkali metal) and copper (a heavy metal).<\/p>\n<table style=\"height: 34px;\" border=\"2\" width=\"394\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"124\"><strong>Element<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"66\">Potassium<\/td>\n<td style=\"text-align: center;\" width=\"67\">Copper<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"124\"><strong>Melting point (\u00b0C)<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"66\">64<\/td>\n<td style=\"text-align: center;\" width=\"67\">1083<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"124\"><strong>Boiling point (\u00b0C)<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"66\">774<\/td>\n<td style=\"text-align: center;\" width=\"67\">2567<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong>3. Trend of change in the physical properties<\/strong><br \/>\nThe physical properties of the elements <strong>vary gradually<\/strong> when <strong>going down Group 1<\/strong> as shown in Table.<\/p>\n<table border=\"2\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"58\"><strong>Group 1 elements<\/strong><\/td>\n<td style=\"text-align: center;\" colspan=\"4\" width=\"547\"><strong>Trend of change in the physical properties<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"58\"><img loading=\"lazy\" class=\"alignnone size-full wp-image-109626\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-2.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 2\" width=\"63\" height=\"303\" \/><\/td>\n<td style=\"text-align: center;\" width=\"112\">The <strong>atomic radius (atomic size)<\/strong> of alkali metals <strong>increases gradually\u00a0<\/strong>down the group.<\/p>\n<p><strong>Reason:<\/strong><br \/>\nThe <strong>number of shells\u00a0<\/strong>occupied with electrons <strong>increases<\/strong> down the group.<\/td>\n<td style=\"text-align: center;\" width=\"197\">Although alkali metals have <strong>low densities,<\/strong> the densities <strong>increase gradually<\/strong> down the group.<\/p>\n<p><strong>For example:<\/strong><br \/>\nLithium, sodium and potassium are <strong>less dense<\/strong> than water. Thus, these metals <strong>float<\/strong> on the water surface.<br \/>\nRubidium, caesium and francium are <strong>denser<\/strong> than water. Thus, these metals <strong>sink<\/strong> in water.<\/p>\n<p>Metallic bond means the chemical bond that holds the atoms together in a metal.<\/td>\n<td style=\"text-align: center;\" width=\"150\">Although alkali metals have <strong>low melting and boiling points,<\/strong> the melting and boiling points <strong>decrease gradually <\/strong>down the group.<\/p>\n<p><strong>Reason:<br \/>\n<\/strong>As the <strong>atomic size increases<\/strong> down the group, <strong>the metallic bond<\/strong> between the atoms of alkali metals <strong>becomes weaker.<\/strong> Hence, <strong>less heat energy<\/strong> is required to overcome the weaker metallic bonding during melting or boiling when going down the group.<\/td>\n<td style=\"text-align: center;\" width=\"88\">Alkali metals <strong>become softer<\/strong> down the group.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong>People also ask<\/strong><\/p>\n<ul>\n<li><a href=\"https:\/\/cbselibrary.com\/history-periodic-table-elements\/\">What is the periodic table of the elements?<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/physical-chemical-properties-group-18-elements\/\">Physical and Chemical Properties of Group 18 Elements<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/physical-chemical-properties-group-17-elements\/\">Physical and Chemical Properties of Group 17 Elements<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/mean-transition-metals\/\">What do you mean by transition metals?<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/need-classification-elements\/\">What is the Need for Classification of Elements?<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/modern-periodic-table-significance\/\">Modern Periodic Table and Its Significance<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/mendeleev-arrange-the-periodic-table\/\">How did Mendeleev Arrange the Periodic Table?<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/periodic-trends-properties-elements\/\">Periodic Trends in Properties of Elements<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/valency-and-atomic-radius\/\">What is Valency and Atomic Radius?<\/a><\/li>\n<li><a href=\"https:\/\/cbselibrary.com\/metallic-and-nonmetallic-properties\/\">What are Metallic and Nonmetallic Properties?<\/a><\/li>\n<\/ul>\n<h3><strong>Chemical <\/strong><strong>Properties of Group 1 Elements<\/strong><\/h3>\n<p><strong>1.<\/strong> Table shows the electron arrangements of alkali metals.<\/p>\n<table border=\"2\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"89\"><strong>Element<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"169\"><strong>Electron arrangement<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"89\">Lithium<\/td>\n<td style=\"text-align: center;\" width=\"169\">2.1<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"89\">Sodium<\/td>\n<td style=\"text-align: center;\" width=\"169\">2.8.1<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"89\">Potassium<\/td>\n<td style=\"text-align: center;\" width=\"169\">2.8.8.1<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"89\">Rubidium<\/td>\n<td style=\"text-align: center;\" width=\"169\">2.8.18.8.1<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"89\">Caesium<\/td>\n<td style=\"text-align: center;\" width=\"169\">2.8.18.18.8.1<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"89\">Francium<\/td>\n<td style=\"text-align: center;\" width=\"169\">2.8.18.32.18.8.1<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong>2. Similar chemical properties<\/strong><\/p>\n<ul>\n<li>All alkali metal exhibit <strong>similar chemical properties.<\/strong><\/li>\n<li>This is because all the atoms of alkali metals have <strong>one valence electron.<\/strong><\/li>\n<\/ul>\n<p><strong>3. Reactivity<\/strong><\/p>\n<p>Alkali metals are <strong>very reactive.<\/strong><br \/>\nAlthough alkali metals exhibit similar chemical properties, they <strong>differ<\/strong> in <strong>reactivity.<\/strong><br \/>\nThe <strong>reactivity<\/strong> of alkali metals <strong>increases<\/strong> when going down Group 1.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109648\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-3.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 3\" width=\"316\" height=\"41\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-3.png 316w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-3-300x39.png 300w\" sizes=\"(max-width: 316px) 100vw, 316px\" \/><br \/>\nThe reactivity of an alkali metal is measured by how easily its atom loses its single valence electron to achieve a <strong>stable noble gas electron arrangement<\/strong> (duplet or octet electron arrangement).<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109662\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-4.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 4\" width=\"230\" height=\"50\" \/><br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109665\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-5.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 5\" width=\"232\" height=\"109\" \/><br \/>\nThe <strong>easier<\/strong> an alkali metal atom <strong>releases its single valence electron,<\/strong> the <strong>more reactive<\/strong> is the alkali metal.<\/p>\n<p><strong>Explanation:<\/strong><br \/>\nThe increase in reactivity of alkali metals down Group 1 can be explained as follows.<\/p>\n<ul>\n<li>All alkali metals have <strong>one valence electron.<\/strong><\/li>\n<li>Each atom of an alkali metal will release <strong>one valence electron during<\/strong> a chemical reaction to achieve a <strong>stable duplet<\/strong> or <strong>octet<\/strong> electron arrangement. Hence, an ion with a charge of+1 is formed.\n<ul>\n<li>When going down Group 1, the <strong>atomic size<\/strong> of alkali metals <strong>increases<\/strong>.<\/li>\n<li>The single valence electron becomes <strong>further away<\/strong> from the nucleus and is <strong>screened<\/strong> by more inner shells containing electrons.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109671\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-6.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 6\" width=\"175\" height=\"288\" \/><\/li>\n<\/ul>\n<\/li>\n<li>This means that the <strong>effective nuclear charge<\/strong> felt by the single valence electron <strong>decreases<\/strong> when going down the group.<\/li>\n<li>This causes the attractive forces between the nucleus and the single valence electron become weaker, so the single valence electron is <strong>more weakly pulled<\/strong> by the nucleus.<\/li>\n<li>Hence, the single valence electron can be <strong>released more easily<\/strong> when going down the group.<\/li>\n<li>As a result, the reactivity of alkali metals <strong>increases<\/strong> down the group.<\/li>\n<\/ul>\n<p><strong>4. As reducing agents<\/strong><\/p>\n<ul>\n<li>Reducing agents are <strong>good electron donors<\/strong> in chemical reactions.<\/li>\n<li>Alkali metals are <strong>good reducing agents<\/strong> because the <strong>single valence electron<\/strong> in the atom of each alkali metal can be easily released to <strong>achieve<\/strong> a stable electron arrangement of a noble gas (good electron donor).\n<ul>\n<li>The <strong>strength<\/strong> of alkali metals as reducing agents <strong>increases<\/strong> when going down Group 1.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109672\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-7.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 7\" width=\"385\" height=\"50\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-7.png 385w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-7-300x39.png 300w\" sizes=\"(max-width: 385px) 100vw, 385px\" \/><\/li>\n<li>This is because the <strong>single valence electron<\/strong> of the alkali metals becomes <strong>much easier to be released<\/strong> when going down the group.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n<p><strong>5. Electropositivity<\/strong><\/p>\n<ul>\n<li><strong>(a) Definition:<\/strong><br \/>\n<strong>Electropositivity<\/strong> of an element is a measurement of the ability of an atom to donate electrons to form a positive ion.<\/p>\n<ul>\n<li>Alkali metals are <strong>very electropositive.<\/strong><\/li>\n<li>This is because the atom of each alkali metal can release its single valence electron easily to form a positive ion.<\/li>\n<\/ul>\n<\/li>\n<li>However, the <strong>electropositivity<\/strong> of alkali metals <strong>increases<\/strong> when going down Group 1.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109674\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-8.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 8\" width=\"380\" height=\"50\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-8.png 380w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-8-300x39.png 300w\" sizes=\"(max-width: 380px) 100vw, 380px\" \/><\/li>\n<\/ul>\n<p>This can be explained as below:<\/p>\n<ul>\n<li>The <strong>atomic size<\/strong> of alkali metals <strong>increases<\/strong> from lithium to francium.<\/li>\n<li>The <strong>single valence electron<\/strong> in the outermost occupied shell becomes <strong>further away<\/strong> from the nucleus and is <strong>screened<\/strong> by more inner shells containing electrons.<\/li>\n<li>So, the attractive forces between the nucleus and the single valence electron become weaker when going down Group 1.<\/li>\n<li>This causes the single valence electron <strong>to be released<\/strong> more easily when going down Group 1.<\/li>\n<li>As a result, the <strong>electropositivity<\/strong> of alkali metals <strong>increases<\/strong> when going down the group.<\/li>\n<\/ul>\n<p><strong>6.<\/strong> Group 1 elements exhibit <strong>similar chemical properties<\/strong> in their reactions with<\/p>\n<ul>\n<li><strong>water<\/strong> to liberate hydrogen gas and form metal hydroxide.<\/li>\n<li><strong>oxygen<\/strong> to produce metal oxides.<\/li>\n<li><strong>chlorine<\/strong> to produce metal chloride.<\/li>\n<li><strong>bromine<\/strong> to produce metal bromide.<\/li>\n<\/ul>\n<p><strong>7. To predict the properties of rubidium, caesium and francium<\/strong><\/p>\n<ul>\n<li>Rubidium, caesium and francium are <strong>placed below<\/strong> potassium in Group 1 of the Periodic Table.<\/li>\n<li>Hence, rubidium, caesium and francium are expected to react with water, oxygen, chlorine or bromine in a <strong>similar way<\/strong> as potassium but these reactions are <strong>more vigorous (more reactive)<\/strong> than potassium.<\/li>\n<li>For example:<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109696\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-9.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 9\" width=\"394\" height=\"203\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-9.png 394w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-9-300x155.png 300w\" sizes=\"(max-width: 394px) 100vw, 394px\" \/><\/li>\n<\/ul>\n<p><strong>8. Solubility of the salts of alkali metals<\/strong><\/p>\n<ul>\n<li>Carbonate, nitrate, chloride, sulphate, bromide and iodide salts of alkali metals are <strong>white solids.<\/strong><\/li>\n<li>These salts are soluble in water. They dissolve in water to form colourless solutions.<\/li>\n<\/ul>\n<p><strong>9. Safety precautions in handling Group 1 elements<\/strong><\/p>\n<ul>\n<li>Alkali metals are <strong>very reactive.<\/strong><\/li>\n<li>Alkali metals, when exposed, can react with <strong>oxygen and water vapour<\/strong> in the air.<\/li>\n<li>Hence, alkali metals such as lithium, sodium and potassium must be kept in paraffin oil, whereas rubidium and caesium are stored in sealed glass tubes. This is to prevent them from reacting with oxygen and water vapour in the air.<\/li>\n<li>The following <strong>safety precautions<\/strong> must be taken when handling alkali metals.\n<ul>\n<li><strong>Avoid<\/strong> holding the highly reactive alkali metals with your <strong>bare hands.<\/strong><\/li>\n<li>Wear <strong>safety goggles<\/strong> and <strong>gloves<\/strong> during an experiment.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n<h2><strong>Chemical Properties of Group 1 Elements Experiment 1<\/strong><\/h2>\n<p><strong>Aim:<\/strong> To investigate the chemical properties of Group 1 metals in their reactions with water and oxygen.<br \/>\n<strong>Problem statement:<\/strong> How do Group 1 metals react with water and oxygen?<\/p>\n<p><strong>A. Reactions of alkali metals with water<\/strong><\/p>\n<p><strong>Hypothesis:<\/strong> When going down Group 1, alkali metals become more reactive in their reactions with water.<br \/>\n<strong>Variables:<\/strong><br \/>\n(a) Manipulated variable : Different types of alkali metals<br \/>\n(b) Responding variable : Reactivity of alkali metals<br \/>\n(c) Controlled variables : Water, size of alkali metals<br \/>\n<strong>Operational definition:<\/strong> An alkali metal that reacts more vigorously and rapidly with water is a more reactive metal. <strong>Materials:<\/strong> Small pieces of lithium, sodium and potassium, distilled water, red litmus paper and filter paper.<br \/>\n<strong>Apparatus:<\/strong> Water troughs, small knife and forceps.<br \/>\n<strong>Safety Measure:<\/strong><br \/>\nDo not touch the extremely reactive alkali metals with your bare hands.<br \/>\nAlways wear safety goggles and gloves.<br \/>\n<strong>Procedure:<\/strong><br \/>\n<strong>A. small piece of lithium is cut out using a knife.<\/strong><\/p>\n<ol>\n<li>The oil on the surface of lithium is removed by rolling it on a piece of filter paper.<\/li>\n<li>The lithium is then placed slowly onto the water surface in a water trough with the help of forceps, as shown in Figure.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109698\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-10.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 10\" width=\"227\" height=\"127\" \/><\/li>\n<li>All changes that occur are recorded.<\/li>\n<li>When the reaction stops, the solution formed is tested with a piece of red litmus paper.<\/li>\n<li>Steps 1 to 5 are repeated using sodium and potassium respectively to replace lithium.<\/li>\n<\/ol>\n<p><strong>Observations:<br \/>\n<\/strong><\/p>\n<table border=\"2\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"99\"><strong>Alkali metal<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"488\"><strong>Observation<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"99\">Lithium<\/td>\n<td style=\"text-align: center;\" width=\"488\">Lithium moves<strong> slowly<\/strong> on the water surface with a soft &#8216;hiss&#8217; sound. A <strong>colourless solution<\/strong> that <strong>turns red litmus paper blue<\/strong> is formed.<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"99\">Sodium<\/td>\n<td style=\"text-align: center;\" width=\"488\">Sodium melts to become a small sphere, moves <strong>rapidly<\/strong> and <strong>randomly<\/strong> on the water surface with a hiss&#8217; sound. A <strong>colourless solution<\/strong> that <strong>turns red litmus paper blue<\/strong> is formed.<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"99\">Potassium<\/td>\n<td style=\"text-align: center;\" width=\"488\">Potassium melts to become a small sphere, burns with a <strong>lilac flame,<\/strong> moves <strong>very rapidly<\/strong> and <strong>randomly<\/strong> on the water surface with &#8216;hiss&#8217; and &#8216;pop&#8217; sounds. A <strong>colourless solution<\/strong> that <strong>turns red litmus paper blue<\/strong> is formed.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong> Discussion:<\/strong><\/p>\n<ol>\n<li>The alkali metals <strong>fizz and push around<\/strong> on the water surface like a hovercraft. This is <strong>due to the liberation of hydrogen gas<\/strong> as they react with water.<\/li>\n<li>Lithium, sodium and potassium react with water to produce a <strong>colourless gas<\/strong> (&#8216;hissing&#8217; sound) and an <strong>alkaline solution<\/strong> (metal hydroxide) that turns red litmus paper <strong>blue.<\/strong> Hence, lithium, sodium and potassium <strong>exhibit similar chemical properties.<\/strong><\/li>\n<li>The observations also show that the <strong>reactivity<\/strong> of the alkali metals in their reactions with water <strong>increases<\/strong> from lithium \u2192 sodium \u2192 potassium.<\/li>\n<li>Alkali metals react with water to produce a metal hydroxide solution (an alkaline solution) and hydrogen gas.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109699\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-11.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 11\" width=\"690\" height=\"160\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-11.png 690w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-11-300x70.png 300w\" sizes=\"(max-width: 690px) 100vw, 690px\" \/><\/li>\n<\/ol>\n<p><strong>B. Reactions of alkali metals with oxygen<\/strong><\/p>\n<p><strong>Hypothesis:<\/strong>\u00a0When going down Group 1, alkali metals become more reactive in their reactions with oxygen.<br \/>\n<strong>Variables:<\/strong><br \/>\n(a) Manipulated variable : Different types of alkali metals<br \/>\n(b) Responding variable : Reactivity of alkali metals<br \/>\n(c) Controlled variables : Oxygen gas, size of alkali metals<br \/>\n<strong>Operational definition:<\/strong> An alkali metal that burns more rapidly and vigorously in oxygen gas is a more reactive metal.<br \/>\n<strong>Materials:<\/strong> Small pieces of lithium, sodium and potassium, filter paper, red litmus paper and three gas jars filled<br \/>\nwith oxygen gas.<br \/>\n<strong>Apparatus:<\/strong> Forceps, gas jar spoon, small knife and Bunsen burner.<br \/>\n<strong>Procedure:<\/strong><\/p>\n<ol>\n<li>A small piece of lithium is cut out using a knife.<\/li>\n<li>The oil on the surface of lithium is removed by roiling it on a piece of filter paper.<\/li>\n<li>The lithium is then heated in a gas jar spoon until it starts to burn.<\/li>\n<li>The gas jar spoon with the burning lithium is then quickly lowered into a gas jar filled with oxygen gas, as shown in Figure.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109701\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-12.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 12\" width=\"187\" height=\"260\" \/><\/li>\n<li>The changes that occur are recorded.<\/li>\n<li>When the reaction stops, 10 cm3 of distilled water is poured into the gas jar and shaken well.<\/li>\n<li>The solution formed is then tested with a piece of red litmus paper.<\/li>\n<li>Steps 1 to 7 are repeated using sodium and potassium respectively to replace iithium.<\/li>\n<\/ol>\n<p><strong>Observations:<br \/>\n<\/strong><\/p>\n<table style=\"height: 276px;\" border=\"2\" width=\"844\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"66\"><strong>Alkali metal<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"524\"><strong>Observation<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Lithium<\/td>\n<td style=\"text-align: center;\" width=\"524\">Lithium burns <strong>slowly<\/strong> with a <strong>red flame<\/strong> and liberates white fumes which become a <strong>white solid<\/strong> on cooling to room temperature. The white solid dissolves in water to produce a <strong>colourless solution.<\/strong> This solution <strong>turns red litmus paper blue.<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Sodium<\/td>\n<td style=\"text-align: center;\" width=\"524\">Sodium burns <strong>rapidly<\/strong> and <strong>brightly<\/strong> with a <strong>yellow flame<\/strong> and liberates white fumes which become a <strong>white solid<\/strong> on cooling to room temperature. The white solid dissolves in water to produce a <strong>colourless solution.<\/strong> This solution <strong>turns red litmus paper blue.<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"66\">Potassium<\/td>\n<td style=\"text-align: center;\" width=\"524\">Potassium burns <strong>very rapidly<\/strong> and <strong>brightly<\/strong> with a <strong>lilac flame<\/strong> and liberates white fumes which become a <strong>white solid<\/strong> on cooling to room temperature. The white solid dissolves in water to produce a <strong>colourless solution.<\/strong> This solution <strong>turns red litmus paper blue.<\/strong><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong> Discussion:<\/strong><\/p>\n<ol>\n<li>Lithium, sodium and potassium burn in oxygen gas respectively to produce <strong>white fumes<\/strong> which then become a<strong> white solid (metal oxide).<\/strong> The white solid dissolves in water to form an <strong>alkaline solution (metal hydroxide). <\/strong>Hence, it can be inferred that these alkali metals <strong>exhibit similar chemical properties.\u00a0<\/strong><\/li>\n<li>From the <strong>brightness<\/strong> of the flame and the <strong>speed<\/strong> of burning, it can be inferred that the <strong>reactivity<\/strong> of the alkali metals in their reactions with oxygen gas <strong>increases<\/strong> from lithium \u2192\u00a0sodium \u2192\u00a0potassium.<\/li>\n<li>All the alkali metals react with oxygen gas when heated to produce white solid metal oxides.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109702\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-13.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 13\" width=\"680\" height=\"132\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-13.png 680w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-13-300x58.png 300w\" sizes=\"(max-width: 680px) 100vw, 680px\" \/><\/li>\n<li>The white solid metal oxides formed dissolve in water to produce metal hydroxide solutions which are alkaline.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109742\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-14.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 14\" width=\"497\" height=\"130\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-14.png 497w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-14-300x78.png 300w\" sizes=\"(max-width: 497px) 100vw, 497px\" \/><\/li>\n<\/ol>\n<p><strong>Conclusion:<\/strong><br \/>\nThe alkali metals <strong>exhibit similar chemical properties<\/strong> in their reactions with water or oxygen gas. The <strong>reactivity<\/strong> of alkali metals <strong>increases<\/strong> down Group 1. Hence, the hypothesis proposed can be accepted.<\/p>\n<h2><strong>Chemical Properties of Group 1 Elements Experiment 2<\/strong><\/h2>\n<p><strong>Aim:<\/strong> To investigate the chemical properties of Group 1 metals in their reactions with chlorine and bromine.<br \/>\n<strong>Problem statement:<\/strong> How do Group 1 metals react with chlorine and bromine?<br \/>\n<strong>Hypothesis: <\/strong>When going down Group 1, alkali metals become more reactive in their reactions with chlorine or bromine.<br \/>\n<strong>Variables:<\/strong><br \/>\n(a) Manipulated variable : Different types of alkali metals<br \/>\n(b) Responding variable : Reactivity of alkali metals<br \/>\n(c) Controlled variables : Chlorine and bromine, size of alkali metals<br \/>\n<strong>Operational definition:<\/strong> An alkali metal that reacts more vigorously and rapidly with chlorine or bromine gas is a more reactive metal.<br \/>\n<strong>Materials:<\/strong> Small pieces of lithium, sodium and potassium, filter paper, three gas jars filled with chlorine gas and three gas jars filled with bromine vapour.<br \/>\n<strong>Apparatus:<\/strong> Bunsen burner, forceps, gas jar spoon and small knife.<br \/>\n<strong>Safety Measures:<\/strong><br \/>\nChlorine gas and bromine vapour are poisonous. Wear gloves and safety goggles when handling these halogens.<br \/>\n<strong>Procedure:<\/strong><\/p>\n<ol>\n<li>A small piece of lithium is cut out using a knife.<\/li>\n<li>The oil on the surface of lithium is removed by rolling it on a piece of filter paper.<\/li>\n<li>The lithium is then heated in a gas jar spoon until it starts to burn.<\/li>\n<li>The gas jar spoon with the burning lithium is then quickly lowered into a gas jar filled with chlorine gas, as shown in Figure.<br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109744\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-15.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 15\" width=\"184\" height=\"250\" \/><\/li>\n<li>The changes that occur are recorded.<\/li>\n<li>Steps 1 to 5 are repeated using sodium and potassium respectively to replace lithium.<\/li>\n<li>Steps 1 to 6 are repeated using bromine vapour to replace chlorine gas.<\/li>\n<\/ol>\n<p><strong>Observations:<br \/>\n<\/strong><\/p>\n<table border=\"2\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" rowspan=\"2\" width=\"57\"><strong>Alkali metal<\/strong><\/td>\n<td style=\"text-align: center;\" colspan=\"2\" width=\"540\"><strong>Observation<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"223\"><strong>Chlorine gas<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"318\"><strong>Bromine vapour<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"57\">Lithium<\/td>\n<td style=\"text-align: center;\" width=\"223\">Lithium burns <strong>slowly<\/strong> with a <strong>red flame<\/strong> and liberates <strong>white fumes<\/strong> which become a <strong>white solid<\/strong> at the end of the reaction.<\/td>\n<td style=\"text-align: center;\" width=\"318\">Lithium burns <strong>slowly<\/strong> with a <strong>red flame<\/strong> and liberates <strong>white fumes<\/strong> which become a <strong>white solid<\/strong> at the end of the reaction. The reddish-brown bromine vapour is <strong>decolourised.<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"57\">Sodium<\/td>\n<td style=\"text-align: center;\" width=\"223\">Sodium burns <strong>rapidly<\/strong> and <strong>brightly<\/strong> with a <strong>yellow flame<\/strong> and liberates <strong>white fumes<\/strong> which become a <strong>white solid<\/strong> at the end of the reaction.<\/td>\n<td width=\"318\">\n<p style=\"text-align: center;\">Sodium burns <strong>rapidly<\/strong> and <strong>brightly<\/strong> with a <strong>yellow flame<\/strong> and liberates <strong>white fumes<\/strong> which become a <strong>white solid<\/strong> at the end of the reaction. The reddish-brown bromine vapour is <strong>decolourised.<\/strong><\/p>\n<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"57\">Potassium<\/td>\n<td style=\"text-align: center;\" width=\"223\">Potassium burns <strong>very rapidly<\/strong> and <strong>brightly<\/strong> with a lilac flame and liberates <strong>white fumes<\/strong> which become a <strong>white solid<\/strong> at the end of the reaction.<\/td>\n<td style=\"text-align: center;\" width=\"318\">Potassium burns <strong>very rapidly<\/strong> and <strong>brightly<\/strong> with a lilac flame and liberates <strong>white fumes<\/strong> which become a <strong>white<\/strong> solid at the end of the reaction. The reddish-brown bromine vapour is <strong>decolourised.<\/strong><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong> Discussion:<\/strong><\/p>\n<ol>\n<li>Lithium, sodium and potassium exhibit<strong> similar chemical properties<\/strong> in their reactions with <strong>chlorine gas<\/strong> or<strong> bromine vapour.<\/strong> This is because all these alkali metals have <strong>one valence electron.<\/strong><\/li>\n<li>From the <strong>brightness<\/strong> of the flame and the <strong>speed<\/strong> of burning, it can be inferred that the <strong>reactivity<\/strong> of alkali metals in their reactions with chlorine or bromine <strong>increases<\/strong> from lithium \u2192\u00a0sodium \u2192\u00a0potassium.<\/li>\n<li>All alkali metals react with chlorine gas when heated to produce <strong>white solid metal chlorides.<\/strong><br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109746\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-16.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 16\" width=\"672\" height=\"138\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-16.png 672w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-16-300x62.png 300w\" sizes=\"(max-width: 672px) 100vw, 672px\" \/><\/li>\n<li>Alkaliali metals react with brorr ine vapour when heated to produce <strong>white solid metal bromides.<\/strong><br \/>\n<img loading=\"lazy\" class=\"alignnone size-full wp-image-109747\" src=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-17.png\" alt=\"Physical and Chemical Properties of Group 1 Elements 17\" width=\"674\" height=\"132\" srcset=\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-17.png 674w, https:\/\/cbselibrary.com\/wp-content\/uploads\/2017\/05\/Physical-and-Chemical-Properties-of-Group-1-Elements-17-300x59.png 300w\" sizes=\"(max-width: 674px) 100vw, 674px\" \/><\/li>\n<\/ol>\n<p><strong>Conclusion:<\/strong><br \/>\nThe alkali metals exhibit <strong>similar chemical properties<\/strong> in their reactions with chlorine gas or bromine vapour. The <strong>reactivity<\/strong> of alkali metals <strong>increases<\/strong> down Group 1. Hence, the hypothesis proposed can be accepted.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Physical and Chemical Properties of Group 1 Elements Group 1 Elements: The Alkali Metals The elements in Group 1 are: These elements are known as alkali metals. Physical Properties of Group 1 Elements 1. Table shows some properties of Group 1 elements. Element Proton number Nucleon number Density (g cm-3) Hardness (Brinell) Melting point (\u00b0C) &#8230; <a title=\"Physical and Chemical Properties of Group 1 Elements\" class=\"read-more\" href=\"https:\/\/cbselibrary.com\/physical-chemical-properties-group-1-elements\/\" aria-label=\"More on Physical and Chemical Properties of Group 1 Elements\">Read more<\/a><\/p>\n","protected":false},"author":3,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"spay_email":""},"categories":[84],"tags":[5391,5390,5387,5385,5408,5409,5384,5393,5392,5389,5383,5388,5386],"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v17.8 (Yoast SEO v18.4.1) - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Physical and Chemical Properties of Group 1 Elements - CBSE Library<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/cbselibrary.com\/physical-chemical-properties-group-1-elements\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Physical and Chemical Properties of Group 1 Elements\" \/>\n<meta property=\"og:description\" content=\"Physical and Chemical Properties of Group 1 Elements Group 1 Elements: The Alkali Metals The elements in Group 1 are: These elements are known as alkali metals. Physical Properties of Group 1 Elements 1. Table shows some properties of Group 1 elements. Element Proton number Nucleon number Density (g cm-3) Hardness (Brinell) Melting point (\u00b0C) ... 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