Topic 1 - Atomic Structure And The Periodic Table

Question 1

Mass and charge of the particles

Answer 1

Proton, 1, +1
Neutron, 1, 0
Electron, very small (1/1838), -1

Question 2

What makes an ion different to an atom

Answer 2

The number of electrons are different to the number of protons

Question 3

How big is an atom

Answer 3

0.1 nanometers

Question 4

What determines the size of the atom?

Answer 4

The volume of orbit of the electrons

Question 5

What is an element

Answer 5

This is a substance made up of atoms that all have the same number of protons in their nucleus

Question 6

Out of the three particles, which one determines what atom it is?

Answer 6

The number of protons in the nucleus

If the neutrons or electron number changes, it is still the same atom

Question 7

What makes an isotope?

What changes in the atomic and mass numbers?

Answer 7

Different forms of the same element with a different number of electrons

Same atomic number, different mass number

Question 8

Name two common isotopes

Answer 8

Carbon - 12

Carbon - 13

Question 9

Why is the relative atom mass used instead of the mass number when referring to an element as a whole

Answer 9

Because many elements can exist as a number of different isotopes

Question 10

What is the relative atomic mass formula

Answer 10

Relative atomic mass =

Sum of (isotope abundance X isotope mass number)
____________________________________
Sum of abundance of all isotopes

Question 11

When is a compound formed

Answer 11

When elements react with other elements

Question 12

What is a compound

Answer 12

A substance formed from 2 or more elements

Question 13

What holds compounds together

Answer 13

Chemical bonds

Question 14

What are the three ways bonds are made

Answer 14

By giving away, taking or sharing electrons

Question 15

What is required in ionic, covalent and metallic bonding

Metals and non metals

Answer 15

Ionic: metal + non-metal
Covalent: non-metal + non-metal
Metallic: metal + metal

Question 16

What happens in ionic bonding (electron wise)

Answer 16

Metal atoms lose electrons and non metals gain electrons

Question 17

Why are there strong bonds in ionic bonding?

Answer 17

Because the opposite charges (the positive of the metal and the negative of the non-metal) means they are strongly attracted to each other.

Question 18

What happens in covalent bonding (electron wise)

Answer 18

The electrons are shared

Question 19

What are the ways of showing chemical equations

Answer 19

Word equations
Symbol equations (need to be balanced)

Question 20

Whats the difference between a mixture and a compound

Answer 20

Mixtures are not chemically bounded

Question 21

What is the goal of atoms

Answer 21

To have full shells (also known as energy levels)

Question 22

What similarities do the elements in a period have

Answer 22

The same number of outer shells

Question 23

What similarities do the elements in a group have

Answer 23

They have the same amount electrons on their outer shell

GROUP 0 are an exception to this (Helium has two and Neon has 8)

Question 24

What is the difference between groups and periods have in the periodic table

Answer 24

Groups are vertically down

Columns are horizontal

Question 25

Why do non metals have a hard time forming positive ions

Answer 25

They are generally near the top: So they are closer to the nucleus, and therefore feel a stronger attraction and far right of the periodic table: So the have more electrons to lose (e.g) group 7 have to lose 7

Question 26

Different physical properties of metals and non metals

Answer 26

``` Metals: Metallic bonding Strong Good at conducting heat and electricity Have high boiling and melting points ``` Non-metals: Dull looking Aren't always solid at room temperatures Don't generally conduct heat or electricity Have a lower density

Question 27

Factors of the group 1 metals

Answer 27

Also known as the Alkali metals One electron so very reactive Soft and low density Lower melting and boiling points the lower you go

Question 28

Reactivity of group 1

Answer 28

More reactive the further down you go | The outer electron is easier to lose the further down you go as it is further away from the attraction o pf the nucleus

Question 29

What happens to group 1 metals when the react with A)water B)chlorine C)oxygen

Answer 29

``` A)produce hydrogen gas They react vigorously Lithium, Sodium and Potassium float, move and fizz Also makes the water alkaline B)produce salt called METAL CHLORIDE Again react vigorously C) from a METAL OXIDE ```

Question 30

Factors of group 7

Answer 30

The halogens Non metals Must be in pairs of 2 Most poisonous Higher boiling and melting points the further you go down

Question 31

Reactivity of group 7

Answer 31

As you go down, it gets less reactive | This is because its harder to gain an extra electron as it is further from the attraction of the nucleus

Question 32

What happens when two halogens (elements in group 7) react

Answer 32

The more reactive halogen will displace (remove) the less reactive one. Eg chlorine will displace iodine Eg Cl2 + 2Kl = I2 + 2KCL

Question 33

What must all gases except for the noble gases do and why

Answer 33

They must all travel in pairs as this gives them a full outer shell Eg Oxygen E.g O2

Question 34

Features of the noble gases (group 0)

Answer 34

All colourless gas at room temperature Non-flammable Full outer shells already

Question 35

What are the pattern of boiling points for group 7/the noble gases

Answer 35

The boiling point increases as you move down | This is because there are more electrons, so more bonds are needed to be broken

Question 36

How would you guess what state a noble gas is in | Eg Neon is a gas at 25 degrees. Predict what state helium is at this temperature

Answer 36

The further down you go, the higher the boiling point becomes As neon is further down the group than helium, it must have a higher boiling point Therefore, helium would be a gas at 25 degrees