Chapter 2 - Atoms, Ions, and Compounds

Question 1

What are the three subatomic particles?

Answer 1

Protons, Neutrons, and Electrons

Question 2

Subatomic particle

Abbreviation

Relative Charge

Relative Mass

Answer 2

Proton, Nuetron, Electron

p+, n, e-

1+, 0, -1

1, 1, 1/1836

Question 3

What is the atomic number?

Answer 3

The amount of protons an atom has.

Question 4

What is the mass number?

Answer 4

The amount of protons and neutrons an atom has.

Question 5

How would you calculate the amount of neutrons in an atom?

Answer 5

Mass number - atomic number

Question 6

What is the equation for % abundance?

Answer 6

% abundance = (mr 1 x %1) + (mr 2 x %2), etc. / 100

Question 7

State the definition of an ion.

Answer 7

An atom is an ion that has either lost or gained electrons.

Question 8

State the definition of an isotope.

Answer 8

Isotopes are different versions of an atoms with the same number of protons and electrons but a different number of neutrons.

Question 9

What is the general equation for moles?

Answer 9

moles = mass/Mr or n = m/Mr

Question 10

What is positive ion?

Answer 10

It is a cation and has lost electrons.

Question 11

What is a negative ion?

Answer 11

It is a negative ion and has gained electrons.

Question 12

Why do ions generally form?

Answer 12

This is because generally will lose or gain electrons to form a stable electronic configuration similar to the noble gases.

Question 13

List some common examples of ions.

Answer 13

Ammonium ion: NH + => 1+

Hydroxide: OH - => 1-
Nitrate: NO3 - => 1-
Nitrite: NO2 - => 1-
Hydrogencarbonate: HCO3 - => 1-
Manganate (VII) (permanganate):
MnO4 - => 1-

Carbonate: CO3 2- => 2-
Sulfate: SO4 2- => 2-
Sulfite: SO3 2- => 2-
Dichromate: Cr2O7 2- => 2-

Phosphate: PO4 3- => 3-

Question 14

State the definition for relative atomic mass.

Answer 14

The weighted mean mass of an atom of an element for 1/12th of a carbon-12 atom.

Question 15

State the definition for relative isotopic mass.

Answer 15

The weighted mean mass of an isotope relative to 1/12th of a carbon-12 atom.

Question 16

State the definition for relative formula mass.

Answer 16

The weight mean mass of a formula unit of a compound relative to 1/12th of a carbon-12 atom.

Question 17

State the common charges of formed in the periodic table.

Answer 17

Group 1 will form a 1+ charge.
Group 2 will form a 2+ charge.
Group 3 will form a 3+ charge.

Group 4 can vary in the charge formed.

Group 5 will form a 3- charge.
Group 6 will form a 2- charge.
Group 7 will form a 1- charge.

Transition metals are able to form multiple charges.
Noble gases will generally not form a charge since the are normally unreactive.

Question 17

State the definition for relative molecular mass.

Answer 17

The weighted mean mass of a molecule of a compound relative to 1/12th of a carbon-12 atom.