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Chemistry (Tara) > Atomic theory 1 > Flashcards

Atomic theory 1 Flashcards

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1
Q

Define Element

A

A substance that cannot be broken down into simpler substances by chemical means.

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2
Q

How are elements arranged horizontally?

A

In periods

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3
Q

How are elements arranged vertically?

A

In groups

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4
Q

What does the number of electrons in the outer shell give rise to and what does it mean?

A

Valency - which means the number of chemical bonds an element can make.

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5
Q

What is the name of group 1

A

Alkali metals (1 electron in outer shell, valency =1)

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6
Q

What is the name of group 2

A

Alkaline earth metals (2 electrons in outer shell, valency = 2)

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7
Q

What is the name of group 7

A

Halogens( 7 electrons in outer shell, valency = 1)

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8
Q

What is the name of group 0?

A

Noble gases ( 8 electrons in outer shell, valency = 0\0

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9
Q

Protons

A

Positively charged

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10
Q

Neutrons

A

Neutral

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11
Q

Electrons

A

Negatively charged

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12
Q

Where are protons and neutrons found?

A

In the nucleus of the atom

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13
Q

Where are electrons in orbitals (sub-levels) found?

A

Around the nucleus

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14
Q

Do ions have a charge?

A

Yes

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15
Q

Do atoms and molecules have a charge?

A

No they are neutral

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16
Q

Are the words atoms and ions interchangeable?

A

No as atoms and ions are completely different

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17
Q

What is the whole number above the symbol for the element called?

A

The atomic number (Z)

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18
Q

What is the decimal number below each element called?

A

The relative atomic mass number (Ar)

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19
Q

What does the atomic number tell us?

A

The number of protons an atom of the element will have.

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20
Q

What does the relative atomic mass give?

A

An average mass of all known isotopes of that element.

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21
Q

Define metal

A

Any element that loses electrons to form a positive ion (cation).

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22
Q

Define atomic number

A

The number of protons present in the nucleus of an atom.

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23
Q

Define mass number

A

The mass number is the number of protons plus neutrons in the nucleus of an atom.

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24
Q

Define isotopes

A

Isotopes are atoms of the same element that have the same atomic number but different mass numbers due to the different numbers of neutrons present in the nucleus.

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25
Q

Define relative atomic mass number

A

The average mass of an atom of an element compared to 1/12 the mass of the carbon - 12 isotope, taking relative abundances of the naturally occurring isotopes into account.

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26
Q

What is valency linked to?

A

‘Octet rule’

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27
Q

Valency of group 1

A

1

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28
Q

Valency of group 2

A

2

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29
Q

Valency of group 3

A

3

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30
Q

Valency of group 4

A

4

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31
Q

Valency of group 5

A

3

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32
Q

Valency of group 6

A

2

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33
Q

Valency of group 7

A

1

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34
Q

Valency of group 8

A

0

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35
Q

Alkali metals

A
  • Extremely reactive
  • Soft metals
  • Low densities
  • Shiny when freshly cut but tarnish rapidly due to reaction with air
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36
Q

Alkali metal + oxygen gas –>

A

Metal oxide

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37
Q

Alkali metal + water –>

A

Metal hydroxide + hydrogen gas

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38
Q

Alkaline earth metals

A
  • Very reactive but less reactive than the alkali metals

- Magnesium reacts slowly with water

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39
Q

Halogens

A
  • Very reactive non-metals

- Low melting and boiling points

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40
Q

Noble gases 3

A
  • Gaseous at r.t
  • B.P increases down group
  • Least reactive of all elements (as have 8 electrons in outer shell - except He which has 2 electrons in its only shell)
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41
Q

What can particles be?

A

Atoms, molecules or ions.

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42
Q

Where is the mass of an atom concentrated?

A

In a small central nucleus consisting of protons and neutrons.

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43
Q

What is around the nucleus?

A

Electrons

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44
Q

Why can the mass of an electron often be ignored?

A

As its so small

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45
Q

In an atom what does the number of electrons always equal to?

A

The number of protons in the nucleus

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46
Q

What does the total negative charge equal?

A

The total positive charge

47
Q

Atoms are

A

Neutral

48
Q

On going from left to right across the periodic table the elements get ….

A

Less metallic in nature and more gaseous

49
Q

What are H2,N2,O2,F2 & C2 at r.t?

A

Gaseous % diatomic

50
Q

Can H2,N2,O2,F2 & C2 be found on their own in nature?

A

No

51
Q

What is the only metal that is liquid at r.t?

A

Hg

52
Q

What is Br2 (non-metal) at r.t?

A

Liquid, exists diatomically

53
Q

What is I2 (non-metal) at r.t?

A

Solid, exists diatomically

54
Q

What are C, Si, P & S (non-metals) at r.t?

A

Solids, exist mono-atomically

55
Q

What are all noble gases as r.t?

A

Gaseous

56
Q

How do noble gases exist?

A

Mono-atomically

57
Q

How many isotopes does carbon have?

A

3

58
Q

How many isotopes does hydrogen have?

A

3

59
Q

Why is the relative atomic mass number rarely a whole number?

A

As it is the average of all known isotopes of an element.

60
Q

Define relative molecular mass number (Ar)

A

The average mass of a molecule of a compound compared to 1/12 the mass of the carbon - 12 isotope, taking relative abundances of the naturally occurring isotopes into account.

61
Q

How do you get the Mr?

A

By adding together the relative atomic masses present in a molecule

62
Q

What do atoms do to form ions?

A

They gain or lose electrons

63
Q

What happens if an atom loses an electron?

A

A positive ion will be formed

64
Q

What happens if an atom gains an electron?

A

A negative ion will be formed

65
Q

What is another name for positive ions?

A

Cations

66
Q

What is another name for negative ions?

A

Anions

67
Q

Do metal atoms tend to gain or lose electrons?

A

Lose electrons (to form cations)

68
Q

Do non-metal atoms tend to gain or lose electrons?

A

Gain electrons (to form anions)

69
Q

Naturally occurring chlorine consists of 75.5% of (35)Cl and 24.5% of (37) Cl. Calculate the relative atomic mass (Ar) of chlorine. (L.C)

A
  • 75.5 x 35 = 2642.5
  • 24.5 x 37 = 906.5
    100 atoms = 3549
    1 atom = 35.49 (Ar)
70
Q

*Metal + oxygen =

A

Metal oxide

71
Q

*(usually metals from group 1 or 2)Metal + water =

A

Metal hydroxide + hydrogen gas

72
Q

A dipositive ion, M2+, has 25 electrons and 32 neutrons. What is (i) the atomic number, (ii) the mass number, of M (L.C)

A

i) 27

ii) 59

73
Q

What are isotopes? (L.C)

A

Atoms with the same atomic number (Z) but different mass numbers (A)

74
Q

How many (i) electrons, (ii) neutrons, has the aluminium ion Al3+ (L.C)

A

i) 10

ii) 14

75
Q

Explain why relative atomic masses are rarely whole numbers. (L.C)

A

As it is the average of mass numbers of the isotopes of an element

76
Q

Define (i) mass number, (ii) relative atomic mass (L.C)

A

(i) number of nucleons (protons and neutrons) in the atoms of an isotope
(ii) Average mass of atoms of element relative to 1/12 of mass of carbon-12 atom

77
Q

A sample of the element gallium is composed of 60.1% gallium-69 and 39.9% gallium-71. Calculate the relative atomic mass of gallium from this information. (L.C)

A

69 x 60.1 = 4146.9
71 x 39.9 = 2832.9
100 atoms = 6979.8
Ar = 69.798 (69.8)

78
Q

Define relative atomic mass (L.C)

A

Average mass of atoms of element relative to 1/12 mass of carbon-12 atom

79
Q

Define relative atomic mass (L.C)

A

Average mass of atoms of element relative to 1/12 mass of carbon-12 atom

80
Q

Define (a) atomic number, (b) relative atomic mass (L.C)

A

a) Number of protons in the nucleus of an atom of the element
b) Average mass of atoms of element relative to 1/12 mass of carbon-12 atom

81
Q

What are isotopes? (L.C)

A

Atoms with the same atomic number (Z) but different mass numbers (A)

82
Q

What are isotopes? (L.C)

A

Atoms with the same atomic number (Z) but different mass numbers (A)

83
Q

What is the principle of the mass spectrometer? (L.C)

A

Positive ions separated based on relative mass when moving in a magnetic field

84
Q

Calculate, to two decimal places, the relative atomic mass of a sample of neon shown by mass spectrometer to be composed of 90.5% of neon-20 and 9.5% of neon-22. (L.C)

A

90.5 x 20 = 1810
9.5 x 22 = 209
100 atoms = 2019
Ar = 20.19

85
Q

What are isotopes? (L.C)

A

Atoms with the same atomic number (Z) but different mass numbers (A)

86
Q

Define relative atomic mass, Ar (L.C)

A

Average mass of atoms of element relative to 1/12 mass of carbon-12 atom

87
Q

What is the principle on which the mass spectrometer is based?

A

Positive ions separated based on relative mass(es) when moving in a magnetic field

88
Q

Calculate the relative atomic mass of a sample of lithium, given that a mass spectrometer shows it consists of 7.4% (6)Li and 92.6% (7)Li (L.C)

A

7.4 x 6 + 92.6 x 7 = 692.6
100 atoms = 692.6
1 atom = 6.926

89
Q

Is Na+ an atom, molecule, simple ion or a complex ion?

A

Simple ion

90
Q

Is K an atom, molecule, simple ion or a complex ion?

A

Atom

91
Q

Is SO2+ an atom, molecule, simple ion or a complex ion?

A

Complex ion

92
Q

Is I2 an atom, molecule, simple ion or a complex ion?

A

Molecule

93
Q

Is F- an atom, molecule, simple ion or a complex ion?

A

Simple ion

94
Q

Is Fe an atom, molecule, simple ion or a complex ion?

A

Atom

95
Q

Is KMn04 an atom, molecule, simple ion or a complex ion?

A

Molecule

96
Q

Is 02- an atom, molecule, simple ion or a complex ion?

A

Complex ion

97
Q

What is the atomic number of sulfur?

A

16

98
Q

What is the atomic number of calcium?

A

20

99
Q

What is the atomic number of iron?

A

26

100
Q

What is the atomic number of bromine?

A

35

101
Q

What is the relative atomic mass number of sulfur?

A

32

102
Q

What is the relative atomic mass number of calcium?

A

40

103
Q

What is the relative atomic mass number of iron?

A

56

104
Q

What is the relative atomic mass number of iodine?

A

154

105
Q

How many (i) protons, (ii) neutrons and (iii) electrons in (35) Cl?

A

(i) 17p
(ii) 18n
(iii) 18e

106
Q

Identify the element that has 60.4% of atoms with a mass of 69 and a remainder with a mass of 71.

A

Gallium

107
Q

What is the relative atomic mass of magnesium which normally consists of 78.6% magnesium-24, 10.1% magnesium-25 and 11.3% magnesium-26?

A

24.31 (check this)

108
Q

Identify an element that is a non-metal and is liquid at room temperature.

A

Br

109
Q

Identify an element that is a divalent metal.

A

Anyone from group 2 (Be, Mg, Ca…)

110
Q

Identify an element that exists in both diatomic and triatomic states.

A

Oxygen

111
Q

Identify an element that has an atomic number of 26

A

Fe

112
Q
  • Florine and chlorine
A

Halogens

yellow-green gases

113
Q

Bromine

A

Halogen

a red liquid

114
Q

Iodine

A

Halogen

a dark solid at room temperature

Chemistry (Tara) (50 decks)

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