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Chemistry Y10 > Alkali metals > Flashcards

Alkali metals Flashcards

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1
Q

Group 1 of the Periodic Table contains ……….

A

Lithium (Li)

Sodium (Na)

Potassium (K)

Rubidium (Rb)

Caesium (Cs)

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2
Q

Why do you think that the Group 1 metals are stored under oil?

A) To keep them moist and ready to react in experiments

B) To keep them out of contact with oxygen in the air

C) To lubricate the surface of the metal

A

B

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3
Q

The table below shows that Group 1 elements have low melting points for metals:

Group 1 metalMelting point (°C)

Lithium 180

Sodium 98

Potassium 63

Rubidium 39

Look at the table above. Which statement below is true?

A) There is no pattern in the melting points of the Group 1 metals as we go down the group.

B) The melting points of the Group 1 metals decrease as we go down the group.

C) The melting points of the Group 1 metals increase as we go down the group.

A

B

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4
Q

Predict the approximate melting point of caesium, the element below rubidium in Group 1.

Between 40 °C and 50 °C

Between 20 °C and 30 °C

Between 60 °C and 70 °C

A

B

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5
Q

Which Group 1 metal is most difficult to cut with a knife and has the highest melting point?

Sodium

Lithium

Potassium

Rubidium

Caesium

A

Lithium

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6
Q

Liquid sodium is piped around some nuclear power stations to transfer heat. Which two properties of sodium make it suitable for this use?

A

It has a low melting point.

It is a good conductor of heat.

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7
Q

Group 1 metals are called the alkali metals. why?

A

They get their name from their reaction with water, which produces an alkaline solution

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8
Q

Which of the alkali metals shown below ignites the hydrogen given off, which burns with a lilac flame?

Lithium

Potassium

Sodium

A
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9
Q

Which of the alkali metals shown below melts into a silver ball that moves around the surface of the water as it reacts?

Potassium

Sodium

Lithium

A

Sodium

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10
Q

You can collect the gas given off as lithium reacts with water. Which test shows that the gas collected is hydrogen?

A glowing splint re-lights

A lighted splint explodes with a squeaky ‘pop’

Limewater turns milky

A

A lighted splint explodes with a squeaky ‘pop’

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11
Q

What is the pH value of the solution produced when the Group 1 metals react with water?

7

Greater than 7

Less than 7

A

Greater than 7

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12
Q

Which of the three metals is most reactive with water?

Lithium

Potassium

Sodium

A

Potassium

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13
Q

Caesium explodes when put into water, smashing the glass trough. Which statement do you think describes the pattern in reactivity as we go down Group 1?

The Group 1 metals get less reactive as we go down the group.

The Group 1 metals get more reactive as we go down the group.

There is no pattern in their reactivity.

A

The Group 1 metals get more reactive as we go down the group.

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14
Q

Here are the equations for the reactions with water:

lithium + water lithium hydroxide + hydrogen
2 Li(s) + 2 H2O(l) 2 LiOH(aq) + H2(g)
sodium + water sodium hydroxide + hydrogen
2 Na(s) + 2 H2O(l) 2 NaOH(aq) + H2(g)
potassium + water potassium hydroxide + hydrogen
2 K(s) + 2 H2O(l) 2 KOH(aq) + H2(g)
A
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15
Q

What is the equations of the reaction between rubidium and water?

A

2 Rb(s) + 2 H2O(l) 2 RbOH(aq) + H2(g)

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16
Q

What is the equation of the reaction lithiumand water?

A 
lithium + water lithium hydroxide + hydrogen
2 Li(s) + 2 H2O(l) 2 LiOH(aq) + H2(g)
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17
Q

What is the equation of the reaction sodium and water?

A 
sodium + water sodium hydroxide + hydrogen
2 Na(s) + 2 H2O(l) 2 NaOH(aq) + H2(g)
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18
Q

What is the equation of the reaction potassium and water?

A 
potassium + water potassium hydroxide + hydrogen
2 K(s) + 2 H2O(l) 2 KOH(aq) + H2(g)
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19
Q

Which of the equations below show possible reactions of lithium?

A) 4 Li(s) + O2(g) 2 Li2O(s)

B) Li(s) + Cl2(g) 2 LiCl2(s)

C) 2 Li(s) + Cl2(g) 2 LiCl(s)

D) Li(s) + O2(g) LiO2(s)

A

A & C

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20
Q

Write the equation showing the formation of potassium oxide is:

A 
potassium + oxygen potassium oxide
4 K(s) + O2(g) 2 K2O(s)
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21
Q

The alkali metals react vigorously when heated with chlorine gas. Give an example:

A 
sodium + chlorine sodium chloride
2 Na(s) + Cl2(g) 2 NaCl(s)
potassium + chlorine potassium chloride
2 K(s) + Cl2(g) 2 KCl(s)
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22
Q
A
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23
Q

Summary

A

Group 1 elements are called the alkali metals.

They are soft metals that tarnish quickly in air.

The Group 1 metals get more reactive as we go down the group.

Their melting points decrease as we go down the group. The melting points are all low for metals, as are the densities of these elements.

The alkali metals are the most reactive group of metals in the Periodic Table. They form soluble compounds that are usually white.

They react vigorously with water, giving off hydrogen gas and producing an alkaline solution.

Because they are very reactive, they are stored under oil.

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24
Q

Name the product of the reaction between potassium and chlorine.

Potassium chloride

Potassium oxide

Potassium chlorate

A

Potassium chloride

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25
Q

Predict the colour of the product in the previous question.

A

White

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26
Q

Caesium + water …

A

caesium hydroxide + hydrogen

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27
Q

As the atomic number of an alkali metal increases, its reactivity …

A

increases

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28
Q

Which gas is given off when an alkali metal reacts with water?

A

hydrogen

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29
Q

Which of these alkali metals is easiest to cut with a knife?

Lithium

Sodium

Potassium

A

Potassium

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30
Q

Which of the alkali metals has the highest melting point?

Lithium

Sodium

Potassium

Rubidium

Caesium

A

Lithium

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31
Q

what is the electronic structure for the below atoms

Sodium

Potassium

Lithium

A

Sodium 2,8,1

Potassium 2,8,8,1

Lithium 2,1

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32
Q

How many electrons are in the highest energy level (outer shell) of all the Group 1 metals?

A

1

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33
Q

What is the charge on the ion formed when an atom of an alkali metal reacts?

A

+1

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34
Q

Which of these would make it easier for an atom to lose an electron?

The electron being nearer to the positively charged nucleus

The electron being further from the positively charged nucleus

A

The electron being further from the positively charged nucleus

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35
Q

Why do the alkali metals get more reactive as we go down the group?

A

Because

This is because as we go down the group the outer electron of the atom is further from the attractive force of the nucleus. It is also shielded from the nucleus by more complete lower energy levels (full inner shells) of electrons.

If an electron is further from the attractive force of the nucleus, it is easier to remove it from the atom so it becomes more reactive

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36
Q

Why the alkali metals are the most reactive group of metals in the Periodic Table?

A

the atoms of alkali metals all have just one electron in their highest energy level (outer shell) and It is relatively easy to lose this one electron

losing this outer electron, they form stable ions with a 1+ charge, e.g. Na+.

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37
Q

As we go down Group 1,

The outer electron is more tightly held by the nucleus in larger atoms. True/False

The outer electron is further from the attractive force of the nucleus in larger atoms.

True/False

The outer electron is shielded from the attractive force of the nucleus by more inner shells of electrons. True/False

The outer electron in larger atoms is more strongly attracted by neighbouring atoms.

True/False

A

The outer electron is more tightly held by the nucleus in larger atoms. False

The outer electron is further from the attractive force of the nucleus in larger atoms.

True

The outer electron is shielded from the attractive force of the nucleus by more inner shells of electrons. True

The outer electron in larger atoms is more strongly attracted by neighbouring atoms.

False

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38
Q

Are these statements true or false?

  • Metals are on the right of the periodic table.
  • Metal hydroxide is made when metals react with air.
  • Group 1 metals are kept under oil.
  • Hydrogen is produced when group 1 metals react with water.
  • Hydrogen is tested with limewater.
  • Lithium is the most reactive group 1 metal.
A
  • Metals are on the right of the periodic table. (F)
  • Metal hydroxide is made when metals react with air. (F)
  • Group 1 metals are kept under oil. (T)
  • Hydrogen is produced when group 1 metals react with water. (T)
  • Hydrogen is tested with limewater. (F)
  • Lithium is the most reactive group 1 metal. (F)
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39
Q
  • Name two group 1 metals
  • Describe the trend in reactivity down period 1
  • Explain the trend in reactivity down group 1
  • Explain why group 1 metals are called the alkali metals
  • What gas is produced when the group 1 metals react with water- how can we test for the presence of this gas?
A

•Name two group 1 metals

Lithium and sodium

•Describe the trend in reactivity down period 1

they get more reactive as we go down the group and the reactions occur more rapidly

•Explain the trend in reactivity down group 1

As we move down the group the atoms have more shells of electrons and the atom gets bigger. and as the atom gets bigger the outer electrome is further from the nucleus so it is less strongly attached by the nucleus , and therefore it is more easily lost.

•Explain why group 1 metals are called the alkali metals

Because they react with water forming a metal hydroxide which is alkaline. PH above 7 (universal indicator is blue) (OH- ion)

•What gas is produced when the group 1 metals react with water- how can we test for the presence of this gas?

Hydrogen which burns with a lilac flame.

40
Q

Alkali metals react with oxygen to form

A

metal oxides

41
Q

Alkali metals react with halogens to form

A

IONIC SALTS

42
Q

The alkali metals react with water to form

A

METAL HYDROXIDES

43
Q

The melting and the boiling point of halogens become ………………. as we go down the group, and the molecules become ………..

A

increase, bigger

44
Q

Why Lithium, Sodium and Pottasium float on water?

A

Becasue they are less dense than water

45
Q

Bromine and iodine are not gaseous, but have low boiling points. This means that they produce vapour at relatively low temperature. They are……

A

volatile

46
Q

Bromine produces some ,…………..vapour, seen here above the liquid bromine in the jar.

A

red-brown

47
Q

When iodine is heated gently, it changes directly from a ………… to a …………… without first becoming a liquid

this is called

A

solid, gas

This is called sublimation.

48
Q

Physical Properties of Halogens

A
  • The boiling points of the halogens increases down the group.
  • Fluorine and chlorine are gases at RTP.
  • Bromine is a liquid at RTP.
  • Iodine is a solid at RTP.
49
Q

The boiling points of the halogens increases down the group 7 (halogens) Explain why

A

this can be explained because the size of the intermolecular forces down the group increase. This means a higher temperature and more energy is needed to overcome the attractions between molecules to change to the gaseous state.

50
Q

How do halogen molecules exist?

A

All halogen atoms require one more electron to obtain a full outer shell and become stable.

Each atom can achieve this by sharing one electron with another atom to form a single covalent bond.

diatomic molecules

51
Q

colours of halogens

A
52
Q

in halogens group

Reactivity ………… up the group.

A

increases

53
Q

The reactivity of halogens decreases going down the group. What is the reason for this?

A
  • The atoms of each element get larger going down the group.
  • This means that the outer shell gets further away from the nucleus and is shielded by more electron shells.
  • The further the outer shell is from the positive attraction of the nucleus, the harder it is to attract another electron to complete the outer shell.
54
Q

where does the attraction of halogens for an extra electron gets greater?

Florine ? or clorine ?

A

going up the group

55
Q

If we mix a metal halide with a more reactive halogen, the electron will be transferred from the ………….to the ………………….reactive halogen:

A

less , more

56
Q

a reaction of chlorine and sodium bromide

what is the initial color of the solution , and what the final colour of the solution?

A
57
Q

uses of bromine

uses of chlorine

uses of fluorine

A

cromine : photography, medicines

chlorine : antiseptics and disinfectants, Bleach to kill bacteria

fluorine: toothpase prevention from decay , polymers, add to water

58
Q

Astatine is below iodine in group 7. Predict, with a reason, which halogens astatine will displace from solutions of their halides.

A

Astatine will not displace any of the other halogens as reactivity decreases down the group so astatine is the least reactive.

59
Q

During a displacement reaction, the halogen atoms gain an electron to form a negative halide ion.

Fluorine atoms form F− ions and chlorine atoms form Cl− ions.

draw the electronic structure ( brackets, and ions)

A
60
Q

As you go down group 7, it becomes more difficult for the atoms to form a negative ion because:

A

the atoms are getting larger as there are more shells of electrons

so the force of attraction between the positive nucleus and the incoming electron decreases.

61
Q

§the atoms are getting larger as there are more shells of electrons

§

§so the force of attraction between the positive nucleus and the incoming electron decreases.

A

Iodine atoms are larger than chlorine atoms as they have more shells of electrons.

There is a weaker force of attraction between the positive nucleus and the incoming electron in iodine than in chlorine.

62
Q

Displacement reactions are also …………………reactions.

A

redox

Oxidation Is Loss of electrons

Reduction Is Gain of electrons

63
Q

Bromine reacts with potassium iodide solution.

Br2 + 2KI → I2 + 2KBr

(a) Write the ionic equation for this reaction.
(b) Write the half equations.
(c) Explain what has been oxidised and what has been reduced.

A

Answers

(a) Br2 + 2I− → I2 + 2Br−
(b) Br2 + 2e → 2Br−

2I− → I2 + 2e

(c) Bromine molecules have gained electrons so they have been reduced.

Iodide ions have lost electrons so they have been oxidised.

64
Q
  • The air is made up mostly of ………………and ……………..along with small amounts of other gases
  • Gases of the air can be separated by ……………..
A
  • The air is made up mostly of nitrogen and oxygen along with small amounts of other gases
  • Gases of the air can be separated by fractional distillation.
65
Q

The composition of air

A
  • Around 78% of the air is nitrogen.
  • About 21% is oxygen.
  • The remaining 1% is mostly argon (0.93%), with carbon dioxide (.04%) and varying amounts of water vapour.
66
Q

Nitrogen - 196ºC

Oxygen - 183ºC

Argon - 186ºC

When air is distilled:

  1. Which gas will boil first?
  2. Which gas will there be most of?
  3. Which gas will there be least of?
A

When air is distilled:

  1. Which gas will boil first? Nitrogen
  2. Which gas will there be most of? Nitrogen
  3. Which gas will there be least of? Argon
67
Q
  1. Carbon + oxygen
  2. Hydrogen + oxygen

Methane (CH4) + oxygen

Sulfur + Oxygen à Sulfur Dioxide

Write the symbol equation

A

C + O2 —> CO2

H2 + 1/2 O2 —-> H2O

CH4 + O2 —> CO2 + 2H2O

S + O2——> SO2

SO2 is acid gas

68
Q

is an acid gas that can also dissolve in rainwater and cause acid rain.

It contributes to photochemical smog and is harmful to humans and animals.

A

NO2

Nitrogen Dioxide

69
Q

Write the combusion equation for Nitrogen and Oxygen

A

Nitrogen + Oxygen à Nitrogen Dioxide

N + O2 à NO2

70
Q

is an acid gas that can dissolve in rainwater and cause acid rain.

It is damaging to buildings and can adversely affect sensitive ecosystems by changing the pH.

A
71
Q

what do we use for the combustion of nitrogen and oxygen? and why do we need it?

A

combustion engine

combustion engine temperatures are high enough for the oxygen in the air to combine with the nitrogen:

72
Q

Give 3 causes for the Release of Carbon Dioxide

A
  1. Excess Carbon dioxide can cause a process known as Global Warming.
  2. Acid rain can also release carbon dioxide from rocks; acidic oceans can react with rocks or corals that contain calcium carbonate to also release carbon dioxide gas.
  3. Carbon dioxide is also stored in the lakes and oceans – an increase in temperature can reduce carbon dioxide’s solubility and it is release into the atmosphere.
  4. Carbon dioxide is stored in rocks as carbonates e.g. calcium carbonate.

The carbonates undergo thermal decomposition (breaking down by heating) in many industrial processes

CaCO3 à CaO + CO2

73
Q

explain the reason that the melting points decrease as we go down the group 1

A

this is because the atoms get bigger as we go down the group. in the metallic lattice the protons are further from the delocalised electrons in caesium than in sodium and therefore there is weaker electrostatic attraction.

74
Q

What is the method of seperating gases?

A
75
Q

Nitrogen makes up about 4/5 of the atmosphere.

Oxygen makes up about 1/5 of the atmosphere.

True of false

A

True

76
Q

explain the method to measure oxgen in air

why do we need to heat the copper?

when do we stop heating?

what do you notice regarding the volume of the air during the experiment?

what is the initial colour of Copper?

what is the colour at the end of the experement?

why did the colour change?

Explain why you waited for the apparatus to cool down after the experiment before reading the volume of air in the syringe.

A

https://www.youtube.com/watch?v=xAQ3ACUICcY

so the oxygen in the air reacts with the copper.

when the copper color turnes into black

the volume of the air gets smaller

initial is orange, final is black

cupper reacted with oxygen in the air forming copper oxide

the air volume we measured at the start of the experiment was cool air (100cm3) , and in order to have a fair experiment, we need to let the air cool down so we measure the volume of cool air as well.

otherwise the experiment is not fair.

77
Q

Chemical properties of group 1

A
  1. they all react with water in the same way to form a hydroxide with the formula MOH
  2. they all react with oxygen to form oxide with the formula M2O
  3. they all react with halogens to form compunds with the formula MX
  4. they form ionic compunds which contain an M+ ion.
78
Q

Physical properties of group 1

Li/Na/K/Rb/Cs/Fr

as we go down the group the

meting point ( increases/ decreases)

boiling point ( increases / decreases)

denisty g/cm3 ( increases/ decreases)

softness (increases / decreases)

A

meting point ( increases/ decreases)

boiling point ( increases / decreases)

denisty g/cm3 ( increases/ decreases)

79
Q

Physical properties of elements in group 1

A
  1. melting points are very low
  2. densities is low
  3. very soft and easily cut with knife
  4. shiny and silver whne freshly cut but tarnish very quickly on exposure to air.
80
Q

chemical properties depend on…………

chemical properties of group 1 elements as we go down the group

A

the number of electrones in the outer shell

more reactive with water

more reactive with air tarnishes quickly

more reactive with halogens

81
Q

Write the equation of sodium reaction with water with state symbol

A

2Na(s) + 2H2O(l) –> 2NAOH(aq) + H2(g)

Sodium is usually used ad molten sodium but to avoid confusion we write state symbol as (s)

82
Q

what is your observation for the sodium water reaction?

A
  1. the sodium floats because it is less dense than water
  2. the sodium melts into a ball because its melting point is low and a lot of heat is produced by the reaction (exothermic)
  3. there is fizzing because hydrogen gas is produced.
  4. the sodium moves around on the surface of the water because the hydrogen isn’t given off symmetrically around the ball, the sodium is pushed around the surface of the water by the hydrogen.
  5. the piece of sodium gets smaller an eventually disappears ( used up)
  6. test using universal indicator gives blue.
83
Q

lithium reaction with water compared to sodium reaction with water

It is very similar except that it is (slower / faster)

lithium ( melts/ doesn’t melt)?

A

It is very similar except that it is slower

lithium ( melts/ doesn’t melt)

84
Q

when lithium reacts with water it doesn’t melt. explain why?

A

because the melting point of lithium is higher and the heat isn’t produced so quickly so the lithium doesn’t melt.

85
Q

lithium reaction with water is slower than sodium reaction with water

how can you observe this in the experiment?

A

lithium reaction

fizzes more slowly

lithium moves around the surface of water more slowly.

lithium takes longer to disappear.

86
Q

compare potasium reaction with water and sodium reactions with water

A

Potassium

fizzes more vigorously

moves around more quickly

disappears more quickly

disappears more quickly

Key difference : with potassium the hydrogen bursts into flame but in sodium does not

87
Q
  • compare rabidium and caesium reaction with water and sodium reaciton with water
  • what is your predection about francium?
A

rabidium and caesium reaction can be explosive.

Francium is even more explosive

88
Q

VERY IMPORTANT

write the water half equation when group 1 metal reacts with water. producing a hydroxide.

write the half equation when group1 metal reacts with water forming metal ions in solution ( example sodium)

A

2H2O(l) + 2e- —> 2OH-(aq) + H2(g)

Na(s) —> Na+(aq) + e-

89
Q

burning group 1 metals in the qir we get vigorous reaction , state the different flame colours of burning

lithium

sodium

potassium

A

lithium : red flame to form lithium oxide

sodium : yellow flame to form sodium oxide

potassium : lilac flame to form potassium oxide

90
Q

when burning lithium , sodium and pottasium

what is the desctiption of the product formed?

what is the equation?

what other types of oxides can be formed?

A

It is a white powder in solid state, it is the alkali metal oxide.

they all have the same equation

4M(s) + O2(g) —-> 2M2O(S)

other types of oxides

peroxides (M2O2)

and superoxides (MO2)

lithium can also form a nitride (Li3N)

91
Q

Explain why lithium , sodium and potassium are put in the same group in the periodic table?

VERY IMPORTANT

A

They all have one electrone in their outer shell . the elctronic configurations are:

lithium : 2,1

Sodium, 2,8,1

Potassium 2,8,8,1

also they have similar chemical properties such as

  1. they react with water in the same way to form hydroxide with the formula MOH
  2. they react with oxygen to form oxide with the formula M2O
  3. they react with halogens to form compunds with formula MX
  4. they form ionic compunds which contain an M+ ion.
    5.
92
Q

summary of groups 1 main features

A
  1. are metals
  2. are soft with melting point and densities which are very low for metal.
  3. have to be stored out of contact with air or water
  4. react rapidly with air to form coatings of the metal oxide
  5. react with water to produce alkaline solution of the metal hydroxide and hydrogen gas
  6. increase in reactivity as you do down the group
  7. form compunds in which the metal has a 1+ ion
  8. have mainly white colourless coumpunds which dissolve to produce colourless solutions.
93
Q

find the names of the below letters

B is a metal when dropped onto water it melts into a small ball and moves rapidly around the surface , a gas C is given off and this burns with a lilac flame a solution D is formed

write the reaction equation with state symbol

A

B = Potassium

C = hydrogen

D = Potassium hydroxide KOH

2K(s) + 2H2O(l) —> 2KOH(aq) + H2(g)

94
Q

Explain why all metals in group 1 they react the same with water?

A

chemical properties depend on the number of electrons in the outer shell, and since they all have the same number of electrone in the outer shell (one) so they all have similar chemical properties and react the same with water.

95
Q

All metals in group 1 they react the same way with water

write the equation

write the equation for fracium

A

2M + 2H2O —-> 2MOH + H2

2Fr(s) + 2H2O(l) —-> 2FrOH(aq) + H2(g)

96
Q

predict the features of facium (Fr)

A

very soft

melting point is around the room temperature

has density over 2g/CM3

silvery metal tarnish instantly when cut

react with water violently forming fracium hydroxide and hydrogen

the solution FrOH is strongly alkaline

will form compounds that are white / clourless and dissolve in water giving a colourless solution.

97
Q

Congratulations you discovered a new alkali metal named Ed

is it more or less dense than fracium?

is the melting point higher or lower than fracium?

how many electrons does it have?

what is the equation to react with water?

is the solution acidic or akaline?

what is the equation to react with oxygen?

what is the equation to react with Cl

is it more or less reactive than fracium?

A

GUESS

Chemistry Y10 (5 decks)

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