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period table Flashcards

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1
Q

element

A

a substance that consists of only one type of atom and can’t be broken down into any simpler substances by chemical means

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2
Q

malleable

A

can be hammered into shape

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3
Q

ductile

A

can be drawn into wires

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4
Q

sonorous

A

clangs when struck

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5
Q

group

A

a vertical row in the period table

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6
Q

period

A

a horizontal row in the period table

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7
Q

displacement reaction

A

a reaction in which a more reactive element takes the place of a less reactive element in a compound

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8
Q

diatomic

A

two atoms covalent bonded in a molecule

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9
Q

sublimation

A

the change of state from a solid directly into a gas when heated

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10
Q

how did mendeleev arrange the elements

A

-in order of increasing atomic mass
-elements with similar properties kept in groups
-used creative thought and left gaps for undiscovered elements
-accurately predicted properties of undiscovered elements

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11
Q

describe todays periodic table

A

-there are no spaces
-arranged in order of increasing atomic number
-has the noble gases
-the transition metals are grouped together in a separate block

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12
Q

differences between mendeleev’s and todays period table

A

-mendeleevs was arranged in order of atomic mass, todays is in order of atomic number
-the modern has noble gases mendeleevs didn’t as they hadn’t been discovered
-todays has the transition metals block mendeleevs didn’t
-todays has lanthanides and actinides mendeleevs didn’t
-todays has more elements and no spaces

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13
Q

how can you tell if it’s a solid liquid or gas for the meting and boiling points

A

-melting and boiling point above room temperature means it’s a solid
-melting point below room temperature and boiling point above room temperature means it’s a liquid
-melting and boiling point below room temperature means it’s a gas

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14
Q

what’s the name of group 1 elements

A

alkali metals

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15
Q

name of group 2 elements

A

alkaline earth metals

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16
Q

name of group 7 elements

A

halogens

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17
Q

name of group 8 elements

A

noble gases

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18
Q

what does period number tell us

A

the number of shells of each atom in that period

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19
Q

what does group 1 contain

A

-reactive metals
-all have one electron in their outer shell

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20
Q

why are group one elements so reactive

A

-only have one electron in their outer shell
-they only need to lose one electron to gain a full outer shell and become more stable

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21
Q

density of alkali metals

A

alkali metals have a low density and lithium sodium and potassium are less dense than water therefore when added to water they float on the surface

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22
Q

storage of group 1 elements

A

stored in oil because they react with oxygen and moisture in the air

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23
Q

what do alkali metals look like when cut

A

-can be cut easily with a knife
-initially shiny
-quickly tarnished with air

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24
Q

safety precautions of alkali metals

A

-use small pieces of metal
-use a safety screen to prevent metal sparking out
-wear safety glasses
-handle with tweezers

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25
Q

general reaction of alkali metals with water

A

metal + water —> metal hydroxide + hydrogen

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26
Q

observation of lithium in water

A

-heat released
-moves on water surface
-bubbles
-lithium disappears
-colourless solution is produced

27
Q

observations of sodium in water

A

-heat released
-melts into a tiny ball
-moves on water surface
-bubbles
-sodium disappears
-colourless solution produced

28
Q

observations of potassium and water

A

-lilac flame
-melts into a tiny ball
-moves on waters surface
-bubbles
-potassium disappears
-colourless solution produced
-heat released

29
Q

balanced equation of lithium with water

A

2Li+2H20 -> 2LiOH+H2

30
Q

balanced equation of sodium with water

A

2Na+2H2O -> 2NaOH+H2

31
Q

balanced equation of potassium and water

A

2K+ 2H2O -> 2KOH+H2

32
Q

what happens to reactivity when going down group 1

A

-reactivity increases
-as group is descended the atoms get bigger
-outer shell electron is further away from the nucleus so is easier to remove as outer negative electron is less attracted by positive nucleus

33
Q

what happens to group 1 metals when they react

A

-they lose their electron
-they become an ion with a 1+ charge

34
Q

why do all group 1 metals react the same way

A

-they all have one electron in their outer shell
-so they all have to lose 1 electron when react to form a 1+ ion

35
Q

colours of group 1 compounds

A

-all group 1 compounds form white solids
-when they are dissolved they form colourless solutions

36
Q

what does group seven contain

A

-reactive non metals
-all elements have seven electrons in their outer shell
-all diatomic
-all toxic and must be used in the fume cupboard

37
Q

physical properties of fluorine

A

-gas
-yellow

38
Q

physical properties of chlorine

A

-gas
-green

39
Q

physical properties of bromine

A

-liquid
-red brown

40
Q

physical properties of iodine

A

-solid
-grey

41
Q

what happens as you go down group seven

A

-higher melting/boiling points
-atom size increases
-reactivity decreases
-colour gets darker

42
Q

physical properties of astatine

A

-solid
-black

43
Q

why are group seven elements so reactive

A

-seven electrons in their outer shell
-only need to gain one electron to get a full outer shell and become stable

44
Q

describe iodine in sublimation

A

-grey black crystals as a solid
-purple vapour as a gas

45
Q

test for chlorine

A

-put damp litmus paper into a test tube
-paper turns red then bleaches

46
Q

what happens to reactivity when going down group 7

A

-reactivity decreases
-as group descends atoms get bigger
-outer shell is further from positive nucleus so more difficult to attract an electron

47
Q

what happens to group 7 elements when they react

A

-name changed from ine to ide
-they gain an electron
-they become an ion with a 1- charge

48
Q

why do all group 7 elements react the same way

A

-they all have seven electrons in their outer shell
-they all gain one electron when they react to form a 1- ion

49
Q

observations of chlorine with potassium bromide

A

colourless to orange

50
Q

observation of chlorine with potassium iodide

A

colourless to yellow/brown

51
Q

observations of bromine with potassium bromide

A

colourless to yellow/brown

52
Q

halogen displacement experiment method

A

-add 1cm cubed of chlorine water to two test tubes
-add about same amount of potassium iodide to one and potassium bromide to the other
-record any observations
-repeat with bromine water (potassium chloride and iodide)
-repeat with iodine (potassium chloride and bromide)

53
Q

noble gases properties

A

-colourless
-inert

54
Q

what does inert mean

A

unreactive

55
Q

why are they so unreactive

A

they gave full outer shells so do not need to lose or gain any electrons to become more stable

56
Q

what happens to boiling point when going down the group

A

increase

57
Q

why do boiling points increase going down the group

A

the van der waal’s forces get stronger as you go down the group so more energy is needed to break apart the forces between atoms

58
Q

why are nobles gases’ boiling points low

A

-they are non metals and are monoatomic (exist as separate atoms not molecules)
-this means they only have very weak Van der waals forces between their atoms
-these require very little energy to break apart the atoms

59
Q

where are the transition metals

A

placed in a large block between group 2 and group 3

60
Q

properties of transition metals

A

-good conductors of heat and electricity
-malleable
-ductile
-high melting points
-usually hard and tough
-high densities
-they can form ions with different charges
-their compounds are often coloured

61
Q

charge on ions of transition metals

A

variable charges

62
Q

transition metals reaction with water

A

slow

63
Q

group 1 metals reaction with water

A

very vigorous

64
Q

colour of compounds of transition metals

A

rust

Chemistry (5 decks)

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