Bonding

Question 1

What are the three subatomic particles?

Answer 1

Proton, neutron, electron.

Question 2

What are the charges and masses of the subatomic particles?

Answer 2

Proton: Charge +1, Mass 1
Neutron: Charge 0, Mass 1
Electron: Charge -1, Mass ~0

Question 3

Where are the subatomic particles located?

Answer 3

Protons & neutrons: Nucleus
Electrons: Electron shells

Question 4

What does the atomic number tell you?

Answer 4

The number of protons in an atom.

Question 5

What is the mass number?

Answer 5

The total number of protons and neutrons.

Question 6

What are isotopes?

Answer 6

Atoms of the same element with different numbers of neutrons.

Question 7

How do you calculate relative atomic mass (Ar)?

Answer 7

Ar = (mass1 × abundance1 + mass2 × abundance2) / total abundance

Question 8

What is an ion?

Answer 8

A charged atom (gained or lost electrons).

Question 9

Who developed the modern periodic table?

Answer 9

Dmitri Mendeleev

Question 10

How is the modern periodic table arranged?

Answer 10

By increasing atomic number.

Question 11

What do groups and periods represent?

Answer 11

Groups (columns): Number of valence electrons
Periods (rows): Number of energy levels

Question 12

What are the properties of Group 1 (alkali metals)?

Answer 12

Soft, low density
Highly reactive
Reactivity increases down the group

Question 13

What are the properties of Group 7 (halogens)?

Answer 13

Non-metals, exist as diatomic molecules
Reactivity decreases down the group

Question 14

What are the properties of Group 0 (noble gases)?

Answer 14

Unreactive (full outer shell)
Low boiling points

Question 15

How do transition metals compare to Group 1 metals?

Answer 15

Higher melting points
Stronger & harder
Less reactive

Question 16

What are the key properties of transition metals?

Answer 16

Catalysts
Multiple oxidation states
Form colored compounds

Question 17

What are the three types of chemical bonding?

Answer 17

Ionic, covalent, and metallic.

Question 18

What happens in ionic bonding?

Answer 18

Electrons are transferred from a metal to a non-metal, forming positive and negative ions.

Question 19

Why do ionic compounds have high melting points?

Answer 19

Strong electrostatic forces require a lot of energy to break.

Question 20

What happens in covalent bonding?

Answer 20

Non-metals share electrons to form strong covalent bonds.

Question 21

What happens in metallic bonding?

Answer 21

Positive metal ions are surrounded by a sea of delocalized electrons.

Question 22

Why do simple molecular substances have low melting points?

Answer 22

They have weak intermolecular forces that require little energy to break.

Question 23

Why do metals conduct electricity?

Answer 23

Delocalized electrons can move and carry charge.

Question 24

What are the properties of giant covalent structures?

Answer 24

Very high melting points
Do not conduct electricity (except graphite)

Question 25

What are the four allotropes of carbon?

Answer 25

Diamond, graphite, graphene, fullerenes.

Question 26

Why is diamond extremely hard?

Answer 26

Each carbon atom forms four strong covalent bonds in a giant lattice.

Question 27

Why does graphite conduct electricity?

Answer 27

It has delocalized electrons that can carry charge.

Question 28

What is graphene and why is it special?

Answer 28

A single layer of graphite; extremely strong and conductive.

Question 29

What are fullerenes?

Answer 29

Carbon molecules in the shape of hollow spheres or tubes.

Question 30

Why do ionic compounds only conduct electricity when molten or dissolved?

Answer 30

Ions are free to move, allowing charge to flow.

Question 31

Why is graphite slippery?

Answer 31

Layers of carbon atoms are held by weak forces, allowing them to slide.

Question 32

What is a polymer?

Answer 32

A long chain molecule made from repeating monomers.

Question 33

Why are nano-materials special?

Answer 33

They have a large surface area to volume ratio, making them highly reactive.