workbook 1

Question 1

describe the mass of the subatomic particles

Answer 1

protons and neutron are equivalent to 1.

electrons are so light they aren’t counted as anything

Question 2

describe the nucleus

Answer 2

small and dense and contains 99% of the mass

Question 3

what are the charges of the subatomic particles

Answer 3

proton: +
electron: -
neutron: neutral

Question 4

what is a nuclide

Answer 4

representation of an element

Question 5

what does the top number (A) on a nuclide represent

Answer 5

the atomic mass

Question 6

how can you calculate the atomic mass

Answer 6

protons + neutrons

Question 7

what does the bottom number (Z) represent in a nuclide

Answer 7

the number of protons

Question 8

what is an isotope

Answer 8

an element with the same number of protons to keep its identity but a different number or neutrons

Question 9

what is the bohr model

Answer 9

an early model of an atom where the electrons orbit the nucleus is specific energy levels or shells

Question 10

why do ionic compounds form

Answer 10

an atom is stable if all orbital shells are full. With a single atom this is only possible with the noble gases.
to fill shells, atoms combine to form stable outer shells

Question 11

what is an example of an ionic compound

Answer 11

Sodium and chlorine join so that sodium can give chlorine its valence electron and therefore they each have a full outer shell and are stable

Question 12

why do groups have the same amount of valence electrons

Answer 12

because they have similar chemical properties

Question 13

what is the electron configuration

Answer 13

2,8,8,18

Question 14

what are periods in a periodic table

Answer 14

the rows going across the table

Question 15

what are the groups in a periodic table

Answer 15

the columns going down

Question 16

what is group 1 in the periodic table

Answer 16

alkali metals

Question 17

what is group 2 in the periodic table

Answer 17

alkali earth metals

Question 18

what is group 17 in the periodic table

Answer 18

halogens

Question 19

what is group 18 in the periodic table

Answer 19

noble gases

Question 20

what are 6 properties of metals

Answer 20

1. good conductors
2. hard
3. malleable and ductile
4. high density
5. form positive ions
6. high melting and boiling points

Question 21

what are 5 properties of nonmetals

Answer 21

1. low conductors
2. brittle or soft
3. form negative ions
4. low density
5. low melting and boiling points

Question 22

what are the 3 trends in the periodic table

Answer 22

1. ionisation energy
2. atomic radius
3. electronegativity

Question 23

what is ionisation energy

Answer 23

the energy required to remove an electron from the outermost bracket

Question 24

what is the ionisation energy across a period

Answer 24

it increases

Question 25

what is the ionisation energy down a group

Answer 25

it decreases

Question 26

why does the ionisation energy increase across a period

Answer 26

Due to the increasing positive nuclear charge which pulls valence electrons closer to the nucleus making it harder to remove

Question 27

why does the ionisation energy decrease down a group

Answer 27

because the valence electrons are located further away from the nucleus resulting in a decrease in electrostatic attraction The other electrons are shielding outer electrons from the nuclear charge

Question 28

how do you read ionisation energies in graphs

Answer 28

In a table or graph there will be a large gap in the energy taken to remove a valence electron. The jump is a result of the outmost shell being empty and moving into the next shell closer to the nucleus. Energies before a big jump equals the number of valence electrons

Question 29

how does atomic radius change across a period

Answer 29

it decreases

Question 30

how does the atomic radius change down a group

Answer 30

it increases

Question 31

why does the atomic radius increase across a period

Answer 31

Occurs because of the increasing positive charge (extra protons) in the nucleus pulls the electrons closer and the radius decreases

Question 32

why does the atomic radius decrease down a group

Answer 32

There is a general increase due to the increase in numbers of protons, electrons and neutrons

Question 33

what is electronegativity

Answer 33

a measure of an atom's ability to attract electrons

Question 34

how does electronegativity change across a period

Answer 34

it increases

Question 35

how does electronegativity change down a group

Answer 35

it decreases

Question 36

why does the electronegativity increase across the period

Answer 36

Due to increasing number of protons to attract electrons 

Question 37

why does the electronegativity decrease down the group

Answer 37

There is an increase in electron orbits and shielding from inner electrons

Question 38

describe an emission spectra in simple terms

Answer 38

When an electron is in its ground state, it’s at its lowest energy level. If it absorbs energy (from heat or other particles), it can jump to a higher energy level — this is called the excited state. After a short time, the electron returns to its ground state and releases the extra energy as a photon. If the photon’s frequency is in the visible light range, it appears as a colored line on a black background.

Question 39

describe an absorption spectrum

Answer 39

Dark lines in an absorption spectrum are called absorption lines. They happen when light passes through a cooler gas. As white light passes through the gas, certain wavelengths are absorbed by the gas’s atoms. These are the same wavelengths the gas would give off if it were glowing. The absorbed light is scattered, so we see dark lines in those spots instead of bright ones.

Question 40

how is each element's emission unique

Answer 40

Each element has a unique emission that can be identified. They are all unique because each element has a different structural composition which affects the differences in energies between each shell.

Question 41

what is a continuous spectrum

Answer 41

a continuous spectrum contains all wavelengths of life so it appears as a rainbow. continuous spectrums are emitted from hot, dense objects like stars.

Question 42

what is a flame test

Answer 42

A flame test involves heating a sample of the substance over a flame, which causes the electrons to become excited and release energy in the form of light.

Question 43

what can a flame test be used for

Answer 43

A flame test can used to detect the presence of metal ions in a substance through the characteristic emissions of each element.

Question 44

how do you calculate relative atomic mass

Answer 44

Ar = %a x Ar(a)+ %b x Ar(b)100

Question 45

what is the formulas for percentage composition

Answer 45

% composition = mass of element/ mass of sample x 100