Chapter 2

Question 1

Atom

Answer 1

A particle that consists of a nucleus of protons and neutrons surrounded by electrons.

The basic building block of all matter.

Question 2

Proton

Answer 2

A subatomic particle within the nucleus of an atom.
Charge: +1
Mass: 1amu

Question 3

Neutron

Answer 3

A subatomic particle within the nucleus of an atom.
Charge: 0
Mass: 1amu

Question 4

Electron

Answer 4

A subatomic particle that orbits the nucleus of an atom.
Charge: -1
Mass: ~0

Question 5

Nuclear Symbol

Answer 5

X = The atomic symbol
Z = Mass (# of protons + neutrons)
A = Atomic number (# of protons)

Question 6

Metals

Answer 6

Left side of the periodic table

Highly reactive because they have many free electrons.

Question 7

Ions

Answer 7

An atom or molecule that has a net electrical charge due to an imbalance of protons vs electrons.

Question 8

Cations

Answer 8

Positive ions

Group 1A + 2A

Question 9

Anions

Answer 9

Negative ions

Non-metals
Group 6A, 7A

Question 10

Groups

Answer 10

Vertical columns of the periodic table that share chemical and physical properties

Question 11

Periods

Answer 11

Horizontal rows of the periodic table that denote the number of electron orbitals.

Question 12

Alkali Metals

Answer 12

Group 1A (Except Hydrogen)

Question 13

Alkali Earth Metals

Answer 13

Group 2A

Question 14

Transition Metals

Answer 14

Group 1B - 8B

Question 15

Which group is most stable?

Answer 15

Group 8A

This group has a full valence shell, they will not gain or lose electrons easily.

Question 15

Halogens

Answer 15

Group 7A

Question 16

Which group is least stable?

Answer 16

Group 1A

This group only has one valence electron, which means they are likely to lose it.

Question 17

Group Valence Electrons

Answer 17

Each group denotes the number of valence electrons. This is why group 8A is most stable, because they have a complete valence shell of 8 electrons.

Question 18

Groups with +1 charge

Answer 18

Group 1A

Question 19

Groups with +2 charge

Answer 19

Group 2A

Question 20

Groups with +3 charge

Answer 20

Group 3A

Question 21

Groups with -1 charge

Answer 21

Group 7A

Question 22

Groups with -2 charge

Answer 22

Group 6A

Question 23

Groups with -3 Charge

Answer 23

Group 5A

Question 24

Groups with -3 Charge

Answer 24

Group 5A

Question 25

Groups with 1 valence electron

Answer 25

Subgroup 1A

Question 26

Groups with 2 valence electrons

Answer 26

Group 2A + All B Groups

Question 27

Groups with 3 valence electrons

Answer 27

Group 3A

Question 28

Groups with 4 valence electrons

Answer 28

Group 4A

Question 29

Groups with 5 valence electrons

Answer 29

Group 5A

Question 30

Groups with 6 valence electrons

Answer 30

Group 6A

Question 31

Groups with 7 valence electrons

Answer 31

Group 7A

Question 32

Groups with 8 valence electrons

Answer 32

Group 8A

Question 33

Isotope

Answer 33

An element with a different number of neutrons than usual.

Isotopes are identified by their mass number.

Ne-21 = 10 protons + 11 neutrons

Ne-22 = 10 protons + 12 neutrons

Question 34

Compound

Answer 34

Composed of two or more different elements and always contains exactly the same relative masses of those elements.

Question 35

Chemical formula

Answer 35

Expresses the types of atoms and number of each type in a given compound.

For any formula containing carbon the order is carbon first, hydrogen second, and the rest in alphabetical order.

For non-carbon formulas, all elements are listed in alphabetical order.

Question 36

Ionic compound formula

Answer 36

Ionic compounds are electrically neutral

The cation element component comes first, with the anion element component after.
Mg²⁺ + Cl⁻ + Cl⁻ = MgCl₂

Question 37

Dalton’s Atomic Theory

Answer 37

1. Elements are composed of atoms
2. All atoms of an element are identical
3. Atoms combine to form compounds
4. Chemical reactions are rearrangements of atoms

Question 38

Thompson’s Theory

Answer 38

• Proved the existence of electrons
• Speculated the existence of positive charge as atoms are of neutral charge
• Electrons are negative charges held within a positively charged sphere.

Question 39

Rutherford’s Interpretation

Answer 39

1. Atoms contain a dense center called the nucleus
2. Protons are positively charged particles within the nucleus
3. Equal number of protons and electrons
4. Electrons move around in the empty space of the atom surrounding the nucleus.
5. The nucleus has essentially the entire mass of the atom
6. Neutrons are of neutral charge and within the nucleus.

Question 40

Diatomic Elements

Answer 40

Rule of 7:
* Hydrogen
* Start at the element with the atomic number 7 (Nitrogen)
* Include the elements 3 across up to group 7A, 4 down to “trace” the number seven.

• Hydrogen (H₂)
• Nitrogen (N₂)
• Oxygen (O₂)
• Fluorine (F₂)
• Chlorine (Cl₂)
• Bromine (Br₂)
• Iodine (I₂)

Question 41

Formula To Name: Ionic Compounds

Answer 41

Type I: Ions with one possible charge
Cation name + Anion name + ide
Example: CaS is Calcium Sulfide

Type II: Ions with more than one possible charge. These are the transition metals (groups 1B-8B). Determine the cation charge by finding the anion charge that balances it.
Cation name + Cation Charge + Anion name + ide
Example: CuCl is Copper (I) Chloride
Cl has a charge of -1 so the copper must have a charge of +1 to balance this.

Question 42

Polyatomic Ions

Answer 42

Groups of atoms with a net charge.