Topic 1 - Atomic Structure And The Periodic Table

Question 1

What are the three subatomic particles which make up the atom and what is their position within the atom?

Answer 1

Protons: Nucleus
Neutrons: Nucleus
Electrons: Shells

Question 2

What is the relative mass of all three subatomic particles?

Answer 2

Protons: 1
Neutrons: 1
Electrons: 1/2000

Question 3

What are the relative charges of the three subatomic particles?

Answer 3

Protons: +1
Neutrons: 0
Electrons: -1

Question 4

What is the atomic number of a element show you? (Bottom number)

Answer 4

The atomic (proton) number is the number of protons found in the nucleus. Can be used to identify the element.

Question 5

What does the mass number of an element tell you? (Top number)

Answer 5

The mass number is the total of protons and neutrons in the nucleus of an atom.

Question 6

How do you identify the number of each subatomic particle in an element from its mass and atomic number?

Answer 6

Protons: Atomic number
Neutrons: Mass number - Atomic number
Electrons: Atomic number

Question 7

What are isotopes?

Answer 7

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

Question 8

What is the definition of relative atomic mass?

Answer 8

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

Question 9

What is the definition of relative isotopic mass?

Answer 9

Is mass of an atom of an isotope compared to 1/12th of the mass of a carbon-12 atom

Question 10

What is the definition of an isotope?

Answer 10

Isotopes are atoms of an element with the same number of protons but different number of neutrons

Question 11

What is the difference between an atom and an isotopes chemical properties and why?

Answer 11

There is no difference in reactivity. Number and arrangement of electrons decide chemical properties, electron arrangement is identical in isotopes.

Question 12

What should the term ‘relative formula mass’ be applied to?

Answer 12

Compounds with giant structures

Question 13

How do you calculate relative atomic mass from relative abundance of isotopes?

Answer 13

(1) Multiple each relative isotopic mass by its abundance
(2) Divide by 100

Question 14

What is first ionisation energy?

Answer 14

The energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions

Question 15

What is successive ionisation energy?

Answer 15

The second ionisation energy is the energy needed to remove 1 electron from each atom in 1 mole of gaseous 1+ ions to form 1 mole of 2+ gaseous ions

Question 16

What are the three factors that affect ionisation energy?

Answer 16

Nuclear charge
Electron shell
Shielding

Question 17

Describe and explain the affect of nuclear charge on ionisation energy?

Answer 17

The higher the nuclear charge, the higher the ionisation energy.
The more protons there are in the nucleus, the more positively charged the nucleus is and the stronger the attraction