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GCSE Revision Flashcards > C1 Atomic Structure > Flashcards

C1 Atomic Structure Flashcards

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1
Q

What are group 1 metals known as?

A

Alkali Metals

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2
Q

Looking down group 1, do the metals get more or less reactive?

A

More reactive

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3
Q

What happens when alkali metals react with water?

A

Rapid reaction, producing an alkaline solution and hydrogen gas

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4
Q

What are group 7 elements known as?

A

Halogens

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5
Q

Name the 2 halogens which are gases:

A

Fluorine and Chlorine

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6
Q

What is the Halogen, Bromine?

A

One of only 2 liquid elements in Group 7

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7
Q

What is the Halogen, Iodine?

A

A solid

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8
Q

Do halogens exist as monatomic or diatomic molecules?

A

Diatomic

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9
Q

What are the elements in group 0 known as?

A

Noble Gases

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10
Q

What are diatomic molecules?

A

2 atoms in each molecule

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11
Q

Looking down group 7, do the elements get more or less reactive?

A

Less reactive

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12
Q

Are Noble Gases monatomic or diatomic?

A

Monatomic

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13
Q

What are monatomic elements?

A

Elements which exist as individual atoms

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14
Q

How reactive are Noble Gases and why?

A

They are unreactive as they have a full outer shell of electrons

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15
Q

Where are transition metals found on the periodic table?

A

Groups 2 and 3

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16
Q

Give 3 examples of transition metals:

A

Iron, copper and gold

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17
Q

What are the properties of transition metals? Are they dense? What types of compounds do they form?

A

Generally quite dense (heavy) and may form brightly coloured compounds

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18
Q

How is the periodic table ordered?

A

In order of increasing atomic number

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19
Q

What are the horizontal rows on the periodic table called?

A

Periods

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20
Q

What are the vertical columns on the periodic table called?

A

Groups

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21
Q

Why do elements in the same group have similar chemical properties?

A

They have the same number of outer electrons and the same valency

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22
Q

How many elements are represented by the periodic table?

A

Over 100

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23
Q

What does the structure of the atom impact?

A

Everything in the world is made of atoms. The structure of the atom is what gives the element its chemical and physical properties.

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24
Q

What are electrons?

A

Negatively charged particles that spin around the positive centre of the atom in circles called energy levels

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25
Q

What is the mass of an electron?

A

0 - so small it is nearly 0

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26
Q

What are protons?

A

Positively charged particles that are contained in the nucleus of the atom (the centre)

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27
Q

What is the mass of a proton?

A

1 amu (atomic mass unit)

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28
Q

What are neutrons?

A

Particles with no charge that are also contained in the nucleus of the atom.

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29
Q

What is the mass of a neutron?

A

1 amu (atomic mass unit)

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30
Q

What is the charge of an electron?

A

-1

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31
Q

What is the charge of a proton?

A

+1

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32
Q

What is the charge of a neutron?

A

0

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33
Q

What is the overall charge of every atom?

A
  1. Every atom has no overall charge. While atoms do contain charged particles, they have the same number of positive protons and negative electrons which cancel out causing a neutral charge
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34
Q

What is the atomic number?

A

Number describing how many protons that element has (and also number of electrons)

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35
Q

What is the mass number?

A

Number referring to the number of protons + neutrons in an atom

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36
Q

What is an isotope?

A

An atom with the same atomic number but different mass number

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37
Q

What is an atom?

A

The smallest amount of an element that can still be recognised as that element

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38
Q

What is an element?

A

A substance made up of only one type of atom. An element cannot be broken down into any simpler substance

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39
Q

What is a compound?

A

A substance made up of 2 or more elements chemically bonded together

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40
Q

What is an ion?

A

A charged particle produced by the loss or gain of electrons

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41
Q

What is an isotope?

A

Atoms that have the same number of protons but a different number of neutrons. SAME ATOMIC NUMBER, DIFFERENT MASS NUMBERS

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42
Q

What is the nucleus (of an atom)?

A

The very small and dense centre part of an atom - contains protons and neutrons

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43
Q

What is a shell?

A

An area in an atom around its nucleus where electrons are found

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44
Q

What are fullerenes?

A

Hollow shaped molecules made up of carbon atoms

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45
Q

Give the name of the most common fullerene:

A

C60 Buckminsterfullerene - contains 60 carbon atoms (hence the name)

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46
Q

What is the charge of a proton?

A

+1

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47
Q

What is the mass of a proton?

A

1

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48
Q

What is the charge of an electron?

A

-1

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49
Q

What is the mass of an electron?

A

0 (1/2000th)

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50
Q

What is the charge of a neutron?

A

0

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51
Q

What is the mass of a neutron?

A

1

52
Q

What is a giant lattice structure?

A

A huge 3D network of atoms or ions, such as a GIANT COVALENT STRUCTURE

53
Q

What is a giant covalent structure?

A

A huge 3D network of covalently bonded atoms

54
Q

What are simple molecules?

A

Made when a few non-metal atoms join with strong covalent bonds

55
Q

What is electrostatic attraction?

A

The pulling force between positive and negative particles. Similar to magnet forces (North -> South)

56
Q

What are intermolecular forces?

A

The attraction between simple molecules

57
Q

What is a delocalised electron?

A

An electron that is no longer associated with one particular atom. It can move around and carry a charge

58
Q

What is a neutron?

A

A dense particle found in the nucleus of an atom. It is electrically neutral, carrying no charge

59
Q

What is a proton?

A

A tiny positive particle found inside the nucleus of an atom

60
Q

What is an electron?

A

A tiny particle with a negative charge. Electrons orbit the nucleus of atoms or ions in shells

61
Q

What type of bonding is METAL + NON-METAL?

A

Ionic

62
Q

What type of bonding is METAL + METAL

A

Metallic

63
Q

What type of bonding is NON-METAL + NON-METAL?

A

Covalent

64
Q

Can ionic substances conduct electricity?

A

When molten or in solution

65
Q

Do ionic substances have high/low melting and boiling points?

A

High melting/boiling points

66
Q

What did John Dalton say in 1808?

A

Atoms were tiny solid spheres which can’t be divided

67
Q

What did J.J. Thompson say in 1897?

A

Discovered electrons - theorised it was a ball of positive charge with electrons randomly embedded in it

68
Q

Who came up with the plum pudding model?

A

J.J. Thompson

69
Q

What did Rutherford say in 1909?

A

Observed that after firing alpha particles at gold foil, some were deflected - must be a nucleus in the centre where mass is concentrated

70
Q

Who came up with the nuclear model?

A

Earnest Rutherford

71
Q

What did Niles Bohr say in 1913?

A

Electrons were organised in shells/energy levels - orbit at fixed distances

72
Q

Who came up with the Bohr model?

A

Niles Bohr

73
Q

What did James Chadwick do in 1932?

A

Discovered the neutron and added it to the nucleus of an atom

74
Q

What is the charge of a proton?

A

+1

75
Q

What is the mass of a proton?

A

1

76
Q

What is the charge of an electron?

A

-1

77
Q

What is the mass of an electron?

A

0 (1/2000th of an atom)

78
Q

What is the charge of a neutron?

A

0

79
Q

What is the mass of a neutron?

A

1

80
Q

Which number is the atomic number?

A

Bottom number

81
Q

Which number is the atomic mass?

A

Top number

82
Q

What is the relative atomic mass?

A

Mean average mass of all isotopes in that element

83
Q

What is the equation for calculating relative atomic mass?

A

(mass isotope 1 x % isotope 1) + (mass isotope 2 x % isotope 2) / 100

84
Q

What are the 3 things John Dalton did to develop the periodic table?

A
  1. Gave each element a drawing/symbol
  2. Ordered list by atomic mass
  3. Periodic table arranged in a perfect square
85
Q

What are the 3 things John Newland did to develop the periodic table?

A
  1. Used letter symbols over drawings
  2. Ordered by octave’s law (a failed theory). Where it didn’t apply, he added a seemingly random element
  3. Periodic table arranged a perfect square
86
Q

What are the 3 things Dmitri Mendeleev did to develop the periodic table?

A
  1. Elements ordered by atomic number
  2. Left gaps for undiscovered elements - predictions of properties came true
  3. Not arranged in a perfect square arrangement
87
Q

What is an isotope?

A

An atom of the same element with the same number of protons and a different number of neutrons - different relative atomic mass

88
Q

What is a metallic bond?

A

Electrostatic attraction between positive metal ions and delocalised electrons

89
Q

What is a covalent bond?

A

A shared pair of electrons

90
Q

What is an ionic bond?

A

Strong electrostatic attraction between oppositely charged ions

91
Q

What is an ion/how is it formed?

A

Atoms with a positive or negative charge formed when atoms gain or lose electrons to form a full outer shell

92
Q

Which group on the periodic table is Halogens?

A

7

93
Q

What is the charge of a Halogen - Group 7?

A

-1

94
Q

What is the trend of reactivity for Group 7 (Halogens)?

A

The lower down the group, the darker the colour and the higher the melting/boiling point

95
Q

How reactive are Halogens (Group 7)?

A

Very reactive - only 1 outer electron

96
Q

What is the most reactive element in Group 7?

A

Iodine

97
Q

What are Noble Gases?

A

Chemical elements which are not at all reactive - they have a full outer shell of electrons.

98
Q

How reactive are Noble Gases?

A

They have a full outer shell - do not need to react to form ions

99
Q

What is the name of Group 0 on the periodic table?

A

Noble Gases

100
Q

What is the charge of Alkali Metals?

A

+1

101
Q

What is the name of group 1 elements?

A

Alkali Metals

102
Q

How reactive are Alkali Metals?

A

Very reactive - only 1 electron in the outer shell

103
Q

What is the trend of reactivity of Alkali Metals?

A

Every electron going down group 1 has only 1 electron in its outer shell

104
Q

Give 2 properties of transition metals:

A

Any 2 from:
Lustrous (shiny), malleable, high melting/boiling point, good heat conductors, mostly non-magnetic, coloured compounds, hard and strong, ductile, high density, high conductors of electricity, very unreactive

105
Q

How reactive are transition metals?

A

Very unreactive

106
Q

What are the properties of ionic compounds?

A
  1. Form crystals
  2. Hard and brittle
  3. High melting and boiling points
  4. Conduct electricity when molten or in solution
  5. Good insulators - solid at room temperature
  6. Often soluble in water
  7. Strong ionic bonds
107
Q

What are polymers also known as?

A

Macromolecules

108
Q

What is a polymer?

A

A large molecule made up of many repeating small units

109
Q

What type of bonding is in a polymer?

A

Covalent bonding

110
Q

What are the properties of polymers?

A

Strong and do not melt

111
Q

What are polymers used for?

A

Shopping bags, manufacturing

112
Q

What is graphite?

A

A giant covalent structure

113
Q

What is graphene?

A

One layer of graphite

114
Q

What are the properties of graphite?

A

Strong, high melting/boiling points (covalent bonds), atoms arranged in hexagon layers which can slide over each other (soft surface), bonded to 3 carbon atoms - can conduct electricity

115
Q

What are the properties of graphene?

A

High melting/boiling points - covalent bonds, can conduct electricity (unbonded electron), strong, inexpensive, lightweight, used in solar cells/batteries

116
Q

Why do metals conduct electricity?

A

They contain delocalised electrons

117
Q

What are allotropes?

A

Different structural forms of the same element in the same physical state

118
Q

What is required for a substance to conduct electricity?

A

They must have some delocalised electrons

119
Q

What are the properties of metals?

A

All atoms are same size and shape, layers slide easily - more malleable

120
Q

What are the properties of alloys?

A

Atoms are different sizes - harder for the layers to slide (less malleable/stronger)

121
Q

What are the properties of diamond?

A

Strong, high melting/boiling points (giant covalent structure), bonded to 4 carbon atoms so can’t conduct electricity

122
Q

When are giant lattice structures formed?

A

When a huge number of non-metal atoms are held together by strong covalent bonds

123
Q

What are the properties of giant lattice structures?

A

Very high melting/boiling point, do not conduct electricity (except graphite), very strong

124
Q

What are the properties of small molecules/simple molecular substances?

A

Do not conduct electricity

125
Q

Why do simple molecular substances have a low melting/boiling point?

A

Weak intermolecular forces

126
Q

What are simple molecular substances?

A

Small molecules in which the atoms in the molecules are joined by strong covalent bonds but between the molecules are weak intermolecular forces

GCSE Revision Flashcards (21 decks)

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