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Chemistry IGCSE > Chapter #13 - The Periodic Table > Flashcards

Chapter #13 - The Periodic Table Flashcards

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1
Q

What is similar in the electron configuration of group 1 metals?

A

They all lose one electron.

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2
Q

What are the observations of Li at room temp?

A

Grey solid (stored in oil to prevent reaction with oxygen and water).

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2
Q

What are the observations of Li with water?

A
  • Effervescing
  • Li disappears
  • temp. increase
  • floats and moves on surface
  • Produces colorless solution
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2
Q

What are the observations of Na at room temp.?

A

Shiny silver soft solid. (Like a block of cheddar)

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3
Q

What are the observations of Na with water?

A
  • Effervescing
  • Na disappears
  • Temp. increase
  • Floats and moves on surface
  • Produces colorless solution
  • Melts and forms a sphere
  • If prevented from moving, ignites with yellow/orange flame.
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4
Q

What are the observations of K at room temp.?

A

Very easy to cut (soft), grey solid, when cut, inside shiny.

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5
Q

What are the observations of K with water?

A
  • effervescing
  • K disappears
  • Temp. increases
  • Floats and moves on surface
  • produces colorless solution.
  • Melts and forms a sphere
  • Ignites with lilac flame
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6
Q

Which way are group 1 metals more reactive?

A

The group 1 metals become more reactive descending the group.

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7
Q

why are group 1 metals more reactive descending the group?

A

Because the outer electron is further from the nucleus. therefor, there is weaker electrostatic force of attraction, less energy is needed to remove the outer electron.

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8
Q

What reactivity depend on in metals?

A

Their ease to lose an electrons.

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9
Q

What way do group one metals have a higher mpt.?

A

The mpt. of group 1 metals increases while going up the group.

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10
Q

What is the density of group 1 metals?

A

All group 1 metals have low densities.

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11
Q

What color and state of matter are ALL group 1 compounds?

A

They are ALL white solids.

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12
Q

What are the observations of lithium chloride in water?

A

dissolves (not much)

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13
Q

What are the observations of sodium carbonate with water?

A

dissolves (not much)

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14
Q

What are the observations of potassium chloride with water?

A

dissolves (not much)

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15
Q

What are the observations of lithium chloride when it reacts with oxygen (with flame)

A

Makes red flame (does not melt)

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16
Q

What are the observations of sodium carbonate when it reacts with oxygen (with flame)?

A

Makes a orange/yellow flame

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17
Q

What are the observations of potassium chloride when it reacts with oxygen (with flame)?

A

Makes a lilac flame.

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18
Q

What are group 1 metals called?

A

alkalimetals

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19
Q

What are three things group 1 metal compounds have in common?

A
  • White solids
  • Produce colorless solution (with water)
  • Soluble in water
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20
Q

What are group 7 elements called?

A

Halogens

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21
Q

What elements are diatomic?

A

Halogens

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22
Q

What does diatomic mean?

A

The elements exist in pairs (X2)

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23
Q

What colors is fluorine in its viable states? What is its standard form?

A

Solid: X
Liquid: X
Gas: pale yellow*
(aq): colorless

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24
Q

What colors is chlorine in its viable states? What is its standard form?

A

Solid: X
Liquid: X
Gas: pale green*
(aq): pale yellow

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25
Q

What colors is bromine in its viable states? What is its standard form?

A

Solid: X
Liquid: red/brown*
Gas: orange
(aq): orange

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26
Q

What colors is iodine in its viable states? What is its standard form?

A

Solid: grey*
Liquid: X
Gas: purple
(aq): orange/brown

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27
Q

What way do group 7 non-metals have a higher mpt. and why is this?

A

Group 7 metals have a higher mpt. going down. This is because the atom (and molecules) increase in size. Therefore there are more IMFs so more energy is required to break them apart.

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28
Q

What is test 1 and test 2 for chlorine?

A

Test 1: damp blue litmus => red =>white
Test 2: add hexane => colorless

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29
Q

What is test 1 and test 2 for bromine?

A

Test 1 => damp blue litmus => red => white (but slower than chlorine)
Test 2 => add hexane => orange

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30
Q

What is test 1 and test 2 for iodine?

A

Test 1: add starch => blue/black
Test 2: add hexane => pink

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31
Q

What happens to the colors in group 7 moving down?

A

They get darker.

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32
Q

What is the explanation for test 1 (damp blue litmus paper)of chlorine?

A

Cl2 + H2O => HCl + HOCl
HCL= Hydrochloric acid (red)
HOCl => chloric acid (bleach)

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33
Q

What is the explanation for test 1(damp blue litmus paper) of bromine?

A

Br2 + H2O => HBr + HOBr
HBr = hydrobromic acid
HOBr = bromic acid

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34
Q

What is the reaction of chlorine with iron?
What are the states of matter and color of each substance?
What happens as the reaction occurs?

A

iron + chlorine => iron (III) chloride
2Fe + 3Cl2 => 2FeCl3
Glows red as reaction happens
Fe= grey solid
Cl2= green gas
FeCl3 = brown solid

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35
Q

What is the reaction of bromine with iron (only symbol equation)?
What are the states of matter and color of each substance?

How does it’s reactivity compare to chlorine

A

3Fe + 3Br2 => 2FeBr3
bromine is less reactive than chlorine

36
Q

What way do group 7 non-metals have a lower reactivity and why?

A

Group 7 non-metals reactivity decreases going down the periodic table.The lower you go in the group, the more occupied elements the atoms have, therefor, the nucleus gets farthre away from the electron it needs to attract and so it has a weaker electrostatic force.

37
Q

What is the definition of displacement in chemistry?

A

A more reactive element replaces a less reactive one from a compound.

38
Q

What is displacement of halogens? (In my own words)

A

A more reactive halogen (group 7 non-metal) replaces a less reactive halogen in a compound with a metal.

39
Q

What are halides?

A

Ions of group 7

40
Q

What do you call ions of group 7?

41
Q

What are group 2 metals called?

A

Alkaline earth metals

42
Q

What are alkaline earth metals?

43
Q

What way do group 2 metals decrease in mpt. ?

How does it compare to group 1

A

The mpt. decreases as it goes down the periodic table.This is because the electrostatic forces get weaker as you go down the row. But, the mpt. of any group 2 atom will be higher than any group 1 atom. This is due to higher magnitude of charge and more delocalized electrons.

44
Q

What way are group 2 metals more reactive?

and how does that compare to group 1

A

The reactivity increases going down, but less reactive than group 1 as they need to lose 2 electrons.

45
Q

What are the properties of transition metals?

A
  • High mpt. (higher than 1 & 2)
  • High density
  • Variable charges (2+, 3+ => 8+) (can change on what it is reacting with and how much energy is present)
  • Form color compounds
  • Acts as a catalyst
46
Q

What is the color of the ion Fe^2+

47
Q

What is the color of the ion Fe^3+

48
Q

What is the color of the ion Cu^2+

49
Q

What is the color of the ion Mn^7+

50
Q

What is the color of the ion Cr^3+

51
Q

What is the color of the ion Cr^6+

52
Q

What is group 8 called?

A

Noble gases (0)

53
Q

What are noble gases (0)?

54
Q

What are some of the characteristics of noble gases?

A
  • Full outer energy level => unreactive/inert
  • NO bonding exists as single atoms (discrete)
55
Q

What are the properties of noble gases?

A
  • Very low mpt. , very weak inter-atomic forces. Mpt. increases He=>Ar
  • Do not conduct because they have no charged particles.
  • Insoluble in water
56
Q

What are the uses of He?

A

Balloons/air ships (less dense than air)

57
Q

What are the uses of Ne?

A

Lighting (produces color with electricity)

58
Q

What are the uses of Ar?

A

Lightbulbs (inert atmosphere)

59
Q

Metal + Oxygen =>

A

Metaloxides

60
Q

Metal oxide + water =>

A

Metal hydroxide

61
Q

What happens after metal oxides and water react?

A

They dissociate (if they are soluble). That is why when you add universal indicator, and the solution is soluble, chemicals have already separated, so the acids and base ions are separated from the metal ions.

62
Q

What is Li + O2? Right the WHOLE equation and balance it.

State of matters?
Reaction?
Colors?

A

4Li + O2 => 2LiO
Burns with red flame
Li = Grey (s)
O2 = Colorless (g)
Li2O = White (s)

63
Q

What is Li2O with water?
Colors?
State of matters?
U.I. added?
Sloubility?

A
  • Li2O + H2O => 2LiOH
  • Li2O = white (s)
  • H2O = colorless (g)
  • LiOH = colorless (aq)
  • Turns purple with U.I. (OH ion is strong base)
64
Q

What is Mg with oxygen?

Color?
Reaction?
States of matter?

A
  • 2Mg + O2 => 2MgO
  • Mg = grey (s)
  • O2 = colorless (g)
  • MgO = white (s)
  • Forms white flame
65
Q

What is MgO with water?

Color?
Soluble?
States of matter?
Color with U.I.?

A
  • MgO + H2O => Mg(OH)2
  • Makes white suspension
  • Dissolves very little
  • Add U.I. = Blue (weak acid)
66
Q

What is Ca with oxygen?
Color, States of matter ect.

A
  • 2Ca + O2 => 2CaO
  • Ca = grey (s)
  • CaO = white (s)
  • Burns with brick-red flame

If you are confused, review notes on metal oxides

67
Q

What metal oxides don’t react with H2O?

A
  • Al2O3
  • Fe2O3
  • ZnO

If you are confused, review your notes on metal oxides

68
Q

What is the product of non-metals and oxygen?

A

Covalent(non-metal) oxides

with a discrete structure

69
Q

non-metal oxide + water =>

70
Q

What does exothermic mean?

A

Releases a lot of heat

71
Q

What is the general state of metal oxides at room temp.?

A

Solids

Generally, sometimes they arn’t, but in those instances, you can not tel

72
Q

What is the general state of non-metal oxides and

73
Q

What is the general pH of metal oxides?

A

<7 (bases)

74
Q

What is the different rule for when you write the product of a non-metal + water?

A

You have to write the prefix before each chemical to know how much there is of each chemical.

75
Q

Write the prefixes from 2-7

A

Di = 2
Tri= 3
Tetra = 4
Penta = 5
Hexa = 6
Hepta = 7

76
Q

What is the symbol equation of phosphorus + oxygen and what are some of the things that happen?

A

4P +5O2 => 2P2O5 (diphosphourupent(a)oxide)

  • It spontaeneously combusts with a white flame when it reacts.
  • Product has a high(ish) mpt. even though it is covalently bonded. This is beacuse it has a lot of IMF’s because it is a large molecule.
77
Q

What is the equation for
diphosphourouspentaoxide
+ water => and what happens?

A

P2O5 + 3H2O => 2H3PO4
* When the reaction happens it is exothermic
* It make phosphoric acid
* It makes a really strong acid pH = 0

78
Q

What are the chemicals in the air and how what perecntage of the air do they make up?

A
  • Nitrigen (78%)
  • Oxygen (21%)
  • Argon (0.97%)
  • Carbon dioxide (0.03%)
79
Q

What are the properties of transition metals?

A
  • High mpt. (higher than group 1+2 metals
  • High density
  • Variable charges (2+, 3+…8+) Can change depending on what it is reacting with and how much energy is present.
  • Form color compunds
80
Q

Compared to group 1 metals

What are the mpt. of alkaline earth metals?

A

Always higer than geoup 1 metals - due to higher magnitude of of charge and more delocalized electrons.

81
Q

What way do group 2 metals have a lower mpt.

A

Going down the periodic table

82
Q

What way do group 2 metals decrease in reactivity.

A

They decrease in reactivity going up. But it is less reactive than group 1 beacuse they have to loes to electrons.

83
Q

Are group 1 or group 2 atoms bigger?

A

Group 1 atoms are bigger.

84
Q

What color is any lithium flame (generally)?

85
Q

What color is any sodium in a flame (generally)?

A

Orange/yellow

86
Q

What color is any potassium in a flame (generally)?

87
Q

What is CaO with water?
Color, recation, U.I. ect.

A
  • Ca + H2O => Ca(OH)2
  • White suspension
  • dissolves only a little
  • Add U.I. => blue (weak base - a little stronger the Mg(OH)2)
88
Q

What is Al with oxygen?Also what happens when you add U.I to product?

A

4Al +3O2 => 2Al2O3
Burns with orange flame

89
Q

Fe with oxygen
only need color and the clarification. write the symbol equation but also the product in words.

Does the product dissolvein water?

A
  • 4Fe + 3O2 => 2Fe2O3
  • Fe2O3 = Iron (III) oxide
  • Fe2O3 = Orange /brown
  • The product does not dissolve and U.I does not work on it beacuse U.I. only works on solutions.

Chemistry IGCSE (13 decks)

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