WorksheetsChemistry revision - bonding
Total questions: 11
Worksheet time: 5mins
What type of elements can react using covalent bonding?
metals only
non-metals only
metals and non-metals together
any element can react
What type of force holds the atoms together in all of the different types of bonding?
ionic bonding
intermolecular forces
electrostatic forces of attraction
electromagnetic forces
Define ionic bonding.
when atoms share electrons so both atoms have a full outer shell
when atoms lose electrons so both atoms have a full outer shell
when atoms swap electrons so both atoms have a full outer shell
when atoms gain electrons so both atoms have a full outer shell
What type of elements can react using ionic bonding?
metals only
non-metals only
metals and non-metals together
any element can react
Define metallic bonding.
the electrostatic force of attraction between two metals
the electrostatic force of attraction between the positive ions and delocalised electrons
the electrostatic force of attraction between the positive and negative ions
the metallic bonding in a metal due to intermolecular forces
Explain why metals can conduct electricity.
metals have delocalised electrons that are free to move
metals have delocalised ions that are free to move
metals have ions that are free to move
metals have atoms that are free to move
Why are metals malleable?
the layers of atoms are arranged in a regular structure and can slide over each other
the atoms have different sizes so they can slide over each other
the atoms are arranged in an irregular structure and slide over each other in certain directions
the layers of atoms are arranged in an irregular structure and can slide over each other
Why are alloys stronger than pure metals?
alloys have lots of different elements interacting with each other
alloys have lots of covalent bonds between the different atoms
pure metals have metallic bonding between the different metals which is very strong
the atoms have different sizes so the alloy has an irregular structure and the layers can't slide over each other
Why will group 2 metals have a higher melting point than group 1 metals?
group 2 elements have more ionic bonding than group 1
group 2 exhibits stronger covalent bonds between the metals
group 2 exhibits stronger electrostatic forces of attraction between the higher charge of the ion and the delocalised electrons
group 2 has more protons and neutrons which requires more energy to break apart
Why will group 2 metals be better electrical conductors than group 1 metals?
they have twice as many delocalised electrons
they have twice as many ions that are free to move
they have stronger metallic bonding which helps conductivity
they have more protons and electrons than group 1
Define covalent bonding.
swapping of electrons
a shared pair of electrons
an electron being shared
transfer of electrons between metals and non-metals
