Bonding

Question 1

What are the 3 types of chemical bond?

Answer 1

• Ionic
• Covalent (polar/non-polar)
• Metallic

Question 2

What does an ionic bond form between?

Answer 2

A metal and a non-metal

Question 3

If an electron is lost, what charge does the particle have?

Answer 3

Positive

Question 4

If an electron is gained, what charge does the particle have?

Answer 4

Negative

Question 5

What is a positively charged ion called?

Answer 5

Cation

Question 6

What is a negatively charged ion called?

Answer 6

Anion

Question 7

What is a covalent bond?

Answer 7

A bond formed between atoms by the sharing of electrons

Question 8

What is a non-polar covalent bond?

Answer 8

When electrons are shared equally

Question 9

What is a polar covalent bond?

Answer 9

When electrons are shared unequally

Question 10

What is the electron domain geometry of minimum repulsion?

Answer 10

Tetrahedral

Question 11

What is the trend in electronegativity in the periodic table?

Answer 11

Increased from left to right (across periods)

Question 12

What model is based on the idea that electron pairs will repel each other?

Answer 12

Valence shell electron pair model (VSEPR)

Question 13

How many electron domains are there?

Answer 13

4

Question 14

What are electron domains?

Answer 14

Where electrons are likely to be found

Question 15

What is the electron domain geometry of water?

Answer 15

Tetrahedral

Question 16

What is the molecular geometry of water?

Answer 16

Bent

Question 17

What is the electron domain geometry for carbon dioxide?

Answer 17

Linear shape

Question 18

What is the electron domain geometry for boron trifluoride (BF3)?

Answer 18

Trigonal planar

Question 19

What is the electron domain geometry for methane?

Answer 19

Tetrahedral

Question 20

What is lattice energy?

Answer 20

A measure of the stabilisation caused by oppositely charged ions forming a solid lattice

Question 21

What do polar covalent bonds result in?

Answer 21

A dipole

Question 22

What is electronegativity?

Answer 22

The ability of an atom in a molecule to attract electrons to itself

Question 23

Why is electronegativity so important?

Answer 23

Intermolecular electrostatic interactions means water is liquid at room temperature

Question 24

What is valence bond theory

Answer 24

• When a valence atomic orbital of one atom merges with that of another atom
• Orbitals overlap

Question 25

What does Lewis theory state?

Answer 25

That covalent bonding occurs when atoms share electrons, which concentrates the electron density between the nuclei

Question 26

What are sigma bonds?

Answer 26

Covalent bonds in which the electron density is concentrated symmetrically about the internuclear axis

Question 27

What are pi bonds?

Answer 27

Bonds that form as a result of sideways overlap of 2p orbitals, in which the overlap regions lie above and below the internuclear axis

Question 28

Describe a sp hybrid orbital

Answer 28

- 2 lobes - One is lever than the other - Identical in shape - Opposite direction

Question 29

Which bond has lower energy levels; sigma or pi?

Answer 29

Sigma

Question 30

Why do orbitals hybridise?

Answer 30

- The large lobe of hybrid orbitals can be better directed at other atoms than unhybridised atomic orbitals - They overlap more strongly, resulting in stronger bonds

Question 31

What is the uncertainty principle?

Answer 31

Impossible to say where an electron is at any given time

Question 32

What is a lone pair?

Answer 32

A pair of electrons in a fully occupied orbital

Question 33

Where do covalent bonds form?

Answer 33

Between 2 non metals