1.2 - Atomic Structure

Question 1

What is the relative mass of an electron?

Answer 1

1/1837

Question 2

Where are electrons found in atoms?

Answer 2

The shells of atoms

Question 3

Atomic number definition

Answer 3

The number of protons in the nucleus of an atom.

Question 4

Mass number definition

Answer 4

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

Question 5

Relative Atomic Mass (RAM) definition

Answer 5

The average (weighted mean) mass of an atom of an element relative to one-twelfth of the mass of an atom of carbon-12.

Question 6

Relative Isotopic Mass (RIM) definition

Answer 6

The mass of an atom of an isotope of an element relative to one-twelfth of the mass of an atom of carbon-12.

Question 7

Isotopes definition

Answer 7

Atoms which have the same atomic number but a different mass number (contain the same number of protons but different number of neutrons).

Question 8

Relative Molecular Mass (RMM) definition

Answer 8

The average (weighted mean) mass of a molecule relative to one-twelfth of the mass of an atom of carbon-12.

Question 9

Relative Formula Mass (RFM) definition

Answer 9

The average (weighted mean) mass of a formula unit relative to one-twelfth of an atom of carbon-12.

Question 10

What is an orbital?

Answer 10

An orbital is a region within an atom that can hold up to two electrons with opposite spins.

Question 11

How many electrons can fit in an orbital?

Answer 11

2

Question 12

How many subshells are present in the s orbital?

Answer 12

1

Question 13

How many subshells are present in the p orbital?

Answer 13

3

Question 14

How many subshells are present in the d orbital?

Answer 14

5

Question 15

How many subshells are present in the f orbital?

Answer 15

7

Question 16

How many electrons are present in the s orbital?

Answer 16

2

Question 17

How many electrons are present in the p orbital?

Answer 17

6

Question 18

How many electrons are present in the d orbital?

Answer 18

10

Question 19

How many electrons are present in the f orbital?

Answer 19

14

Question 20

What is the chronological filling of orbitals in energy levels?

Answer 20

1s
2s
2p
3s
3p
4s
3d
4p
5s

Question 21

What is Hund’s Rule?

Answer 21

Where electrons have choice between orbitals of equal energy, they will fill the orbitals singly as far as possible.

Question 22

Although the 4S orbital is filled before the 3D orbital, upon being completed the 4S level rises to a higher energy level. Therefore when electrons are being removed, they are removed from 4S (blank) 3D.

Answer 22

Before

Question 23

What is the shape of an s orbital?

Answer 23

Spherical

Question 24

What is the shape of a p orbital?

Answer 24

Dumbbell

Question 25

What group(s) in the periodic table belong to the s-block?

Answer 25

Group 1 and 2

Question 26

What group(s) in the periodic table belong to the d-block?

Answer 26

Transition metals

Question 27

What group(s) in the periodic table belong to the p-block?

Answer 27

Groups 3,4,5,6,7 and 0

Question 28

What group(s) in the periodic table belong to the f-block?

Answer 28

Lanthanum series | Actinium series

Question 29

What is meant by 's-block'?

Answer 29

The outer sub-shell to be filled is an s sub-shell

Question 30

What is meant by 'p-block'?

Answer 30

The outer sub-shell to be filled is a p sub-shell

Question 31

What is meant by 'd-block'?

Answer 31

The outer sub-shell to be filled is a d sub-shell

Question 32

First ionisation energy definition

Answer 32

The energy required to convert one mole of gaseous atoms into one mole of gaseous ions with a single positive charge.

Question 33

Second ionisation energy definition

Answer 33

The energy required to convert one mole of gaseous ions with a single positive charge into one mole of gaseous ions with a double positive charge.

Question 34

Form an equation for the first ionisation energy of an element X.

Answer 34

X(g) -----> X+(g) + e-

Question 35

Form an equation for the second ionisation energy of an ion X+.

Answer 35

X+(g) -----> X2+(g) + e-

Question 36

What factors affect the size of ionisation energy?

Answer 36

* Nuclear charge * Distance of the electron from the nucleus (atomic radius) * Shielding effect of the inner electrons * Stability of filled and half-filled subshells

Question 37

What is the trend in ionisation energy across a period?

Answer 37

General trend shows an increase in ionisation energies across a period. Due to: • Increase in nuclear charge • Decrease in atomic radius (as the electrons are pulled closer) • Same number of shielding electrons (although the number of electrons increase they are only being added to the same energy level).

Question 38

What is the trend in ionisation energy down a group?

Answer 38

Ionisation energy decreases as you go down a group. This is due to: • Increase in atomic radius • Better shielding from inner radius

Question 39

Third Ionisation Energy Definition

Answer 39

The energy required to convert one mole of gaseous ions with a double positive charge into one mole of gaseous with a triple positive charge.