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Chemistry > C1- Atomic Structure and the Periodic Table > Flashcards

C1- Atomic Structure and the Periodic Table Flashcards

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1
Q

Can you see atoms with a microscope?

A

No they are too small

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2
Q

What do atoms contain?

A

Protons ,neutrons and electrons

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3
Q

Where is the nucleus in the atom?

A

Middle

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4
Q

Where are the protons and neutrons within the atom?

A

The nucleus

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5
Q

What charge does the nucleus have?

A

Positive

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6
Q

How much of the mass of the atom is concentrated in the nucleus?

A

Almost all of it

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7
Q

What do electrons move around the nucleus in?

A

Electron shells

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8
Q

What charge do electrons have?

A

Negative

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9
Q

What changes the volume of the electrons orbit?

A

The size of the atom

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10
Q

How much mass does the electron have?

A

Virtually none

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11
Q

How many more electrons does an atom have than protons?

A

None

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12
Q

What charge do atoms have and why?

A

Neutral ,they have the same number of protons and electrons

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13
Q

In an ion does the number protons equal the number of electrons?

A

No

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14
Q

What number on each element on the periodic table describes the element?

A

Atomic number and mass number

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15
Q

What does the atomic number tell you about an atom?

A

How many protons there are

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16
Q

What does the mass number tell you about an atom?

A

The total number of protons and neutrons in the atom

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17
Q

How to get the number of neutrons?

A

Subtract the atomic number from the mass number

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18
Q

What is an element?

A

A substance made up of atoms that all have the same number of protons in their nucleus

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19
Q

How many different atomic numbers do the atoms have within the elements?

A

They are all the same

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20
Q

What within the atom nucleus determinants what type of atom it is?

A

The number of protons

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21
Q

What is a substance called if it only contains atoms with the same number of protons?

A

Element

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22
Q

How many different elements are there (roughly)?

A

100

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23
Q

What are isotopes?

A

The same as elements apart from extra neutrons

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24
Q

Do isotops have the same number of protons as the element?

A

Yes

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25
Q

Because elements can exists a number of different isotopes what is used instead of mass number?

A

Relative atomic mass

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26
Q

What is relative atomic mass?

A

An average mass taking into account the different masses and abundances (amounts) of all the isotopes that make up the element

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27
Q

What is the formula for working out the relative atomic mass of an element

A

relative atomic mass=sum of(isotope abundance x isotope mass number/sum of abundances of all the isotopes

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28
Q

What do atoms join together to make?

A

Compounds

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29
Q

What are compounds?

A

Substances formed from two or more elements, the atoms of each are in fixed proportions throughout the compound and they’re held together by chemical bonds

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30
Q

How do atoms make bonds?

A

Give away, take or share electrons

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31
Q

Are the nuclei effected by bonds made in atoms?

A

No

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32
Q

What needs to happen to separate the original element of a compound ?

A

A chemical reaction

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33
Q

What type of substance is made from a non-metal and metal?

A

An ion

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34
Q

When forming an ion does the metal loose electrons or loose them?

A

Loose

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35
Q

What does a compound made from non-metals consist of?

A

Molecules

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36
Q

What is covalent bonding?

A

Each atom shares an electron with another atom

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37
Q

Are the properties of a compound normally similar to the original element?

A

No

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38
Q

How are chemical changes shown?

A

Using chemical equations

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39
Q

Do symbol equations show the atoms on one side?

A

No ,both

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40
Q

Do symbol equations need to be balanced?

A

Yes

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41
Q

Can mixtures be easily separated?

A

Yes

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42
Q

Are there any chemical bonds between different elements in a mixture?

A

No

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43
Q

Can elements and compounds be part of a mixture?

A

Yes

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44
Q

How can u separate mixtures?

A

Physical methods

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45
Q

Name four examples of physical methods to separate mixtures?

A
  • Filtration
  • Crystallisation
  • Simple distillation
  • Fractional distillation
  • Chromatography
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46
Q

Is air a mixture, element or compound?

A

Mixture

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47
Q

What elements are in the air?

A
  • Nitrogen
  • Oxygen
  • Carbon dioxide
  • Argon
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48
Q

What is in crude oil?

A

A mixture of different length hydrocarbon molecules

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49
Q

Are the properties of mixture just a mixture of the properties of the separate parts?

A

Yes

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50
Q

When did John Dalton have theory of the atom?

A

The start of the 1800s

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51
Q

What was John Dalton’s theory of the atom?

A

He described atoms as a solid spheres and said that different spheres made up the different elements

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52
Q

What scientist had a theory on the atom in 1897?

A

J J Thomson

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53
Q

What was JJ Thomson’s theory of the atom?

A
  • Atoms weren’t solid spheres
  • He showed the atoms could contain even smaller negatively charged particles-electrons
  • he came up with the plum pudding model
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54
Q

What did the plum pudding model show?

A

The atoms as a ball of positive charge with electrons stuck in it

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55
Q

Who showed that the plum pudding model was wrong?

A

Ernest Rutherford

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56
Q

When was it shown that the plum pudding model was wrong?

A

1909

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57
Q

What experiment showed the plum pudding model was incorrect ?

A

Alpha particle scattering experiment

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58
Q

What was the alpha particle scattering experiment?

A

Ernest Rutherford and his student Ernest Marsden fired positively charged alpha particles at extremely thin sheet of gold

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59
Q

What were the people conducting the alpha particle scattering experiment expecting to happen based on the plum pudding model?

A

The particles to go straight through or be slightly deflected at most

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60
Q

What did the particles do in the alpha particle scattering experiment?

A
  • Some deflected backwards ( more than expected)
  • Most went straight through
  • A small number deflected backwards
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61
Q

What was Ernest’s Rutherford particle model called?

A

The nuclear model

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62
Q

What is the nuclear model?

A

There is a tiny positive positively charged nucleus in the centre, where most of the mass is concentrated. A ‘cloud’ of negative electrons surrounds this nucleus- so most of the atom is empty space .

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63
Q

Who realised that Ernest Rutherford’s model was incorrect?

A

Niels Bohr

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64
Q

Why did the scientist realise that Ernest Rutherford?

A

If there were a cloud of electrons they would be attracted to the nucleus causing the atom to collapse?

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65
Q

What new thing did Niels Bohr’s model have?

A

Shells and the electrons orbit the nucleus in fixed shells and aren’t anywhere in-between. Each shell in a fixed distance from the nucleus.

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66
Q

Was Neil Bohr’s model supported by experiment ?

A

Yes

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67
Q

Who showed there were protons?

A

Rutherford

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68
Q

How many years after scientists said there was a nucleus in an atom did a scientist come up with the idea that there are neutrally charged particles?

A

20

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69
Q

Who first said there neutrons?

A

James Chadwick

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70
Q

What are five electron rules?

A

-Electrons always occupy shells (sometimes called energy levels)
-The lowest energy levels are always filled first - these are the ones closest to the nucleus
-Only a certain number of electrons are allowed in each cell:
1st shell: 2 2nd shell: 8 3rd shell: 8
-Atoms are much happier when they have full electron shells- like the noble gases
-In most atoms, the outer shell is not full and this makes the atom want to react to fill it

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71
Q

What number in the first 20 elements tells you the number of protons?

A

Atomic number

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72
Q

How were elements arranged in the 1800s?

A

By atomic mass

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73
Q

Until recently what were the 2 obvious ways to categorise elements?

A
  • Their physical and chemical properties

- Their relative atomic mass

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74
Q

When did scientists realise that they could arrange elements by atomic number?

A

After they discovered protons neutrons and electrons. 20th century

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75
Q

What were the issues with early periodic tables?

A
  • They were not complete

- Some elements were placed in the wrong group

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76
Q

What did Dmitri Mendeleev do that was special when creating his periodic table?

A

He left gaps

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77
Q

In what year did Dmitri Mendeleev create his first periodic table ?

A

1869

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78
Q

How many elements were in Dmitri Mendeleev original periodic table?

A

50

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79
Q

How did Dmitri Mendeleev mainly order the elements?

A

In order of atomic mass

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80
Q

When were isotopes discovered?

A

20th century

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81
Q

What is the main reason for how elements are laid out?

A

Increasing atomic (proton) number

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82
Q

Which side of the periodic table are metals on?

A

left

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83
Q

How are elements with similar properties laid out on the periodic table?

A

They are in columns

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84
Q

What are the vertical columns called?

A

Groups

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85
Q

What does the group number tells you?

A

The number of electrons in the outer shell

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86
Q

What is the exception for the group number telling you what it tells you?

A

Group 0

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87
Q

How can you predict what the properties of one element knowing the properties of another?

A

If they are in the same group they have similar properties

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88
Q

What are rows called in the periodic table?

A

Periods

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89
Q

What do the periods tell you in the periodic table?

A

Each new period is another full shell of electrons

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90
Q

Are most elements non-metals?

A

No

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91
Q

What charge ions do metals form?

A

Positive

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92
Q

Do non-metals generally from positive ions?

A

No

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93
Q

Does the electron structure affect how the atom will react?

A

Yes

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94
Q

How do atoms generally react to form?

A

A full outer shell

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95
Q

How do atoms from a full outer shell?

A
  • Losing
  • Gaining
  • Sharing
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96
Q

If the outer shell is close to being shell how is an ion formed?

A

By getting to a full outer shell

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97
Q

Do all metals have a metallic bonding?

A

Yes

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98
Q

Are metals malleable?

A

yes

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99
Q

What does malleable mean?

A

Can be bent or hammered into shape

100
Q

Are metals strong?

A

Yes

101
Q

Are metals good at conducting heat and electricity?

A

Yes

102
Q

Do metals have a low melting or boiling point?

A

No neither

103
Q

Do non-metals have metallic bonding?

A

No

104
Q

What do non-metals tend to look like?

A
  • Dull looing

- More brittle

105
Q

Do non-metals generally conduct electricity?

A

No

106
Q

Do non-metals generally have a lower density?

A

Yes

107
Q

What groups are transition metals in?

A

2 & 3

108
Q

Are transition metals in the left right or middle of the periodic table?

A

Middle

109
Q

Are transition metals good conductors?

A

Yes

110
Q

Are transition metals dense?

A

Yes

111
Q

Are transition metals strong?

A

Yes

112
Q

Are transition metals shiny?

A

Yes

113
Q

Can transition metals only have one ion?

A

No

114
Q

Are transition metals often structured?

A

Yes

115
Q

Do transition metals often make good catalysts?

A

Yes

116
Q

What is a catalyst?

A

Something that speeds up a reaction

117
Q

Is group one acid or alkali?

A

alkali

118
Q

Are group one metals reactive for metals?

A

Yes

119
Q

What are the alkali metals?

A
  • Lithium
  • Sodium
  • Potassium
  • Rubidium
  • Caesium
  • Francium
120
Q

How many electrons do group one metals have in their outer shell?

A

One

121
Q

Are group one metals rough?

A

No, they are soft

122
Q

What type of density do alkali metals have?

A

Low

123
Q

What are the trends of group one metals as you go down the group?

A
  • Increasing reactivity
  • Lower melting and boiling points
  • Higher relative atomic mass
124
Q

What type of ions do alkali metals form?

A

Ionic compounds with non-metals

125
Q

What charge do group one ions form?

A

+1

126
Q

What do ionic compounds look like?

A

White solid

127
Q

What do ionic compounds form when they dissolve in water?

A

Colourless solutions?

128
Q

Do ionic compounds dissolve in water?

A

Yes

129
Q

What do group one metals from with water?

A

Hydrogen gas and metal hydroxides

130
Q

What are metal hydroxides?

A

Salts that dissolve in water to produce alkaline

131
Q

The more reactive the group one metal the more violent the reaction: True/False

A

True

132
Q

What does the amount of energy of during a reaction tell you anything about the group?

A

The amount if energy given of during a reaction as you go down the group

133
Q

Metal + water ->

A

Metal hydroxide + hydrogen

134
Q

What do group one metals do while reacting with chlorine gas?

A

React vigorously

135
Q

Metal + Chlorine->

A

Metal chloride

136
Q

Metal react with chlorine gas to form…?

A

White metal chloride salts

137
Q

What do group one metals react with oxygen to form?

A

Metal oxides

138
Q

What does sodium react with oxygen to form?

A

A mixture of sodium oxide and sodium peroxide

139
Q

What does potassium react with oxygen to form?

A

A mixture potassium peroxide and potassium superoxide

140
Q

Do group one metals have similar properties to transition metals?

A

No

141
Q

Which is more reactive transition metals or group one metals?

A

Group one

142
Q

Are transition metals less dense, strong and hard than group one metals?

A

No

143
Q

Who has a lower melting point group one metals or transition metals?

A

Group one metals

144
Q

What is manganese’s melting point?

A

2000 degrees Celsius

145
Q

What is the boiling point of sodium?

A

98 degrees Celsius

146
Q

What are group 7 metals called?

A

The halogens

147
Q

Are any of the halogens metals?

A

No

148
Q

Is fluorine very reactive?

A

Yes

149
Q

What colour is fluorine?

A

Yellow

150
Q

Is fluorine harmless?

A

No, it is poisonous

151
Q

What state is fluorine?

A

Gas

152
Q

Is chlorine non reactive?

A

No, it is fairly reactive

153
Q

What state is chlorine

A

Dense gas

154
Q

Is chlorine harmful?

A

Yes it is poisonous

155
Q

Is bromine dense?

A

Yes

156
Q

Is bromine poisonous?

A

Yes

157
Q

What colour is bromine?

A

Red-brown volatile

158
Q

What state is bromine?

A

Liqued

159
Q

What is one colour and state is iodine?

A

Dark grey and crystalline solid or purple vapour

160
Q

Are any of the halogens molecules?

A

All of them

161
Q

What happens when you go down group 7?

A
  • Become less reactive- it’s harder to gain an extra electron, because the outer shell’s further from the nucleus.
  • Have higher melting and boiling points.
  • Have higher relative atomic masses.
162
Q

Do group 7 elements react very differently to each other?

A

No

163
Q

Why do group 7 elements all react similarly?

A

Because they all have seven electrons in their outer shell

164
Q

Can halogens form molecular compounds?

A

Yes

165
Q

Halogen atoms can share electron via…

A

Covalent bonding

166
Q

Why do group 7 elements react with non-metals?

A

In order to achieve a full outer shell

167
Q

Do compounds that form halogens have a complex molecular structures?

A

No, they are simple

168
Q

What do halogens form with ionic bonds?

A

Metals

169
Q

What is the charge of halogens ions?

A

-1

170
Q

What are the halogen ions called?

A

Halides

171
Q

What type of structure do halogen compounds have?

A

Ionic structures

172
Q

What will more reactive halogens do to less reactive ones?

A

They displace

173
Q

What are group 7 elements called?

A

Noble gases

174
Q

What is the colour of group 0 elements?

A

Colourless

175
Q

How many electrons are in the outer shell of the noble gasses (apart from helium)?

A

8

176
Q

Are the noble gasses reactive?

A

No

177
Q

Are noble gasses monatomic gases?

A

Yes

178
Q

What state are group 0 at room temperature?

A

Gasses

179
Q

Are noble gasses flammable?

A

No

180
Q

Are their properties patterns in the noble gasses?

A

Yes

181
Q

Does the boiling point go up or down as you go down group 0?

A

Up

182
Q

Why does the boiling point go up as you go down noble gasses?

A

Due to an increase in the number of electrons in each atom leading to greater intermolecular forces between which need to overcome. There’s more on intermolecular forces for small molecules

183
Q

What is an atom

A

An atom is the smallest part of an element what can exist

184
Q

Elements can be classified into two groups based on

their properties; what are these groups

A

Metals and non-metals

185
Q

Elements may combine through chemical reactions
to form new products; what are these new
substances called?

A

Compounds

186
Q

Do compounds have the same properties as their

constituent elements

A

No, they have different properties

187
Q

What is a mixture? Does it have the same chemical

properties as its constituent materials

A

A mixture consists of two or more elements or compounds not chemically
combined together; it does have the same chemical properties

188
Q

What are the methods through which mixtures
can be separated (there are five)? Do these
involve chemical reactions

A

Filtration, crystallisation, simple distillation, fractional distillation and
chromatography; they do not involve chemical reactions

189
Q

Describe and explain simple distillation

A

Simple distillation is used to separate liquid from a solution – the liquid
boils off and condenses in the condenser. The thermometer will read the
boiling point of the pure liquid. Contrary to evaporation, we get to keep the
liquid.

190
Q

Describe and explain crystallisation/evaporation

A

Evaporation is a technique for separation of a solid dissolved in a solvent from a
solvent (e.g. salt from H2O).
The solution is heated until all the solvent evaporates; the solids stays in the vessel.
Crystallisation is similar, but we only remove some of the solvent by evaporation to
form a saturated solution (the one where no more solid can be dissolved). Then,
we cool down the solution. As we do it, the solid starts to crystallise, as it becomes
less soluble at lower temperatures. The crystals can be collected and separated
from the solvent via filtration.

191
Q

Describe and explain fractional distillation

A

Fractional distillation is a technique for separation of a mixture of liquids.
It works when liquids have different boiling points.
The apparatus is similar to the one of simple distillation apparatus, with the
additional fractionating column placed on top of the heated flask.
The fractionating column contains glass beads. It helps to separate the compounds.
In industry, mixtures are repeatedly condensed and vapourised. The column is hot at
the bottom and cold at the top. The liquids will condense at different heights of the

192
Q

Describe and explain filtration

A

Filtration is used to separate an insoluble solid is suspended in a liquid.
The insoluble solid (called a residue) gets caught in the filter paper,
because the particles are too big to fit through the holes in the paper.
The filtrate is the substance that comes through the filter paper.
Apparatus: filter paper + funnel.

193
Q

Describe and explain chromatography

A

Chromatography is used to separate a mixture of substances dissolved in a solvent.
In paper chromatography, we place a piece of paper with a spot containing a mixture
in a beaker with some solvent. The bottom of the paper has to be in contact with
the solvent. The solvent level will slowly start to rise, thus separating the spot
(mixture) into few spots (components).

194
Q

What is a separating funnel?

A

A separatory funnel is an apparatus for separating immiscible liquids.
Two immiscible liquids of different densities will form two distinct layers in
the separatory funnel.
We can run off the bottom layer (the liquid with greater density) to a
separate vessel.

195
Q

Describe the plum-pudding model

A

The atom is a ball of positive charge with negative electron embedded in
it.

196
Q

Describe the Bohr/nuclear model and how it

came about

A

The nuclear model suggests that electrons orbit the nucleus at specific
distances (shells) – it came about from the alpha scattering experiments

197
Q

Later experiments led to the discovery of
smaller, positive particles in the nucleus; what
are these particles called?

A

Protons

198
Q

What did the work of James Chadwick provide

evidence for

A

The existence of neutrons in the nucleus

199
Q

Describe the structure of an atom

A

The atom has a small central nucleus (made up of protons and neutrons)
around which there are electrons

200
Q

State the relative masses and relative charges

of the proton, neutron and electron

A

Masses: 1, 1, very small ; Charges: 1, 0 , -1 (respectively)

201
Q

Explain why atoms are electrically neutral.

A

They have the same number of electrons and protons

202
Q

What is the radius of an atom

A

0.1 nm

203
Q

What is the radius of a nucleus and what is it

compared to that of the atom?

A

1 x 10-14 m and 1/10 000

204
Q

What name is given to the number of protons in

the nucleus

A

Atomic number

205
Q

Atoms of the same element have the same

number of which particle in the nucleus?

A

Protons

206
Q

Where is the majority of mass of an atom?

A

The nucleus

207
Q

What is the mass number?

A

The total number of protons and neutrons

208
Q

How does one calculate the number of neutrons

using mass number and atomic number

A

Subtract the atomic number from the mass number

209
Q

What is an isotope? Do isotopes of a certain

element have the same chemical properties?

A

Atoms of the same element (same proton number) that have a different
number of neutrons.
They have the same chemical properties as they have the same
electronic structure

210
Q

What is the relative atomic mass

A

The average mass value which takes the mass and abundance of isotopes
of an element into account, on a scale where the mass of 12C is 12.

211
Q

He, Be, F, Na, Ca configurations (respectively):

A 
2
 2,2
 2,7
 2,8,1
 2,8,8,2
212
Q

What are ions

A

Ions are charged particles. They are formed when atoms lose electrons
(positive ions) or gain (negative ions) electrons.
E.g. sodium positive ion, Na+
, has an electronic configuration of 2,8 (same
as Ne). An atom of sodium has lost one electron.

213
Q

What is formed when a metal reacts with a

non-metal?

A

An ionic compound (made of positive and negative ions).

214
Q

What is formed when a non-metal reacts with a

non-metal?

A

A molecular compound containing covalently bonded atoms.
Atoms share electrons, as opposed to transferring electrons between
each other (cf. ionic compounds).

215
Q

Explain the following: solute, solvent, solution,

miscible, immiscible, soluble, insoluble.

A

A solute is a substance that is dissolved in a solvent. Together, they form a
solution.
Miscible refers to the substances (particularly liquids) that mix together, e.g. water
and alcohol. Water and oil are immiscible, i.e. they do not mix.
Soluble refers to the substance that can be dissolved in a solvent, e.g. salt in
water. Insoluble substance won’t dissolve in a particular solvent.

216
Q

The columns of the periodic table are called?

A

Groups

217
Q

The rows of the periodic table are called…?

A

Periods

218
Q

Are elements in the same

group similar or different

A

They may have similar chemical properties, as they have the same
number of outer shell electrons.

219
Q

In terms of energy levels, what are the
differences between elements of the same
period?

A

They have the same number of energy levels

220
Q

Electrons occupy particular energy levels, with each
electron in an atom at a particular energy level; which
available energy level do electrons occupy?

A

The lowest available energy level

221
Q

The elements of Group 0 are more commonly

known as…?

A

The noble gases

222
Q

What makes the periodic

table periodic?

A

Similar properties of elements occur at regular intervals

223
Q

Elements in the same group have the same
number of electrons in their outer shell; what
does this tell us about their chemical properties?

A

They have similar chemical properties

224
Q

In terms of shells, what is the difference

between elements in the same period?

A

They have the same number of shells

225
Q

What change in shell number is seen as one

moves down a group?

A

The number of shells increases

226
Q

Early periodic tables were incomplete and
elements were placed in inappropriate groups if
what was to be followed?

A

The strict order of atomic weights

227
Q

Knowledge of what made it possible to explain
why the order based on atomic weights was not
always correct?

A

Isotopes

228
Q

Mendeleev overcame some problems with the
table by doing what? He also changed the order
of some elements based on what

A

Leaving gaps; atomic weights

229
Q

The majority of elements are…?

A

Metals

230
Q

Elements that react to form positive ions are…?

A

Metals

231
Q

Elements that do not form positive ions are…?

A

Non-metals

232
Q

Elements in Group 1 are known as…?

A

The alkali metals

233
Q

State three characteristics of the Alkali Metals

A

All have one electron in their outer shell; have low density; are stored
under oil (to prevent reactions with oxygen or water); are soft (can be cut
with knife)

234
Q

How do Group 1 elements react with
non-metals? Why are these reactions similar for
the different Group 1 elements?

A

They form ionic compounds which are soluble white solids which form
colourless solutions – they all have one electron in their outer shell.

235
Q

How do Group 1 elements react with water?

A

They release hydrogen and form hydroxides which dissolve to form
alkaline solutions; react vigorously with water fizzing and moving around
on the surface of the water.

236
Q

How does reactivity change moving down Group

1? Why?

A

Reactivity increases as the atoms get larger and the distance between
the nucleus and the outer electrons increases and thus attraction from the
nucleus decreases, allowing them to more easily lose electrons.

237
Q

State five characteristics of Group 7

A
  • 7 electrons in outer shell
  • Coloured vapours
  • Diatomic molecules
  • Form ionic salts with metals
  • Form molecular compounds with non-metals
238
Q

State five State Group 7 elements and states of

matter of molecules they form

A 
- Fluorine, F. F2
 is a pale yellow gas.
- Chlorine, Cl. Cl2
 is a pale green gas.
- Bromine, Br. Br2
 is dark brown liquid
- Iodine, I. I2
 is a grey solid.
239
Q

State three changes that occur in Group 7 as

one moves down the group

A
  • Higher relative molecular mass
  • Higher melting and boiling point
  • Less reactive – less easily gain electrons
240
Q

A more reactive halogen displaces a less reactive one from
an aqueous solution of its salt; write the equations and state
the colour change seen when chlorine reacts with sodium
bromide and when chlorine/bromine reacts with sodium
iodide.

A 
2
 \+ 2 NaBr → Br2
 \+ 2 NaCl, or
 Cl2
 \+ 2Br– → Br2
 \+ 2 Cl–
;
in this reaction, an orange colour of Br2
 would appear
Cl2
 \+ 2 NaI → I2
 \+ 2 NaCl, or Cl2
 \+ 2I–
 → I2
 \+ 2 Cl–
 Br2
 \+ 2 NaI → I2
 \+ 2 NaBr, or Br2
 \+ 2I–
 → I2+ 2 Br–
;
 in these two reactions, a brown colour of I2
 would appear
241
Q

A more reactive halogen displaces a less
reactive one from an aqueous solution of its salt;
explain the trend in reactivity of halogens in these
reactions

A

Reactivity decreases down the group. As we go down the group, the atoms
get larger, so an incoming electron will be less tightly held by the attractive forces
from the nucleus. That’s why Cl2
displaces Br–
and I–
.

242
Q

Compare group 1 metals with transition metals

A

Group 1 metals and transition metals are heat and electricity conductors.
They are shiny when polished and form ionic compounds with non metals.
Transition metals have higher densities and higher melting points than Group
1 metals. They are less reactive and harder than Group 1 metals.

243
Q

State three common characteristics of transition

metals

A
  • Ions with different charges
  • Coloured compounds
  • Catalytic properties
244
Q

What is a catalyst?

A

A catalyst is a chemical substance that increases the rate of a
chemical reaction.
It is not used up over the course of the reaction.

245
Q

State the colours of flames observed when lithium,

sodium, and potassium burn in oxygen

A

Crimson-red, Li
Yellow-orange, Na
Lilac, K

Chemistry (10 decks)

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