T1: Atomic Structure and The Periodic Table

Question 1

Relative mass of a proton

Answer 1

1

Question 2

Relative mass of a neutron

Answer 2

1

Question 3

Relative mass of a electron

Answer 3

1/1835

Question 4

Relative charge of a proton

Answer 4

+1

Question 5

Relative charge of a neutron

Answer 5

0

Question 6

Relative charge of an electron

Answer 6

-1

Question 7

Isotopes

Answer 7

different atoms of the same element with the same proton number but different neutron number

Question 8

Relative Atomic Mass

Answer 8

The weighted mean mass of an atom relative to 1/12th the mass of carbon-12

Question 9

Relative Isotopic Mass

Answer 9

the weighted mean mass of an isotope relative to 1/12th the mass of carbon-12

Question 10

What are the subshells?

Answer 10

s,p,d or f

Question 11

How many orbitals does the ‘s’ subshell have?

Answer 11

1 orbital

Question 12

How many electrons in the ‘s’ subshell?

Answer 12

2 electrons

Question 13

How many orbitals does the ‘p’ subshell have?

Answer 13

3 orbitals

Question 14

How many electrons in the ‘p’ subshell?

Answer 14

6 electrons

Question 15

How many orbitals does the ‘d’ subshell have?

Answer 15

5 orbitals

Question 16

How many electrons in the ‘d’ subshell?

Answer 16

10 electrons

Question 17

How many orbitals does the ‘f’ subshell have?

Answer 17

7 orbitals

Question 18

How many electrons in the ‘f’ subshell?

Answer 18

14 electrons

Question 19

Describe the first electron shell in terms of orbitals and electrons

Answer 19

1s
2 electrons

Question 20

Describe the second shell in terms of orbitals and electrons

Answer 20

2s 2p
8 electrons

Question 21

Describe the third shell in terms of orbitals and electrons

Answer 21

3s 3p 3d
18 electrons

Question 22

What shape is the s orbital?

Answer 22

spherical

Question 23

What shape is the p orbital?

Answer 23

8 shape in all 3 directions x,y and z

Question 24

List all the subshells

Answer 24

1s 2s 2p 3s 3p 4s 3d

Question 25

Define 1st ionisation energy

Answer 25

Minimum amount of energy required to remove 1 mole of electrons from 1 mole of atoms to form 1 mole of gaseous 1 + ions

Question 26

How does shielding effect ionisation energy?

Answer 26

The more electron shells between the nucleus and the outer electron being removed, the weaker the attraction and so less energy is needed.

Question 27

How does nuclear charge affect ionisation energy?

Answer 27

The more protons in the nucleus, the bigger the positive charge SO the bigger the attraction between nucleus and electrons Therefore more energy is needed to remove an electron.

Question 28

How does atomic size affect ionisation energy?

Answer 28

The bigger the atom, the further away the outer electrons are from the nucleus SO the attractive force is smaller hence its easier to remove electrons

Question 29

Why do ionisation energies decrease down a group?

Answer 29

Atomic radius increases so outer electrons are further away (smaller attractive forces + a smaller ionisation energy) Shielding increases (more shells) so attractive force is smaller This offsets the increasing charge

Question 30

Why does ionisation energy increase across a period?

Answer 30

More protons (increased nuclear charge) so attractive force is larger The shielding and atomic radius are similar

Question 31

What 3 factors affect ionisation energy?

Answer 31

Nuclear charge Shielding Atomic size