Atomic Structure and the Periodic Table

Question 1

Structure of the Nucleus

Answer 1

• In the centre of the atom
• Contains protons and neutrons
• Positively charged because of protons
• Has a radius of 1x10-14

Question 2

Electrons

Answer 2

• Orbit the nucleus in shells
• Negatively charged
• Volume of orbit determines size of the atom
• Have a very small mass

Question 3

Proton Relative Mass and Charge

Answer 3

• Relative Mass: 1
• Charge: +1

Question 4

Neutron Relative Mass and Charge

Answer 4

• Relative Mass: 1
• Charge: 0

Question 5

Electron Relative Mass and Charge

Answer 5

• Relative Mass: Very Small
• Charge: -1

Question 6

Why is the overall charge of an atom 0?

Answer 6

There are an equal amount of protons and electrons in an atom so the charge cancels out

Question 7

Relative Atomic Mass Formula

Answer 7

Total mass of atoms/Total number of atoms

Question 8

Top and Bottom Numbers on Nuclear Symbol

Answer 8

• Top: Mass Number
• Bottom: Atomic Number/Proton Number

Question 9

Number of Neutrons Calculation

Answer 9

Mass Number - Atomic Number

Question 10

Solute

Answer 10

A substance that is being dissolved in a solvent

Question 11

Solvent

Answer 11

The liquid that the solute dissolves in

Question 12

Solution

Answer 12

A mixture made when a solute dissolves into a solvent.

Question 13

Simple Distillation

Answer 13

Used to separate a liquid from a solution

Question 14

Simple Distillation Method

Answer 14

• Heat flask using a bunsen burner so the liquid that is being separated evaporates
• The vapour of said liquid rises to the top of the flask and passes through the condenser
• The cold water in the condenser causes the vapour to cool and condense
• The liquid runs down the pipe and is collected in a beaker

Question 15

Fractional Distillation

Answer 15

Used to separate mixtures of liquids with different boiling points

Question 16

Fractional Distillation Method

Answer 16

• Heat flask using a bunsen burner so the liquid with the lowest boiling point condenses first
• The vapour rises through a column that is hotter at the bottom and cooler at the top
• It rises up the fractioning column, passes through the condenser and condenses
• Collect the condensed liquid
• You are left with the other liquid in the flask

Question 17

Newlands Periodic Table

Answer 17

• Ordered by atomic weight and maintained this order
• Every 8 elements had similar properties
• Didn’t work as it forced Newlands to group elements that didn’t have similar chemical properties
• Wasn’t accepted by other scientists

Question 18

Mendeleev’s Periodic Table (The table we use to this day)

Answer 18

• Ordered elements by atomic weight
• Left gaps for undiscovered elements
• Swapped the order of some elements based on if their properties matched better elsewhere
• Elements in groups had similar chemical properties
• Accepted by other scientists when newly discovered elements were found to fit Mendeleev’s system

Question 19

Why do metals form positive ions?

Answer 19

• They don’t have many electrons in their outer shells
• The outer electron can be lost more easily as it would require less energy

Question 20

Why does reactivity increase down metal groups?

Answer 20

• Elements further down the table have more shells
• The outer shell would be further from the nucleus so the attraction between the 2 is weaker
• The electron is more easily lost

Question 21

Non Metals

Answer 21

Form either no ions or negative ions

Question 22

Metal Properties

Answer 22

• High melting and boiling points so are solids at room temperature
• Good conductors of heat and electricity
• Lustrous (shiny)
• Malleable
• Sonorous
• Have high densities

Question 23

Non Metal Properties

Answer 23

• Poor conductors of heat and electricity
• Appear dull
• Weak and brittle
• Low melting and boiling points so liquids and gases at room temperature
• Not sonorous
• Low densities

Question 24

Transition Metals

Answer 24

• Can form more than 1 type of ion
• Form coloured ions
• Melting points and densities are higher than group 1 metals
• Stronger and harder than group 1 metals
• Shiny when freshly cut

Question 25

Group 1 Metal Properties

Answer 25

- Reactive, soft metals - Alkali metals - Low density - More reactive than transition metals - React vigorously with water, oxygen and group 7 elements

Question 26

Group 1 Trends

Answer 26

- Reactivity increases down the group - Melting and boiling point decrease down the group - Relative atomic mass increases down the group

Question 27

Group 1 Reactions

Answer 27

- Group 1 + water --> Metal Hydroxide + Hydrogen - Group 1 + Chloride --> Metal Chloride + Salt - Group 1 + Oxygen --> Metal Oxide

Question 28

Group 7 Properties

Answer 28

- Non metals - All halogens are diatomic molecules - At room temperature, fluorine is a pale yellow gas, chlorine is a pale green gas, bromine is an orange liquid and iodine is a grey solid

Question 29

Group 7 Trends

Answer 29

- Relative atomic mass increases down the group - Melting and boiling points increase down the group - Reactivity decreases down the group

Question 30

Group 0

Answer 30

- Have full outer shells so they are unreactive - Exist as single atoms - Non-flammable - Boiling point increases down the group

Question 31

What is the limitation of a dot and cross diagram?

Answer 31

It doesn't show how the atoms are arranged in space

Question 32

What are the limitations of a ball and stick diagram?

Answer 32

- Not to scale - Doesn't give information about the forces pf attraction of the movement of electrons to form the ions