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GCSES > chemistry > Flashcards

chemistry Flashcards

1
Q

tell me the details of the periods

A
  • they are horizontal
  • they tell us how many occupied shells there are
  • all elements in the same period have the same number of occupied energy shells
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2
Q

tell me the details of groups

A
  • they are vertical
  • they tell us how many electrons are on the outer shelll
  • all elements in the same group have thw same number of of electrons in their outer shells
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3
Q

where are non metals

A

on the right

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4
Q

solid to liquid?explain

A

melting
Particles gain kinetic energy and
vibrates faster, allowing particles to
overcome forces of attraction that
hold them together in the solid

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5
Q

liquid to solid? explain

A

freezing
Particles lose kinetic energy,
allowing forces of attraction
between the particles to hold them
together

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6
Q

liquid to gas? explain

A

evaporating
Particles gain kinetic energy and
move further apart, causing the
forces of attraction between them
to be completely broken

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7
Q

gas to liquid? explain

A

condensation
Particles lose kinetic energy and
vibrates faster, allowing forces of
attraction to bring particles closer
together

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8
Q

what state are metal oxides at room temp

A

solid

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9
Q

are metal oxides soluble or insoluble in water

A

insoluble

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10
Q

what state are non-metal oxides at room temp

A

solids or gases

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11
Q

are non-metal oxides soluble or insoluble in water

A

soluble

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12
Q

what do non-metal oxides from in water

A

acids

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13
Q

group one physical properties

A
  • soft
  • float in water
  • only shiny when freshly cut
  • stored in oil
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14
Q

what happens with lithium and water

A
  • it floats and efferveces
  • gets small until it dissapears
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15
Q

what does lithium and water make (pH)

A

a strong alkali (blue/purple)

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16
Q

lithium + water…

A

lithium hydroxide + hydrogen

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17
Q

how to know if a gas given off is hydrogen

A

squeaky pop with a lighted spling

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18
Q

what does sodium do different than lithium in water

A
  • it melts into a silver colored ball
  • it moves around faster and efferves more
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19
Q

what color is a sodium flame

A

yellow

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20
Q

sodium + water…

A

sodium hydroxide + hydrogen

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21
Q

what does potassium do differenly than sodium when reacting with water

A

it moves around faster and effereveces more

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22
Q

what flame color does potassium turn

A

lilac flame

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23
Q

potassium + water…

A

potassium hydroxide + hydrogen

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24
Q

what happens with rubidium and water

A

it immediatley sparks and almost looks like fireworks

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25
Q

what happens with water and caesium

A

it pops and then produces like fireworks and it is extremely powderful that it causes the glass to break

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26
Q

group 1 metals + water…

A

metal hydroxide + hydrogen

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27
Q

what do all group 1 metals form with water

A

alkalis

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28
Q

does the reactivity increase or decrease down group 1

A

increase

29
Q

why does the reactivity in group 1 increase going down

A

all atoms in group one only have 1
electron in their outer shell which
means in chemical reactions they
lose the outer electron to become
more stable

the outer shell is further from the
nucleus as you go down so it is
more easily lost causing there to be
a stronger reaction

30
Q

what do all group 7 elements have in common

A
  • they are all non metals
  • they have 7 electrons in their outer shelll
31
Q

what are the physical properties of group 7

A
  • they are all made up of diatomic molecules
  • they are made up of 2 atoms bonded together
32
Q

why is iodine unusual

A

when it is heated it sublimes (changes directly from a solid to a gas)

33
Q

trends down group 7

A
  • reactivity decreases
  • elements get darker in color
  • metling and boiling points increase
34
Q

what is the chemical test for chlorine

A

use damp blue litmus paper

result - the paper turns white if chlorien is present

35
Q

chlorine and hot iron wool

A

the iron glows brightly
a reddish-brown solid called iron(III) chloride is formed

36
Q

bromine and hot iron wool

A

the wool will only react is the bromind vapour is heated consistantly

it will glow but not as brightly as chlorine

it produces iron(III)bromide

37
Q

iodine and hot iron wool

A

they react very slowly

the only evidence is a reddish brown solid called iron(III) iodine

38
Q

what do all group 7 elements produce with iron

A

Halides

39
Q

what happens in group 7 chemical reactions

A

group 7 electrons gain an electron to achieve a full outer shell

40
Q

why does reactivity decrease in group 7

A

as we go down the outer shell is
further from the positive nucleus so
the incoming electron feels a
weaker attraction so it is less easily
gained

41
Q

how are the halogens formed

A

ionic compounds
called metal halides

42
Q

what is the aim of the displacement reaction

A

the aim of the displacement
reactions is to take a free halogen
elecent (Cl,Br,I) and see if it reacts
with a group one metal halide
(KCl,KBr,KI)

43
Q

what happens if a free halogen reacts with a group one metal halide

A

it changes color

44
Q

chlorine water + potassium bromide solution…

A

bromine water + potassium chloride

45
Q

how is a solution made

A

when a solid is dissolved in a liquid

46
Q

what is a concentrated solution

A

one which has a high proportion of a solute

47
Q

what is a dilute solution

A

one wich has a small amount of solute

48
Q

what is a saturated solution

A

one which no more will dissolve at that temperature

49
Q

units of solubility

A

g/100g of water

50
Q

what is the solubility of a solute

A

the mass in grams of the solute that will dissolve in 100g of solvent at a certain temperature

51
Q

solubility curve

A

solutbility on y axis
temperature on x axis

52
Q

what are chemical reactions

A

the movement of electrons

53
Q

where does ionic bonding occur

A

between a metal and non metal

54
Q

what is an ionic bond

A

an ionic bond is the strong electrostatic force of attraction between oppositley charged ions in a giant structure

55
Q

what does it imply is sodium is a solid with a high melting point at room temperature

A

if it has a high melting point it means the bonds must be so strong that they are hard to overcome

56
Q

what is sodium chloride made of

A

positively charged sodium ions
negitivley charged chloride ions

57
Q

what is a giant structure in sodium chloride

A

millions of sodium chloride ions in one sodium chloride crystal

58
Q

how does the sodium chloride ion form

A

each sodium atom looses one
electron to a chloride atom so that
both achieve a full outer shell of
electrons

The sodium atom becomes
positively charged

The chlorine atom becomes
negatively charged

59
Q

what must substances have to conduct electricity

A

charged free moving particles

60
Q

written explination of magnesium fluoride

A

each magnesium atom has 2
electrons in its outer shell. each
fluorine atom needs 1 more
electron to have a full outer shell.
This means 2 fluorine atoms are
needed for each magnesium atom.
A magnesium atom transfers 1 of
its outer shell electrons to one
fluorine atom and the second outer
shell electron to the other fluorine
atom. The magnesium atom
becomes positively charged and
the fluorine atom becomes
negatively charged fluoride ion

the ratio is 1:2

61
Q
A
62
Q

structure of metals

A

metals consist of a giant structure
of millions of regularly arranged
positive ions surrounded by a ‘sea’
of delocalized electrons

63
Q

what is a metallic bond

A

The metallic bond is the strong
electrostatic force of attraction
between the positively charged
metal ions and the negatively
charged delocalized ions

64
Q

where is metalic bonding present

A

metallic bonding is present in
metal elements such as iron,
copper, silver, gold and more

65
Q

what is an alloy

A

a mixture of a metal and non metal and usually one or more other elements

66
Q

why are alloys not as malleable as metals

A

the 2 elements are not the same
size which disrupts the layers
causing them to not slide over
each other

67
Q

melting point of metals and why

A

metals have a high melting point
because they have a giant structure
and these strong electrostatic
forces of attraction require a lot of
thermal energy to overcome them

68
Q

why are metals good conductors of energy

A

they have
delocalised electrons which are free to move

69
Q

why are metals malleable and ductile

A

the layers of metal ions in
the structure can slide over one
another without disrupting the
bond

GCSES (6 decks)

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