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LQB180 > Atoms and elements > Flashcards

Atoms and elements Flashcards

1
Q

The area within an atom is mostly filled by ____ ____

A

Empty space

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2
Q

Where are the protons and neutrons located in an atom?

A

In the nucleus

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3
Q

How much of the mass of an atom is contained in its nucleus?

A

99%

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4
Q

The nucleus contains ____% of the mass of the atom

A

99%

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5
Q

Electrons ____ around the nucleus

A

Orbit

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6
Q

What charge is carried by protons?

A

Positive charge

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7
Q

What charge is carried by electrons?

A

Negative charge

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8
Q

What charge is carried by neutrons?

A

Neutrons are neutral

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9
Q

Overall, atoms are ____ charged

A

Neutrally

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10
Q

Why is an atom (generically) neutrally charged?

A

The number of protons is equal to the number of electrons

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11
Q

What is the name of a charged atom?

A

An ion

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12
Q

What is an ion?

A

A charged atom

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13
Q

What is the atomic cloud?

A

The space occupied by electrons around the nucleus of an atom

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14
Q

What are subatomic particles?

A

Particles smaller than an atom - protons, neutrons, and electrons

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15
Q

One electron carries what charge?

A

1-

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16
Q

One proton carries what charge?

A

1+

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17
Q

One neutron carries what charge?

A

0

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18
Q

What is the mass of one proton?

A

1.007

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19
Q

What is the mass of one neutron?

A

1.008

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20
Q

What is the mass of one electron?

A

0.00055 (considered to be negligible)

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21
Q

What makes atoms different from each other?

A

Their atomic mass and their atomic number

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22
Q

What is the atomic mass of an atom?

A

The sum of all p⁺ and n⁰ in the nucleus

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23
Q

What is given by the sum of all p⁺ and n⁰ in the nucleus of an atom?

A

The atomic mass

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24
Q

What is the atomic number of an atom?

A

The number of all p⁺ in the nucleus

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25
Q

What is given by the number of all p⁺ in the nucleus of an atom?

A

The atomic number

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26
Q

What is the atomic mass of carbon?

A

6p⁺ : 6n⁰ : 6e⁻ = 12

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27
Q

What is the atomic number of carbon?

A

6

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28
Q

What is amu?

A

Atomic mass units; the mass of a proton

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29
Q

What is the meaning of Da in biochemistry?

A

Daltons, the mass of a proton

Da (used in biochemistry) = amu (used in chemistry

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30
Q

What is the definition of a Dalton?

A

1/12th of a carbon atom

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31
Q

The more p⁺ or n⁰ you have, the larger the ____ will be

A

Mass

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32
Q

1 amu = 1 Da = 1 ____

A

g/mol

1 amu = 1 Da = 1 g/mol

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33
Q

What is an isotope?

A

An atom with the same number of protons but different number of neutrons

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34
Q

How many protons and neutrons in carbon-12?

A

Carbon-12 has 6p⁺ and 6n⁰

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35
Q

How many protons and neutrons in carbon-13?

A

Carbon-13 has 6p⁺ and 7n⁰

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36
Q

How many protons and neutrons in carbon-14?

A

Carbon-14 has 6p⁺ and 8n⁰

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37
Q

What is the atomic mass of carbon-13?

A

13 Da

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38
Q

What is the atomic mass of carbon-14?

A

14 Da

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39
Q

Which is more stable, carbon-12 or carbon-14?

A

Carbon-12 is more stable than carbon-14

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40
Q

Which is more stable, carbon-13 or carbon-14?

A

Carbon-13 is more stable than carbon-14

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41
Q

What is an important property of carbon-14?

A

Carbon-14 is radioactive

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42
Q

Is carbon-13 stable?

A

Yes, carbon-13 is stable (it accounts for 1.11% of carbon found on earth)

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43
Q

Most elements found on earth are a mixture of ____

A

Isotopes

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44
Q

If chlorine found on earth is 75.77% chlorine-35 and 24.23% chlorine-37, how do we calculate the true atomic weight of chlorine?

A

By multiplying the atomic mass of each isotope by their percentage of occurrence before adding them together and finding the average by dividing by 2.

[(35 x 0.7577) + (37 x 0.2423)] / 2 = 35.5 Da

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45
Q

The number after the dash in the name of an isotope (e.g. the ‘14’ in carbon-14) gives what information?

A

The atomic mass of that isotope

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46
Q

The higher the atomic number, the more ____ could potentially exist

A

Isotopes

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47
Q

Elements further down the periodic table, i.e. those with higher atomic numbers, are more likely to have a greater number of different ____

A

Isotopes

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48
Q

What is emitted by unstable isotopes?

A

Radiation

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49
Q

Name one use of unstable isotopes

A

Diagnostic imaging (CT-scan)

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50
Q

As the number of protons rises, there are increasingly more ____ than protons

A

Neutrons

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51
Q

Every element has a different number of ____

A

Protons

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52
Q

The atomic number tells you how many ____ the atom has

A

Protons

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53
Q

How many protons does oxygen have?

A

Oxygen has the atomic number 8, therefore it has 8 protons

54
Q

How many protons does carbon have?

A

Carbon has the atomic number 6, therefore it has 6 protons

55
Q

How many protons does sodium have?

A

Sodium has the atomic number 11, therefore it has 11 protons

56
Q

What is the difference beween an atom and an element?

A

An atom is a singular entity, whereas an element is comprised of multiple atoms of one type

57
Q

How is molecular mass calculated?

A

By adding the atomic mass of each atom in the molecule

58
Q

What is the molecular mass of water? Describe how it’s calculated.

A

H₂O contains 2 hydrogen and 1 oxygen atoms.

The atomic mass of hydrogen = 1. The atomic mass of oxygen = 16.

Molecular mass = (2x1) + (1x16) = 18 Da

59
Q

What is Avogadro’s constant (the number)?

A

6.022x10²³, the number of atoms in one mole of that substance

60
Q

What is 6.022x10²³ ?

A

Avogadro’s constant, the number of atoms in one mole of that substance

61
Q

How many atoms in one mole of a substance?

A

6.022x10²³

62
Q

12 eggs in a dozen = ____ atoms in a mole

A

6.022x10²³

63
Q

The molar mass of carbon is 12.01. This means that in one mole of carbon there are ____ grams of carbon

A

12.01

64
Q

The molar mass of water is 18. This means that in one mole of water there are ____ grams of water.

A

18

65
Q

If the molar mass of water is 18 Da, how many molecules of water are in 1mL?

A

6.022x10²³ x 1/18 = 3.3x10²² molecules of water in one mL

66
Q

If there are 3.3x10²² molecules of water in 1mL, how many moles of water is in that 1mL?

A

3.3x10²² / 6.022x10²³ = 0.055 moles

67
Q

What is the name of the discrete energy levels at which electrons exist?

A

Quanta

68
Q

What is required for electrons to populate higher quantised states?

A

Higher energy

69
Q

Electrons require higher energy to exist in higher ____ states

A

Quantised

70
Q

The ____ atomic model shows the simplified arrangement of electrons in rings around the nucleus

A

Bohr

71
Q

The further out from the nucleus an electron is, the more ____ is required

A

Energy

72
Q

Electrons reside in ____

A

Shells

73
Q

What is the name of the outermost electron shell?

A

Valence shell

74
Q

What is the name of the outermost electrons?

A

Valence electrons

75
Q

The most important subatomic particles in chemistry are the ____ ____

A

Valence electrons

76
Q

Ions are formed by the gain and loss of ____

A

Electrons

77
Q

The gain and loss of electrons forms what?

A

Ions

78
Q

What is the net charge when an electron is lost?

A

Net +ve charge

79
Q

What is the net charge when an electron is gained?

A

Net -ve charge

80
Q

Where do electron gains or losses occur?

A

Within the valence shell

81
Q

Which electrons are involved in ion formation?

A

Valence electrons

82
Q

What are cations?

A

Ions with a net +ve charge; more protons than electrons

83
Q

What type of ion has more protons than electrons?

A

Cation

84
Q

What type of ion has a net +ve charge?

A

Cation

85
Q

What are anions?

A

Ions with a net -ve charge; more electrons than protons

86
Q

What type of ion has more electrons than protons?

A

Anion

87
Q

What type of ion has a net -ve charge?

A

Anion

88
Q

Quantised states are ____ within atoms

A

Shells

89
Q

Electron shells contain electron ____

A

Orbitals

90
Q

What defines electron filling and configuration?

A

Electron orbitals

91
Q

Every electron shell is made up of one or more ____

A

Orbitals

92
Q

The number of ____ increases with the number of electron shells

A

Orbitals

93
Q

Do orbitals increase in odd or even values?

A

Odd.

s has 1, p has 3, d has 5, f has 7, etc.

94
Q

What orbitals are in electron shell 1?

A

S

95
Q

What orbitals are in electron shell 2?

A

An s orbital and a p orbital

96
Q

What orbitals are in electron shell 3?

A

An s orbital, a p orbital, and a d orbital

97
Q

How many orientations does a p orbital have?

A

Three

98
Q

How many orientations does a d orbital have?

A

Five

99
Q

Which has higher energy, s or p orbitals?

A

p orbitals

100
Q

How many electrons can any orbital orientation hold?

A

A maximum of 2

101
Q

How many electrons can an s orbital hold?

A

2 electrons, because s orbitals have one orientation

102
Q

How many electrons can a p orbital hold?

A

6 electrons, because p orbitals have 3 orientations

103
Q

How many electrons can a d orbital hold?

A

10 electrons, because d orbitals have 5 orientations

104
Q

What is the filling of orbitals based on?

A

Energy levels

105
Q

What does orbital filling determine?

A

Electron configuration

106
Q

What is determined by orbital filling and so electron configuration?

A

Atom reactivity

107
Q

What determines atom reactivity?

A

Orbital filling which determines electron configuration

108
Q

The rows of the periodic table are called ____

A

Periods

109
Q

The columns of the periodic table are called ____

A

Groups

110
Q

What increases from left to right across the periodic table?

A

Atomic number and atomic weight

111
Q

What increases from top to bottom across the periodic table?

A

Atomic number and atomic weight

112
Q

The periodic table is grouped in blocks by ____

A

Orbitals

113
Q

The periods (rows) of the periodic table show what?

A

Which electron shell is filling

114
Q

Electron configuration gave chemists the rationale for what?

A

How compounds and molecules form

115
Q

The group (column) an element belongs to in the periodic table tells us what?

A

How many valence electrons are in the outer shell of that element

116
Q

Carbon is in group 4 in the periodic table. How many valence electrons does carbon have?

A

4

117
Q

Oxygen is in group 6 in the periodic table. How many valence electrons does oxygen have?

A

6

118
Q

Electrons are given/taken to obtain stable configuration - what does this mean?

A

Stable configuration, an electron valency of 8 (full outer shell)

119
Q

Chlorine is in group 7 of the periodic table. How many valence electrons does chlorine have?

A

7

120
Q

The elements in the 8th group of the periodic table have full valency. What does this mean for the properties of these elements?

A

The elements in the 8th group of the periodic table are very stable and not very reactive

121
Q

What is the name given to the 8th group of elements on the periodic table?

A

Noble gases

122
Q

What is electronegativity?

A

An atom’s attraction for other electrons (to make a chemical bond)

123
Q

Do atoms with higher values of electronegativity generally lose, share, or gain electrons?

A

Gain

124
Q

Do atoms with low values of electronegativity generally lose, share, or gain electrons?

A

Lose

125
Q

Do atoms with middle values of electronegativity generally lose, share, or gain electrons?

A

Share

126
Q

Essentially, an atom’s electronegativity is its desire to become what?

A

A noble gas

127
Q

Elements in groups 1, 2, and 3 tend to become ____ (ion type)

A

Cations

128
Q

Elements in groups 5, 6, and 7 tend to become ____ (ion type)

A

Anions

129
Q

Elements in groups 1, 2, and 3 tend to become cations by ____ their electrons

A

Losing

130
Q

Elements in groups 5, 6, and 7 tend to become anions by ____ their electrons

A

Gaining

131
Q

When Na bonds with Cl₂, which element loses electrons?

A

Na is in group 1 of the periodic table - Na loses one electron, becomes a cation

132
Q

When Na bonds with Cl₂, which element gains electrons?

A

Cl is in group 7 of the periodic table - Cl gains one electron, becomes an anion

LQB180 (3 decks)

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