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C1 > C1 > Flashcards

C1 Flashcards

1
Q

What is an element

A

All atoms are the same

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2
Q

How many elements are in the periodic table

A

100

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3
Q

What does each element represent

A

Different atoms with different symbols

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4
Q

What is a compound

A

Two or more elements chemically combined in a fixed proportion

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5
Q

What do we do to break compounds back into elements

A

We use chemical reaction

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6
Q

Different elements or compounds NOT chemically combined together

A

Mixtures

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7
Q

If we want to separate a ——- then we use physical techniques

A

Mixture

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8
Q

What physical techniques do we use to separate a mixture

A

Filtration crystallisation,distillation

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9
Q

Define molecule

A

Any elements chemically joined,can be same element unlike compound which needs different ones

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10
Q

What is an atom

A

Smallest part of an element, no overall electrical charge,all substances are made of atoms

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11
Q

Radius of an atom

A

0.1nm

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12
Q

What are physical separation techniques used for

A

Mixtures

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13
Q

What can physical techniques not be used to separate and why?

A

Elements in a compound because they are chemically combined in a fixed proportion

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14
Q

What is filtration

A

Used to separate insoluble solid from liquid

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15
Q

What is crystallisation

A

Used to separate soluble solid from liquid

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16
Q

What is simple distillation

A

Used to separate liquid from solid if we want to keep liquid

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17
Q

What is fractional distillation

A

Allows us to separate 2 different liquids

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18
Q

What is chromatography

A

Physical process used to separate mixtures

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19
Q

What does chromatography work

A

Because each chemical in mixture is attracted to the stationary phase to a different extent

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20
Q

What are atoms not

A

Divisible

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21
Q

Who invented the plumb pudding model

A

JJ Thompson

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22
Q

What does the plum pudding model show

A

An atom is a ball of positive charge with negative electrons embedded in it. Was WRONG!

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23
Q

Who did the alpha scattering experiment

A

Rutherford

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24
Q

Why did Rutherford experiment using a piece of gold foil

A

Can be hammered down to be a few atoms thick

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25
Q

Results from alpha scattering experiment (3 marks)

A
  • most alpha particles went straight through the gold atoms
    -some deflected (changed direction)
    -bounced straight back
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26
Q

Most alpha particles went straight through gold atoms. Why?

A

Atoms are mainly empty space

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27
Q

Some alpha particles defelcted. Why?

A

Centre of atom must have positive charge- alpha particles close to this repell/ change direction

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28
Q

Alpha particles bounced straight back. Why?

A

Centre of atom must contain great deal of mass- now call this a nucleus

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29
Q

What did James chadwick discover

A

Nucleus also contained neutral particles called neutrons

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30
Q

Example of substance that you can filter

A

Silver chloride + water
AgCl= solid
H20= liquid

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31
Q

Example of substance you can crystallise

A

Sodium chloride + water
NaCl = aqueous- forms crystals
H20= water- evaporates

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32
Q

Equipment needed for filtration

A

Filter paper
Filter funnel
Beaker

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33
Q

Equipment needed for crystallisation

A

Beaker
Evaporating basin
Bunsen burner- if u wish to heat substance- don’t over heat otherwise compounds will start to break down

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34
Q

How does simple distillation work

A
  • First evaporate liquid by heating
  • we then condense water by cooling
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35
Q

Can fractional distillation work if liquids have same m.p/ b.p

A

No, otherwise we won’t be able to collect pure form

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36
Q

What is fractional distillation used for

A

To purify larger volumes of liquid e.g. crude oil- requires different equipment but principle is same

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37
Q

How do you know if a chemical is pure in chromatography?

A

Will produce a single spot in all solvents

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38
Q

What chemicals will move further up chromatography paper?

A

Chemicals that are weakley attracted to stationary phase

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39
Q

Why do we draw a line in pencil on chromatography paper

A

It’s insoluble

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40
Q

What is the solvent called in chromatography

A

Mobile phase because it doesn’t move

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41
Q

Soluble meanning

A

Can dissolve in water

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42
Q

Insoluble meanning

A

Can’t dissolve in water

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43
Q

Solute meanning

A

Dissolved in solvent

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44
Q

Solvent meaning

A

Dissolves solute resulting in solution

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45
Q

What’s the nuclear model (3)

A
  • negative electrons around the edge
  • tiny positive nucleus
  • empty space
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46
Q

What was Niels Bohr model

A
  • belived electrons orbited nucleus at specific distance (now call this orbit or energy levels/shells)
  • several years later discovered protons- positive charge in nucleus
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47
Q

What was the final version of nuclear model

A
  • atoms have no overall charge because number of electrons is the same as number of protons
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48
Q

What is radius of nucleus

A

1 x 10 ^ -14

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49
Q

Relative charge and mass of protons

A

Charge= +1
Mass= 1

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50
Q

Relative charge and mass of neutrons

A

Charge= 0
Mass= 1

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51
Q

Relative charge and mass of electrons

A

Charge= -1
Mass= very small

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52
Q

How does energy progress through the outer shells

A

shell- further away from nucleus= higher energy

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53
Q

What charge does the nucleus overall have

A

Positive because of protons

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54
Q

What happens if an atom absorbs electromagnetic radiation

A

An electron can move from a lower energy shell to a higher energy shell/level

55
Q

How can electrons change energy levels/ shells

A

By absorbing or emitting electromagnetic radiation

56
Q

What is the structure of how many electrons can be present in each shell

A

2, 8,8,18

57
Q

The group number represents…

A

The number of electrons on outer shell

58
Q

What is the relative atomic mass

A

Protons and neutrons- the bigger number

59
Q

What is the atomic number

A

Smaller number

60
Q

What did Döbereiner discover

A
  • elements with similar properties occurred in 3s [triads]
  • e.g. Lithium, sodium, potassium (all react rapidly with water)
  • Chlorine, Bromine, Iodine (all reactive non-metal)
61
Q

Work of Newlands…

A

Octaves

62
Q

What was Newlands law of octaves

A
  • arranged elements in order of Increasing atomic weight- every 8th reacts in similar way
  • e.g. lithium, sodium, potassium
63
Q

What was the problem with Newlands discovery

A
  • by always sticking to exact order of atomic weight sometimes elements were grouped together when they had different properties
64
Q

Who was the Russian scientist

A

Dmitri Mendeleeve

65
Q

What did Mendeleeve do

A
  • arranged elements by order of Increasing atomic weight
  • If needed he would switch order of elements to fit pattern of other elements in same group
  • realised some elements had not been discovered so left gaps in periodic table
66
Q

What 3 things did Mendeleeve do that no other scientist did

A
  • would switch order of specific elements to fit partern of other elements in same group
  • realised some elements had not been discovered- left gaps
  • predicted properties of undiscovered elements based on the group- he was correct elements discovered fit his periodic table
67
Q

What are the differences between Mendeleevs table and modern periodic table

A
  • protons had not been discovered- he ordered them with atomic weight ( elements could be in wrong order due to isotopes)
  • modern includes noble gases which weren’t fully discovered when Mandeleev published his table
68
Q

What are group 0 known as

A

Noble gases- monatomic gases (singles atoms- not bonded)

69
Q

How many electrons do nobles gases have in outer shell

A

8- full, energetically stable except helium which has 2

70
Q

List properties of Group 0 (4)

A
  • inert: don’t react, non flammable
  • colourless gases
  • do not form molecules
  • unreactive elements
71
Q

What is the trend in noble gases (4 marks)

A

Boiling point Increases as you move down the group along with relative atomic mass
- atoms become larger intermolecular forces between atoms gets stronger- more energy Is needed to overcome the forces

72
Q

Why does Boiling point Increases as you move down group 0

A
  • atoms become larger intermolecular forces between atoms gets stronger- more energy Is needed to overcome the forces
73
Q

How do noble gases react

A

Very unreactive as they have full outer shell

74
Q

What are group 1 known as

A

Alkali metals

75
Q

Group 1 have …. electrons in outer shell

A

1

76
Q

How reactive are group 1 elements

A

Very reactive because they can lose the one electron in outer shell

77
Q

Properties of Group 1 elements

A
  • soft (can be cut with a knife)
  • low density (first 3 are less dense than water)
  • low m.p and b.p- decreases down the group
  • form ionic compounds with non- metals
78
Q

Describe the trend in group 1 elements

A
  • Increasing reactivity as you move down the group- outer electron is more easily lost as attraction between the nucleus and electron decreases as electron is further from nucleus
  • hence electron is lost easier as you move down group
  • lower m.p. and b.p. as you move down
  • higher relative atomic mass- atoms become larger
79
Q

List the reactions of group 1 elements with water, oxygen and chlorine

A

Metal + water = metal hydroxide and hydrogen
Metal + oxygen= Metal oxide
Metal + chlorine = Metal chloride

80
Q

Lithium + water =?

A

Lithium hydroxide + hydrogen

81
Q

What is the formula for lithium reacting with water

A

2Li + 2H₂0 = 2LiOH + H₂

82
Q

What are the observations for when lithium reacts with water

A
  • fizzes steadily but furiously along surface
  • slowly becomes smaller until dissappears
83
Q

Sodium + water =?

A

Sodium hydroxide + hydrogen

84
Q

Formula for sodium reacting with water

A

2Na +2H₂0 =2NaOH + H₂

85
Q

What’s the observations when sodium reacts with water

A
  • fizzes rapidly, melts to form a ball
  • quickly becomes smaller until it dissappears- more violent than lithium
86
Q

Potassium + water =?

A

Potassium hydroxide + hydrogen

87
Q

Formula of potassium reacting with water

A

2K + 2H₂0 = 2KOH + H₂

88
Q

Observations made when potassium reacts with water

A
  • burns violently with a spark and lilac flame
  • quickly melts to form a ball
  • dissappears rapidly often with small explosion
  • hot enough to ignite hydrogen gas
  • very violent
89
Q

Lithium + chlorine

A

Lithium chloride

90
Q

Formula for lithium and chlorine

A

2Li + Cl₂ = 2LiCl

91
Q

Sodium + chlorine

A

Sodium chloride

92
Q

Potassium + Chlorine

A

Potassium Chloride

93
Q

Formula for sodium and chlorine

A

2Na + Cl₂ = 2NaCl

94
Q

Formula for potassium and chlorine

A

2K + Cl₂ = 2KCl

95
Q

Observations made during reaction of lithium, potassium and sodium with chlorine

A
  • act vigorously when heated in chlorine gas to form white metal chloride salts
  • as you move down relativity increases so reaction with chlorine gas gets more vigorous
96
Q

Lithium + oxygen

A

Lithium oxide

97
Q

Sodium + oxygen

A

Sodium oxide

98
Q

Potassium + oxygen

A

Potassium oxide

99
Q

Formula for lithium reacting with oxygen

A

4Li + O₂ = 2Li₂O

100
Q

Formula of sodium reacting with oxygen

A

4Na + O₂ = 2Na₂O

101
Q

Formula for when potassium reacts with oxygen

A

4K + O₂ = 2K₂O

102
Q

Observations made when group 1 alkaline metals react with oxygen

A
  • burn vigorously when heated and placed in a gas jar of oxygen
  • oxide forms white smoke
  • as reactivity increases down group so does reaction with oxygen
103
Q

What are group 7 called

A

Halogens

104
Q

How are halogens found

A

Diatomic molecules joined together by single covalent bond

105
Q

Properties of Group 7 [7]

A
  • non metals
  • coloured vapours: poisonous
  • diatomic molecules
  • form 1- ions
  • ionic bonds with metal halide
  • displacement reaction can occur between more reactive halogen and salt of less reactive one
  • all have 7 electrons in outer shell
106
Q

What colour is fluorine gas

A

Yellow- very reactive

107
Q

What colour is chlorine gas

A

Dense green gas- fairly reactive

108
Q

What colour is bromine

A

Red brown volatile liquid= dense

109
Q

What colour is iodine

A

Purple vapour- dark grey crystalline solid

110
Q

What happens to molecules as you move down group 7

A

Molecules become larger, intermolecular forces become stronger, more energy Is needed to overcome these forces

111
Q

What happens to reactivity as you move down group 7

A
  • halogens become less reactive- harder to gain extra electron because outer shell Is further from nucleus
112
Q

What happens to m.p and b.p as you move down group 7

A

Increases along with relative atomic mass

113
Q

At room temperature what is Flourine

A

Gas

114
Q

At room temperature what is chlorine

A

Gas

115
Q

At room temperature what is Bromine

A

Liquid

116
Q

At room temperature what is Iodine

A

Solid

117
Q

What happens when halogens react with metals

A
  • produce salt- made of ions which are held together by ionic bonding
118
Q

What does Halogen mean

A

Salt producing

119
Q

What happens as you move down group 7 to the reactivity

A

Reactivity of elements decreases down group

120
Q

What happens to force of attraction as you move down group 7

A

Force of attraction between nucleues and outer shell decreases

121
Q

What happens when halogen reacts with hydrogen

A

Product= Compound called hydrogen halide
- gases at room temperature + dissolve in water to produce acidic solutions

122
Q

What do group 7 form when they react with other non- metal atoms

A

Covalent compounds

123
Q

In this reaction what is displaced:
Sodium bromide + fluorine = sodium fluoride + Bromine

A
  • fluorine displaces Bromine
  • because fluorine is more reactive than Bromine
124
Q

What do group 7 elements form when they react with metals

A

Ionic compounds

125
Q

What bonds do group 7 make

A

Ionic bonds with metal halide

126
Q

What do group 1 elements form

A

Ionic bonds with non metals

127
Q

Define Isotope

A

Atoms have same number of protons and electrons but different number of neutrons

128
Q

Do isotopes have same chemical properties

A

Yes because they have same electronic structure

129
Q

How do you find the relative atomic mass of isotopes

A

(Isotopic mass x%abundance ) +(Isotopic mass x % abundance) /100

E.g. chlorine has 2 isotopes
Cl 35- 75%
Cl 37- 25%

[(75 x 35) + (25 x 37)] /100
= 35.5

130
Q

What elements react to form positive ions

A

Metals

131
Q

What elements do not form positive ions

A

Non- metals except hydrogen

132
Q

Compare transition metals with group 1 metals

A
  • have higher m.p. (except Mercury)
  • have higher densities
  • are stronger
  • are harder
  • much less reactive so do not react as vigorously with oxygen or water
133
Q

Properties of transition metals

A
  • have ions with different charges
  • form coloured compounds
  • useful as catalysts

C1 (5 decks)

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