UNIT 1: CHAPTER 2 TEST

Question 1

Binary Compounds

Answer 1

Compound with 2 elements

Question 2

How do ionic bonds form

Answer 2

Because of an attraction between a cation and an anion. They are held together by electrostatic force

Question 3

Properties of IONIC compounds

Answer 3

Solids at room temp

Hard/Brittle

High melting/boiling points

Conduct electricity when dissolved in water

Question 4

Structure of ionic compounds (Crystal lattice)

Answer 4

Crystal Lattice: rigid arrangement of ions in an ionic substance

• High melting and boiling points: strong electrostatic forces between ions
• Hard: bonds resist being stretched
• Brittle: offset of crystal lattice = repulsion between like charges

Shape is determined by the size of the ions that make up the compound and the strength with which they attract each other

Question 5

Electrolytic

Answer 5

Soluble in water, and conduct electricity

Question 6

Hydrate

Answer 6

Ionic compound that contains water as part of its crystal structure

The water inside hydrate is called water of hydration

When the water is removed = anhydrous

Question 7

Identifying acids

Answer 7

They are all AQUEOUS (dissolved in water)

They all have HYDROGEN IN THEM

Question 8

NAMING ACIDS

Answer 8

ATE=IC
ITE=OUS

Question 9

Covalent bond

Answer 9

A bond that causes from a pair of electrons from different atoms sharing

Question 10

Molecular element vs compound

Answer 10

A molecular element consists of multiple atoms of the same type chemically bonded together. A molecular compound consists of atoms of different elements chemically bonded together

Question 11

Properties of MOLECULAR compounds

Answer 11

Can be solid, liquid, or gas at room temp

Low melting/boiling point

Poor electrical conductivity

Question 12

Bonding capacity

Answer 12

The number of covalent bonds an atom can make

Question 13

Bonding electron

Answer 13

An electron in the valence shell of an atom, that can form a covalent bond with another atom

Question 14

Lone pair

Answer 14

A pair of electrons that is not involved in covalent bonding

Question 15

Electronegativity (EN)

Answer 15

The ability of an atom (when bonded) to attract bonding electrons to itself

Question 16

What are the trends in EN from left to right and from top to bottom? Why?

Answer 16

• Electronegativity and atomic radius size are inversely
  related to one another:
• Therefore, as the atomic radius decreases, the
  electronegativity value increases for that element, because valence electrons are closer to the nucleus so there’s a stronger attraction force

Question 17

Non-polar
Polar
ionic

Answer 17

0 - 0.4
0.4 - 1.7
above 1.7

Question 18

VSEPR

Answer 18

Valence Shell Electron Pair Repulsion

theory says that e- repel each other as far away as possible

HELPS predict the 3D geometry of a molecule

MOLECULAR SHAPE: There is Tetrahedral, trigonal pyramid, and linear

Question 19

Octet rule

Answer 19

When bonds form between atoms, the atoms gain, lose, or share electrons in such a way that they create a filled outer shell containing eight electrons

Question 20

Carbonate

Answer 20

CO 3 -

Question 21

Hydrogen carbonate/bicarbonate

Answer 21

HCO 3 -

Question 22

Iodate

Answer 22

IO 3 -

Question 23

Hydrogen sulfate/bisulfate

Answer 23

HSO 4 -

Question 24

Sulfate

Answer 24

SO4 2-

Question 25

Phosphate

Answer 25

PO4 3-

Question 26

Nitrate

Answer 26

NO 3 -

Question 27

Chlorate

Answer 27

ClO 3 -

Question 28

Acetate

Answer 28

C2 H3 O2 -

Question 29

FOUR TYPES OF SHAPES

Answer 29

Lewis structure Ball-and-stick Structural formula Space-filling model

Question 30

IntERmolecular forces vs intramolecular bonds

Answer 30

Intramolecular forces are the forces that hold atoms together within a molecule. IntERmolecular forces are forces that exist between molecules.

Question 31

Types of intermolecular forces

Answer 31

London dispersion Diplole-dipole (Hydrogen bonding) Stronger IMF are harder to separate when boiling

Question 32

LONDON DISPERSION

Answer 32

Weak Temporary induced dipoles (imbalance of e-) The larger the entity, the greater the London forces will be

Question 33

Why does boiling point increase for Halogens and Noble gases down the group

Answer 33

Larger atoms means more e- shells which means more opportunities for partial charges which means more LDF

Question 34

Why does boiling point increase for larger-non polar compounds

Answer 34

Longer molecules have more spaces for LDF = higher boiling point

Question 35

Dipole-dipole

Answer 35

Polar molecules ONLY Stronger than LDF (cuz of partial charges on neighbouring molecules)

Question 36

Hydrogen "Bonds"

Answer 36

Stronger type of dipole-dipole. MUST have an H bonded to N, O, F

Question 37

Properties of WATER

Answer 37

-High melting/boiling point -Low density of ice -High surface tension -High specific heat capacity