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chemistry Flashcards

(69 cards)

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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
what happens with water and caesium
it pops and then produces like fireworks and it is extremely powderful that it causes the glass to break
26
group 1 metals + water...
metal hydroxide + hydrogen
27
what do all group 1 metals form with water
alkalis
28
does the reactivity increase or decrease down group 1
increase
29
why does the reactivity in group 1 increase going down
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
what do all group 7 elements have in common
* they are all non metals * they have 7 electrons in their outer shelll
31
what are the physical properties of group 7
* they are all made up of diatomic molecules * they are made up of 2 atoms bonded together
32
why is iodine unusual
when it is heated it sublimes (changes directly from a solid to a gas)
33
trends down group 7
* reactivity decreases * elements get darker in color * metling and boiling points increase
34
what is the chemical test for chlorine
use damp blue litmus paper result - the paper turns white if chlorien is present
35
chlorine and hot iron wool
the iron glows brightly a reddish-brown solid called iron(III) chloride is formed
36
bromine and hot iron wool
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
iodine and hot iron wool
they react very slowly the only evidence is a reddish brown solid called iron(III) iodine
38
what do all group 7 elements produce with iron
Halides
39
what happens in group 7 chemical reactions
group 7 electrons gain an electron to achieve a full outer shell
40
why does reactivity decrease in group 7
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
how are the halogens formed
ionic compounds called metal halides
42
what is the aim of the displacement reaction
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
what happens if a free halogen reacts with a group one metal halide
it changes color
44
chlorine water + potassium bromide solution...
bromine water + potassium chloride
45
how is a solution made
when a solid is dissolved in a liquid
46
what is a concentrated solution
one which has a high proportion of a solute
47
what is a dilute solution
one wich has a small amount of solute
48
what is a saturated solution
one which no more will dissolve at that temperature
49
units of solubility
g/100g of water
50
what is the solubility of a solute
the mass in grams of the solute that will dissolve in 100g of solvent at a certain temperature
51
solubility curve
solutbility on y axis temperature on x axis
52
what are chemical reactions
the movement of electrons
53
where does ionic bonding occur
between a metal and non metal
54
what is an ionic bond
an ionic bond is the strong electrostatic force of attraction between oppositley charged ions in a giant structure
55
what does it imply is sodium is a solid with a high melting point at room temperature
if it has a high melting point it means the bonds must be so strong that they are hard to overcome
56
what is sodium chloride made of
positively charged sodium ions negitivley charged chloride ions
57
what is a giant structure in sodium chloride
millions of sodium chloride ions in one sodium chloride crystal
58
how does the sodium chloride ion form
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
what must substances have to conduct electricity
charged free moving particles
60
written explination of magnesium fluoride
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
62
structure of metals
metals consist of a giant structure of millions of regularly arranged positive ions surrounded by a 'sea' of delocalized electrons
63
what is a metallic bond
The metallic bond is the strong electrostatic force of attraction between the positively charged metal ions and the negatively charged delocalized ions
64
where is metalic bonding present
metallic bonding is present in metal elements such as iron, copper, silver, gold and more
65
what is an alloy
a mixture of a metal and non metal and usually one or more other elements
66
why are alloys not as malleable as metals
the 2 elements are not the same size which disrupts the layers causing them to not slide over each other
67
melting point of metals and why
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
why are metals good conductors of energy
they have delocalised electrons which are free to move
69
why are metals malleable and ductile
the layers of metal ions in the structure can slide over one another without disrupting the bond

GCSES (6 decks)

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