Atomic Structue/ Periodic Table/ Test 1 revision

Question 1

Define atom

Answer 1

• Smallest unit of matter
• made up of 3 subatomic particles : protons, neutrons, electrons
• Atoms combine to form molecules and make up everything

Question 2

Charge of protons

Answer 2

positive
- relative charge of +1`

Question 3

charge of neutron

Answer 3

neutral

Question 4

charge of electron

Answer 4

negative

Question 5

what makes up the nucleus?

Answer 5

protons and neutrons

Question 6

Where are the electrons located?

Answer 6

Orbits around the nucleus in shells/ energy levels/ orbits

Question 7

what does the atomic number tell?

Answer 7

Number of protons and also the same number of electrons

Question 8

what does atomic mass number tell?

Answer 8

number of protons + neutrons

Question 9

How to differentiate between atomic and mass number?

Answer 9

mass number:
- often decimals
- often the bigger number

atomic number:
- whole number
- often smaller

Question 10

Why is the atomic mass a decimal number?

Answer 10

Decimal number as it is the average mass of the atom’s isotopes, factoring the percentage abundance of its isotopes

Question 11

Isotope definition

Answer 11

Variations of an atom, with the same number of protons but different number of neutrons.
- Isotopes have identical chemical properties due to same number electrons.

Question 12

Examples of isotopes:

Answer 12

H-1, H-2, H-3
C-14, C-15, C-16

Question 13

Define Ion

Answer 13

Charged atom (positive or negative) through the lost or gainage of electrons through ionic bonding.

Question 14

name of positive changed ion?

Answer 14

Cation

Question 15

name of negative charged ion

Answer 15

anion

Question 16

charge of ion when an electron is lost

Answer 16

positive as it lost a negative charge

Question 17

charge of ion when gained an electron

Answer 17

negative charge as it gained a negative charge

Question 18

Define electronegativity

Answer 18

How strongly/ closely an atom holds onto its electrons

Question 19

Define ionisation energy

Answer 19

The energy required to remove an atom’s electrons

Question 20

how does electronegativity and ionisation energy connect?

Answer 20

The higher the electronegativity/ the more electronegative, the higher the ionisation energy/ the more ionisation energy

Question 21

Define atomic radii

Answer 21

How far away valence electrons are from the nucleus

Question 22

As you go across periodic table, describe the electronegativity trend

Answer 22

As you go across, the electronegativity increases. Due to the increased number in protons which attracts the valence electrons more

Question 23

Describe electronegativity trend as you go down a group

Answer 23

The electronegativity decreases as each period it goes down, the more shells are added, therefore, there is a weaker attraction between the valence electrons and the nucleus due to increased atomic radii.

Question 24

Describe ionisation trend going across table

Answer 24

Ionisation energy increases due to increased electronegativity

Question 25

Describe ionisation trend as you go down a group

Answer 25

Ionisation energy decreases as electronegativity deacreases

Question 26

Describe atomic radii across periodic table

Answer 26

Atomic radii decreases due to increased number of protons which make the electrons more attracted to the nucleus, therefore, a shorter distance between them and overall atomic radii

Question 27

Describe atomic radii trend as you go down a group

Answer 27

Atomic radii increases as more electron shells are being added since electrons like to repel eachother due to same charge the valence electrons are a greater distance from the nucleus

Question 28

Describe metallic character trend across table

Answer 28

Metallic character decreases as it moves closer to the non-metals but also posesses less metallic characteristics.

Question 29

Describe metallic character going down a group

Answer 29

The metallic character increases as atomic radii increases, therefore, lower electronegativity.

Question 30

describe non-metallic character trend as you go across

Answer 30

non-metallic character increases as electronegativity increases, where non-metals are located, posesses non-metallic characteristics

Question 31

describe non-metallic character as you go down a group

Answer 31

non-metallic character decreases as the electronegativity decreases