2.1.1 and 2.1.2 - Atomic Structure

Question 1

What are the 3 subatomic particles?

Answer 1

Protons
Neutrons
Electrons

Question 2

What are the positions in the atom, of the subatomic particles?

Answer 2

Proton = Nucleus
Neutron = Nucleus
Electron = Orbitals

Question 3

What are the relative charges of the subatomic particles?

Answer 3

Proton = +1
Neutron = 0
Electron = -1

Question 4

What are the relative masses of the subatomic particles?

Answer 4

Proton = 1
Neutron = 1
Electron = 1/1800

Question 5

What is the atomic number (Z) equal to?

Answer 5

The atomic number, Z, is the number of protons in the nucleus.

Question 6

What is the mass number (A) equal to?

Answer 6

The mass number, A, is the total number of protons and neutrons in the atom.

Question 7

How is the number of neutrons calculated?

Answer 7

Mass of neutrons = A - Z

Question 8

What are isotopes?

Answer 8

Isotopes are atoms of the same element with the same number of protons, but with a different number of neutrons.

Question 9

What are the characteristics of isotopes?

Answer 9

Isotopes have similar chemical properties because they have the same electronic structure. They may have slightly varying physical properties because they have different masses.

Question 10

What is the relative isotopic mass?

Answer 10

Relative isotopic mass is the mass of one isotope compared to one twelfth of the mass of one atom of carbon-12.

Question 11

What is the relative atomic mass?

Answer 11

Relative atomic mass is the weighted mean mass of one atom compared to one twelfth of the mass of one atom of carbon-12.

Question 12

What is the relative molecular mass?

Answer 12

Relative molecular mass is the average mass of a molecule compared to one twelfth of the mass of one atom of carbon-12.

Question 13

What is the relative atomic mass of an element?

Answer 13

the average mass of an element’s atoms compared to one-twelfth the mass of a carbon-12 atom

Question 14

What is the formula for the Relative Atomic Mass calculated?

Answer 14

∑(isotopic mass x relative abundance) / total relative abundance

Question 15

What are the most important +1 ions to know? (4)

Answer 15

Hydrogen
Silver
Gold
Ammonium

Question 16

What are the most important +2 ions to know? (5)

Answer 16

Zinc
Copper (II)
Iron (II)
Tin
Lead

Question 17

What is the most important +3 ion to know?

Answer 17

Iron (III)

Question 18

What is the most important -3 ion to know?

Answer 18

Phosphate (PO4(3-))

Question 19

What are the most important -2 ions to know? (2)

Answer 19

Carbonate (CO3(2-))
Sulphate (SO4(2-))

Question 20

How do you work out the formula of lithium sulfate?

Answer 20

1. Identify the ionic charges of the two ions:
   * Lithium is in group 1, so has a +1 charge (Li+)
   * Sulphate has a 2- charge, SO4(2-)
2. Combine the two ions together to get a neutral compounds
3. We need 2 Li+ ions and 1 SO4(2-) ions, so therefore the formula is: Li2SO4

Question 21

How do you work out the formula of calcium phosphate?

Answer 21

1. Identify the ionic charges of the two ions:
   * Calcium is in group 2, so has a 2+ charge (Ca2+)
   * Phosphate has a -3 charge, PO4(3-)
2. Combine the ions together to get a neutral compound.
3. Therefore, the formula is: Ca3(PO4)2

Question 22

What is a spectator ion?

Answer 22

Spectator ions are ions that are:
* not changing state
* not changing oxidation number

Question 23

When writing spectator ions, what are the three steps to follow?

Answer 23

1. Take full equation
2. Separate (aq) solutions into ions
3. Cancel out spectator ions leaving ionic equation.