Metals conduct electricity using magnetic fields.

Metals conduct electricity through the vibration of atoms.

Metals conduct electricity by trapping electrons in fixed positions.

Metals conduct electricity through the movement of free electrons.

Liquid

Plasma

Solid

Gas

Metals can only be melted and not reshaped.

Metals are only malleable at high temperatures.

Metals are malleable, meaning they can be easily shaped into thin sheets without breaking.

Metals are brittle and cannot be shaped easily.

Metallic luster is unrelated to the structure of materials.

Metallic luster is only found in non-metallic substances.

Metallic luster indicates a lack of conductivity.

Metallic luster signifies the presence of metallic bonds and indicates properties like conductivity and reflectivity.

Non-metals conduct electricity better than metals.

Both non-metals and metals are excellent conductors of electricity.

Non-metals are good conductors of electricity, while metals are poor conductors.

Non-metals are poor conductors of electricity, while metals are good conductors.

Good conductors of heat and electricity

1. Poor conductors of heat and electricity, 2. Brittle in solid form, 3. Typically have high electronegativities.

Malleable in solid form

Typically have low electronegativities

All non-metals are solids at room temperature.

Non-metals are only gases at room temperature.

Non-metals can be gases, liquids, or solids at room temperature.

Non-metals are exclusively liquids at room temperature.

Non-metals lose electrons to metals, forming covalent bonds.

Non-metals do not react with metals at all.

Non-metals react with metals by sharing electrons, creating metallic bonds.

Non-metals react with metals by gaining electrons, forming ionic compounds.

Non-metals generally have higher density than metals.

Non-metals have variable density similar to metals.

Non-metals are always denser than liquids.

Non-metals typically have lower density than metals.

Metallic bonding is characterized by fixed electrons that do not move.

Metallic bonding involves a 'sea of electrons' that are delocalized among positively charged metal ions, allowing for conductivity and malleability.

Metallic bonding occurs when electrons are tightly bound to individual atoms.

Metallic bonding is the attraction between non-metal atoms.

Delocalized electrons are only present in non-metallic substances.

Delocalized electrons make metals brittle and non-malleable.

Delocalized electrons prevent electrical conductivity in metals.

Delocalized electrons allow for electrical conductivity and contribute to the malleability and ductility of metals.

Metals are composed of isolated atoms that do not move freely.

The structure of metals, characterized by closely packed atoms and free-moving electrons, contributes to their conductivity, malleability, strength, and ductility.

The structure of metals prevents them from conducting electricity.

Metals have a random atomic structure that makes them brittle.

Non-metallic bonding is characterized by covalent bonds formed through the sharing of electrons between non-metal atoms.

Non-metallic bonding is characterized by the transfer of electrons from non-metals to metals.

Non-metallic bonding involves metallic bonds between metal and non-metal atoms.

Non-metallic bonding occurs only in ionic compounds formed by non-metal elements.

Ionic bond

Hydrogen bond

Covalent bond

Metallic bond

Reactivity is the same for all metals regardless of their position.

Reactivity increases down a group and decreases across a period in the periodic table.

Reactivity is only influenced by the atomic mass of the metals.

Reactivity decreases down a group and increases across a period.

Alkali metals

Lanthanides

Transition metals

Noble gases

The reactivity of metals increases as you move down a group in the periodic table.

The reactivity of metals decreases as you move down a group in the periodic table.

The reactivity of metals remains constant as you move down a group in the periodic table.

The reactivity of metals fluctuates randomly as you move down a group in the periodic table.

Non-metals do not react with oxygen.

Non-metals react with oxygen to form acids.

Non-metals react with oxygen to produce heat.

Non-metals react with oxygen to form oxides.

Noble gases are more reactive than other non-metals.

Noble gases have similar reactivity to halogens.

Noble gases are highly reactive and form compounds easily.

Noble gases are much less reactive than other non-metals.

Nitrogen

Oxygen

Hydrogen

None of the above

a

b

c

d

a

b

c

d

(a) (i) and (ii)

(b) (i) and (iii)

(c) (ii) and (iii)

(d) (i) and (iv)

hydrogen

carbon dioxide

magnesium oxide / basic in nature

magnesium oxide / acidic in nature

gold

platinium

silver

iron

Copper

Silver

Sodium

Tungsten

Oxygen

Nitrogen

Chlorine

Iodine

Has high melting point

Has low melting point

Conducts electricity in molten state

Occurs as solid