C4

Front 1

Where is the nucleus

Back 1

in the middle of the atom

Front 2

what do nucleus contain

Back 2

protons and neutrons

Front 3

what charge do nucleus have and why

Back 3

positive because of protons

Front 4

describe the size of nucleus

Back 4

whole mass of atom is concentrated in nucleus

size wise its tiny compared to rest of atoms

Front 5

where are electrons

Back 5

move around the nucleus

Front 6

describe the charge of nucleus

Back 6

negatively charged

Front 7

describe the size of electrons

Back 7

tiny but cover a lot of space

Front 8

what determines how big the atom is

Back 8

the volume of their orbits

Front 9

describe the mass of electrons

Back 9

no mass

Front 10

what are protons weight and how are they charged

Back 10

heavy negatively charged

Front 11

what are neutrons weight and how are they charged

Back 11

heavy and neutral

Front 12

what are electrons weight and how are they charged

Back 12

tiny and negatively charged

Front 13

how are neutral atoms charged

Back 13

no charge overall

Front 14

how is the charge of the electron in regard to protons

Back 14

charge of the electron is the same size as the charge of protons but opposite

Front 15

how are he numbers of protons and electrons in a neutral atom?

Back 15

number of protons=number of elecrons

Front 16

what happens if electrons are added or removed

Back 16

the atom becomes charged and is an ion

Front 17

what in an atom decides what element it is

Back 17

the number of protons

Front 18

How are atoms of the same element

Back 18

they all have the same number of protons

Front 19

how are atoms of different element

Back 19

have different number of protons

Front 20

why do elements have different properties from eachoher

Back 20

due to their differences in atomic structure

Front 21

what does (s) (l) (g) (aq) stand for

Back 21

solid liquid gas dissolves in water

Front 22

when heated what does lithium potassium and sodium produce

Back 22

red flame

lilac flame

orange flame

Front 23

when heated what do the atoms in electrons release

Back 23

energy as light

Front 24

why do different elements emit different wave lengths

Back 24

each element has a different electron arrangement

Front 25

what can line spectrums be used to identify

Back 25

elements

Front 26

how do you produce line spectrum

Back 26

spectroscopy

Front 27

How did Dobereiner start to put list of elements into groups

Back 27

based on their chemical properties into groups of three

Front 28

Why was newlands work criticised

Back 28

he mixed up metals and non metals

he didnt leave any gaps for elements that had not been discovered yet

Front 29

how was the periodic table formed

Back 29

mendleeve put elements in form of atomic mass and left gaps for atoms that hadnt been discovered yet

Front 30

How do you identify the number of electrons in the outer shell on periodic table

Back 30

the group number

but group 0 have 8 electrons

Front 31

How can you predict reactivity in periodic table

Back 31

group 1 elements react more rigorously as you go down but in group 7 reactivity decreases

Front 32

how can you calculate the number of neurons

Back 32

relative atomic mass- neutrons

Front 33

What do electrons do?

Back 33

they occupy shells sometimes called energy levels

Front 34

what shells get filled first

Back 34

the lowest

Front 35

how many electrons are allowed in the 1st shell

Back 35

2

Front 36

how many electrons are allowed in the second shell

Back 36

8

Front 37

how many electrons are allowed in the third shell

Back 37

8

Front 38

what happens in atoms when the outer shell is not full

Back 38

makes the atom want to react

Front 39

what does an elements electron arrangement determine

Back 39

its chemical properties

Front 40

how do you work out electron configuration

Back 40

you find out how many protons it has then separate those into shells

Front 41

what happens when atoms lose or gain electrons

Back 41

they form charged particles called ions

Front 42

how can atoms be made

Back 42

from single atoms or groups of atoms

Front 43

why do atoms lose or gain electrons

Back 43

theyre trying to gain a full outer shell

Front 44

How are the atoms in group1 electrons

Back 44

have just one electron in their outer shell and they want to get rid of it because theyll have full shells left as they like

Front 45

what happens when group 1 atoms lose an electorn

Back 45

they form positive ions

Front 46

how are group 7 outer shell

Back 46

nearly full

Front 47

what do group 7 want for their shells

Back 47

to gain electrons to fill their shells

Front 48

what happens when group 7 elements gain an electron

Back 48

they form negative ions

Front 49

How are oppositely charged ions to eachother

Back 49

strongly attracted they join with passing ions that have an opposite charge and form an ionic bond

Front 50

how are group 1 and group 7 elements held together by

Back 50

ionic bonds and theyre ionic compounds

Front 51

what are solid ionic compounds made up of

Back 51

made up of a giant lattice of ions each lattice forms a single crystal

Front 52

what happens when ionic compounds become molten or dissolve

Back 52

they can conduct electricity because the ions are able to move

Front 53

what is the evidence that molten compounds can conduct electricity

Back 53

theyre made up of ions

Front 54

what do the compounds int he total charge always add up to

Back 54

0

Front 55

what do group 1 metals include

Back 55

lithium,sodium,potassium

Front 56

how many outer shell electrons do group 1 have

Back 56

one outer shell making them very reactive and have similar properties

Front 57

how are alkali metals when cut and react in the air

Back 57

very shiny when freshly cut

quickly react with oxygen in air and tarnish

Front 58

what happens as you go down group 1

Back 58

alkali metals become more reactive

because outer electron becomes easily lost as it is away from nucleus

Front 59

what happens to density as you go down group 1

Back 59

have a higher density because atoms have more mass

Front 60

what happens to their melting and boilingpoint as you go down group 1

Back 60

have a lower melting point and boiling point

Front 61

what happens when group 1 metals are put in water

Back 61

they react vigorously and move around the surface fizzing furiously

Front 62

what happens to group 1 metals when put in water

(2)

Back 62

they produce hydrogen.potassium gets hot enough to ignite

Front 63

what indicates hydrogen

Back 63

lighted splint producing a squeaky pop

Front 64

what happens when group 1 metals are put in water

(3)

Back 64

they make an alkaline solution

Front 65

what happens when group 1 metals react with chlorine

Back 65

they react vigorously and produce salts

Front 66

how many outer electrons do group 7 have

Back 66

seven making it very reactive giving them similar properties and they form similar compounds to eachother

Front 67

what are diatomic molecules

Back 67

pair of atoms

Front 68

what happens as you go down group 7

Back 68

halogens become less reactive

Front 69

why do group 7 become less reactive as you go down

Back 69

because the electrons are further from the nucleus and additional electrons are attracted less strongly

Front 70

How are group 7 melting and boiling points as you go down

Back 70

higher melting point and higher boiling point

Front 71

what are group 1 metals known as

Back 71

alkali metals

Front 72

what are group 7 metals known as

Back 72

halogens

Front 73

How is fluorine gas reactivity

Back 73

very reactive

poisonous

yellow gas at room pressure and temperature

Front 74

How is chlorine gas

Back 74

fairly reactive

poisonous

dense green gas at room temp and pressure

Front 75

How is bromine

Back 75

a dense poisonous liquid at room temp and pressure

forms an orange gas

Front 76

how is iodine

Back 76

dark grey crystalline at room temp or purple vapour

Front 77

halogens go from gases to solids down the group what does this show

Back 77

trend in melting and boiling point

Front 78

what happens when halogens react with alkali metals

Back 78

form salts called metal halidides

reactions become less vigorous as you go down group

Front 79

what happens when halogens react with iron

Back 79

form coloured solids called iron halidides

reactions become less vigorous as you go down the group

Front 80

what is this symbol

and give an exapmle

Back 80

oxidising

provides oxygen which allows other materials to burn more fiercely

eg.liquid oxygen

Front 81

what does the highly flammable sign mean give an example

Back 81

catches fire easily

eg petrol

Front 82

what does the toxic sign mean give exapmple

Back 82

can cause death

eg hydrogen cynanide

Front 83

what does explosive symbol mean

Back 83

can explode

eg some peroxide

Front 84

what does corrosive symbol mean

Back 84

attacks and destroys living tissues

eg concentrated sulfuric acid

Front 85

what happens when the group 1 elements are reactive

Back 85

they can combust spontaneously

Front 86

what happens if group 1 come in contact with water vapour

Back 86

there can be a very violent reaction depending on how much alkali is present

Front 87

how are alkali metals stored to prevent a violent reaction

Back 87

under oil

Front 88

why should alkali metals not be touched with bare hands

Back 88

the sweat on hands is enough to produce a reaction that will produce a lot of heat and corrosive hydroxide

alkaline solution is very corrosive

Front 89

what elements in group 7 are toxic

Back 89

chlorine and iodide

Front 90

what is the most reactive halogen

Back 90

fluorine

Front 91

how is liquid bromine

Back 91

corrosive contact with skin should be avoided

Front 92

how are halogens poisonous

Back 92

have poisonous vapours that irritate the respiratory system and eyes they must be in fume cupboard so fumes are not breathed in