This chapter focuses on the classification, properties, and reactivity of metals and non-metals.
Metals and Non-metals - Quick Look Revision Guide
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This compact guide covers 20 must-know concepts from Metals and Non-metals aligned with Class X preparation for Science. Ideal for last-minute revision or daily review.
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Essential formulas, key terms, and important concepts for quick reference and revision.
Key Points
Metals are lustrous, malleable, ductile, and good conductors.
Metals have a shiny appearance, can be hammered into sheets, drawn into wires, and conduct heat and electricity well. Examples include iron, copper, and aluminium.
Non-metals are brittle, non-lustrous, and poor conductors.
Non-metals lack shine, break easily, and do not conduct heat or electricity efficiently. Examples are sulphur, carbon, and oxygen.
Metals react with oxygen to form basic oxides.
When metals react with oxygen, they form oxides that are basic in nature. For example, magnesium oxide (MgO) is a basic oxide.
Non-metals react with oxygen to form acidic or neutral oxides.
Non-metals form oxides that are either acidic or neutral. Sulphur dioxide (SO2) is an acidic oxide, while carbon monoxide (CO) is neutral.
Amphoteric oxides react with both acids and bases.
Oxides like aluminium oxide (Al2O3) and zinc oxide (ZnO) can react with both acids and bases, showing dual nature.
Metals displace hydrogen from dilute acids.
Metals above hydrogen in the reactivity series can displace hydrogen from acids. For example, zinc reacts with HCl to form zinc chloride and hydrogen gas.
Non-metals do not displace hydrogen from acids.
Non-metals cannot displace hydrogen from dilute acids as they are less reactive than hydrogen.
Reactivity series arranges metals by their reactivity.
The series starts with the most reactive metal (potassium) and ends with the least reactive (gold). It helps predict displacement reactions.
Ionic compounds have high melting and boiling points.
Due to strong electrostatic forces between ions, ionic compounds like NaCl have high melting and boiling points.
Metals are extracted from their ores via reduction.
Metals are obtained by reducing their oxides. For example, iron is extracted by reducing iron oxide with carbon.
Electrolytic refining purifies metals like copper.
Impure metal is made the anode, pure metal the cathode, and metal salt solution the electrolyte. Pure metal deposits on the cathode.
Corrosion is the deterioration of metals by oxidation.
Iron rusts in moist air forming Fe2O3.xH2O. Prevention methods include painting, galvanizing, and alloying.
Alloys enhance metal properties.
Mixing metals or with non-metals improves properties. Steel (iron + carbon) is stronger than pure iron.
Gold and platinum are least reactive metals.
They do not corrode easily and are found in native state, making them ideal for jewelry.
Sodium and potassium are stored under oil.
They are highly reactive with air and water, so storing under oil prevents unwanted reactions.
Thermit reaction uses aluminium to extract metals.
Aluminium reduces metal oxides to metals in this highly exothermic reaction, used for welding rails.
Metals conduct electricity due to free electrons.
The sea of delocalized electrons in metals allows them to conduct electricity efficiently.
Non-metals gain electrons to form anions.
Non-metals have high electronegativity, gaining electrons to form negatively charged ions, like Cl-.
Metals lose electrons to form cations.
Metals have low ionization energy, losing electrons to form positively charged ions, like Na+.
Aqua regia dissolves gold and platinum.
A mix of concentrated HCl and HNO3 in 3:1 ratio, aqua regia can dissolve noble metals like gold.
Galvanization prevents rusting by zinc coating.
Coating iron with zinc protects it from rusting, even if the coating is broken, due to zinc's sacrificial protection.
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