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the periodic table Flashcards

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1
Q

all group 1 metals have

A

high reactivity
malluable
low density
in a compound produce white solid.
soluble in water

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2
Q

Cl2, Br2, I2 colours
(aquos)

A

Cl2 is pale yellow
Br2 is orange
I2 orange/brown

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3
Q

mpt in group 1

A

decrease as you go down: Li not melting as well as Na

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4
Q

malluablilty in group 1

A

more mallauble as you go down: easier to cut

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5
Q

reactivity in group 1

A

more reactive as you go down : each reaction is easier to ignite so more reactive

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6
Q

Licl, Na2CO3, K2CO3 state and colour

A

white solid

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7
Q

Licl, Na2CO3, K2CO3 observation with water

A

dissolves to make colourless solution

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8
Q

Licl, Na2CO3, K2CO3 state and colour

A

white solid

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9
Q

halogen, halide

A

halogen= element in group 7
halide= an ion in group 7

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10
Q

K observation with metal and observation with water

A

gray, cut with knife

same as Li, makes white solid, lilac flame

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11
Q

Na observation with metal and observation with water

A

gray, cut with knife

same as Li, forms sphere, orange/yellow flame, makes white solid

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12
Q

Li observation with metal and observation with water

A

gray

effervescing, makes white solid, temp.increase, li disappears

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13
Q

all group 1 metals have

A

high reactivity
malluable
low density
in a compound produce white solid.
soluble in water

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14
Q

periodic patterns mpt

A

group 1: decreases as you go down
group 2: increases as you go down

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15
Q

periodic patterns reactivity

A

group 1: increases as you go down
group 2: decreases as you go down

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16
Q

what are group 2 metals called

A

alkaline earth metals

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17
Q

properties group 2

A

-mpt higher than group 1, because ions have a higher magnitude of charge and more delocalized electrons
-reactivity is lower than group 1, because ions lose 2 electrons instead of 1.

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18
Q

properties transition metals

A

very high mpt: many delocalized e-s
high density
form ions w/ variable changes
form coloured compounds

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19
Q

ions and colours:
Fe2+
Fe3+
Cu2+
Cr3+
Cr6+
Mn2+
Mn7+

A

Fe 2+ — green
Fe 3+ — orange/brown
Cu 2+ — blue
Cr 3+ — green
Cr 6+ — orange
Mn 2+ — faint pink
Mn 7+ — purple

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20
Q

what are group 8 non- metals called

A

noble 8

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21
Q

properties group 8

A

-unreactive due to full outer energy levels —> inert
-melting point increases as you go down, the atoms increase in size and therefore there are more inter-atomic forces
no bonding, exist as single atoms

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22
Q

group 8 element and use:
He
Ne
Ar

A

He = balloons, airships (<dense than air
Ne = electric lights (produce colour with electricity)
Ar = light bulbs (inert atmosphere)

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23
Q

how do halogens exist

A

as diatomic molecules (come in pairs, X2) held together with single covalent bonds

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24
Q

F2 colours

A

s= X
l= X
g= pale yellow
aq= colourless

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25
Q

Cl2 colours

A

s= X
l=X
g= pale green
aq= pale yellow

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26
Q

Br2 colours

A

s=X
l=red/brown
g=orange
aq=orange

27
Q

I2 colours

A

s= grey
l= X (sublimes)
g= purple
aq= brown/orange

28
Q

mpp/bpt and colour of halogens

A

increases as you go down, becuase the atom size increases. more surface area the more IMFs
colour becomes darker as you go down

29
Q

test for halogens: Cl2

A

damp blue litmus paper–>red–>white
hexane–> colourless

30
Q

test for halogens: Br2

A

damp blue litmus paper–>red—>white (slower)
hexane –>orange

31
Q

test for halogen: I2

A

starch—> blue or black
hexane—>pink

32
Q

iron + chlorine:
bromine + iron:

A

iron(3) chloride- brown solid
iron(3) bromide - brown solid

33
Q

all group 2 compounds are

A

white solids
colourless aq

34
Q

what is amphoteric
and which chemicals

A

acts as a acid and a base
Al2O3, ZnO,SiO

35
Q

what is an alkali

A

base that dissolve

36
Q

if it is a base it has OH- or H+

A

more OH-

37
Q

if it is an acid it has OH- or H+

A

more H+

38
Q

if it is neutral it has more OH- or H+

A

neither or equal amounts

39
Q

what four chemicals make up air

A
  1. nitrogen (78%)
  2. oxygen (21%)
  3. argon (0.97%)
  4. carbondioxide (0.03%)
40
Q

Mpt lowest to highest in air

A

Ar
N2/O2
CO2

41
Q

metal carbonate + acid —>

A

salt + water + carbondioxide

42
Q

uses for O2

A

ventilators/diving equipment
welding

43
Q

uses for CO2

A

fire extinguishers(doesn’t support combustion and is more dense than air
dry ice

44
Q

metal + acid —>

A

salt + hydrogen

45
Q

uses for H2

A

hydrogen fuel

46
Q

uses for Cl2

A

water treatment/ swimming pool
—–> HOCl kills bacteria
poinson gas

47
Q

combining powers:
1.phosphate
2.sulfate
3.carbonate
4. nitrate
5. sulfite
6.hydroxide
7. ammonium

A
  1. PO4, 3-
  2. SO4, 2-
  3. CO3, 2-
  4. NO3, 1-
  5. SO3, 2-
  6. OH, 1-
  7. NH4, 1+
48
Q

phosphorous + oxygen —–>

A

diphosphorouspentoxide

P2O5

49
Q

phosphoric acid

A

H3PO4

50
Q

What colour flame does carbon and oxygen burn with

A

orange flame

51
Q

sulfur + oxygen —>

A

sulfurdioxide = SO2 = blue flame
sulfurtrioxide = SO3

52
Q

sulfurdioxide + water —–>
sulfurtrioxide + water —>

A

sulfurous acid = H2SO3
sulfic acid = H2SO4

53
Q

non-metal oxide bonding, state at room temp. , pH in water

A

covalent, gas (except: P2O5, SiO2), acids except SiO.

54
Q

metal oxides bonding, state at room temp. , pH in water

A

ionic, solid, base (except Al2O3, ZnO)

55
Q

what flame does Ca + O2 burn with

A

brick red flame

56
Q

Licl, Na2CO3, K2CO3 with flame

A

red, orange/yellow, lilac

57
Q

Cl with NaCl, NaBr, KI

A

NaCl- nothing
NaBr- yellow to orange
hexane turns orange
KI- yellow to brown
hexane turns pink

58
Q

Br2 with NaCl, NaBr, KI

A

NaCl- nothing
hexane turns orange
NaBr- nothing
KI- orange to orange/brown
hexane turns pink

59
Q

KI with NaCl, NaBr, KI

A

NaCl- nothing
hexane turns orange
NaBr- nothing
hexane turns pink
KI- nothing

60
Q

mpt in simple covalent

A

depends on size of atoms

61
Q

mpt in ionic

A

depends on maginitude of charge and size of particles

62
Q

Al2O3 and ZnO and SiO2 are…

A

amphoteric

63
Q

amphoteric

A

ability to act as a acid and base

chemistry (10 decks)

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