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Science Semester Two > Chemistry > Flashcards

Chemistry Flashcards

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1
Q

What is a proton?

A

Sub-atomic particle with a positive charge

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2
Q

What is a neutron?

A

Sub-atomic particle with a neutral charge

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3
Q

what is an electron?

A

Sub-atomic particle with a negative charge

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4
Q

What is the core of the atom?

A

the nucleus

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5
Q

what is in the nucleus?

A

protons and neutrons

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6
Q

What is the charge of atoms?

A

Neutral, equal protons and electrons

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7
Q

Where are protons found?

A

In the nucleus

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8
Q

Where are neutrons found?

A

nucleus

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9
Q

Where are electrons found?

A

Electron shell

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10
Q

If the atom was the MCG, what would the nucleus be the size of?

A

A marble

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11
Q

What are elements?

A

Pure substances made up of only one type of atom

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12
Q

How many elements have been found to date?

A

118

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13
Q

What determines the element?

A

Number of protons

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14
Q

What does each successive element differ by?

A

One proton

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15
Q

What is the atomic number?

A

Amount of protons

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16
Q

What letter represents the atomic number?

A

Z

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17
Q

What is the mass number?

A

The number of protons and neutrons

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18
Q

What letter represents the mass number?

A

A

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19
Q

What experiment proves that there is a nucleus?

A

Rutherfold’s Gold Experiment

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20
Q

What happened in Rutherford’s Gold Experiment?

A

Alpha particles were fired at gold. Some bounced back, showing that there was a small, dense centre.

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21
Q

What are isotopes?

A

Atoms with the same number of protons but different number of neutrons

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22
Q

What is the relative atomic mass?

A

Weighted average of the isotopic masses based on prevalence in the environment

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23
Q

How are isotopes written/identified?

A

Name of element with mass number (e.g. lithium-3)

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24
Q

What are shells?

A

Different energy levels where electrons are grouped

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25
Q

How many electrons can each shell hold?

A

2, 8, 18, 32, etc

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26
Q

What is the electron shell configuration?

A

Ordered list of the number of electrons in each shell

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27
Q

What do electrons in the same shell have?

A

The same energy

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28
Q

Which electrons have a greater attraction to the nucleus?

A

The ones closer to it

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29
Q

What happens the further away electrons become?

A

Requires less energy to be removed

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30
Q

What are valence electrons?

A

Electrons in the outermost shell

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31
Q

What electrons are used in chemical reactions?

A

Valence electrons

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32
Q

What are elements listed in order of?

A

Increasing atomic number

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33
Q

What are vertical columns called?

A

Groups

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34
Q

What do elements in the same group have in common?

A

Same number of valence electrons. Similar chemical properties

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35
Q

How does the group number signify the number of valence electrons?

A

Group 1-2: group = valence electrons number
Group 13-18: group - 10 = valence electron number

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36
Q

What are the horizontal rows called?

A

Periods

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37
Q

What does the period number relate to?

A

Number of shells filled by electrons

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38
Q

Which element is the exception to group and period rule?

A

Helium

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39
Q

What group is the noble gases?

A

Group 18

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40
Q

What are the traits of noble gases?

A

Full outer shell, unreactive (doesn’t combine with other atoms), stable electron configuration, stable

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41
Q

What is metallic bonding between?

A

Metals

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42
Q

Why do chemical reactions occur?

A

Because atoms change electrons to have a full outer shell

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43
Q

What is ionic bonding between?

A

Non metals and metals

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44
Q

What is covalent bonding between?

A

Non-metals

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45
Q

What are ions?

A

Atoms or groups of atoms that have become charged through loss or gain of electrons

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46
Q

What are cations?

A

Positively charged ions

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47
Q

What are anions?

A

Negatively charged ions

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48
Q

What do metals tend to become in ions?

A

Lose electrons, form cations

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49
Q

What do non-metals tend to become in ions?

A

Gain electrons, become anions

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50
Q

How are non-metals written?

A

Ending with an ‘ide’

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51
Q

What do transition metals form?

A

Cations

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52
Q

What is used to indicate charge for transition metals?

A

Roman numerals e.g. Lead(II)

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53
Q

What is the ion symbol for copper (I)?

A

Cu+

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54
Q

What is the ion symbol for lead (II)?

A

Pb2+

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55
Q

What is the ion symbol for iron (III)?

A

Fe3+

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56
Q

What is the ion symbol for nickel (II)?

A

Ni2+

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57
Q

What is the ion symbol for copper (II)?

A

Cu2+

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58
Q

What is the ion symbol for iron (II)?

A

Fe2+

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59
Q

What is the ion symbol for gold (III)?

A

Au3+

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60
Q

What is the ion symbol for zinc?

A

Zn2+ (no roman numerals)

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61
Q

What is the ion symbol for silver?

A

Ag+ (no roman numerals)

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62
Q

What is a polyatomic ion?

A

Ions composed of more than one atom

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63
Q

What is the ionic symbol for hydroxide?

A

OH-

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64
Q

What is the ionic symbol for carbonate?

A

CO3 2-

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65
Q

What is the ionic symbol for hydrogen carbonate?

A

HCO3 -

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66
Q

What is the ionic symbol for lithium?

A

Li+

67
Q

What is the ionic symbol for sodium?

A

Na+

68
Q

What is the ionic symbol for potassium?

A

K+

69
Q

What is the ionic symbol for magnesium?

A

Mg2+

70
Q

What is the ionic symbol for calcium?

A

Ca2+

71
Q

What is the ionic symbol for aluminium?

A

Al3+

72
Q

What is the ionic symbol for nitrogen/nitride?

A

N3-

73
Q

What is the ionic symbol for phosphorus/phosphide?

A

P3-

74
Q

What is the ionic symbol for oxygen/oxide?

A

O2-

75
Q

What is the ionic symbol for sulfur/sulfide?

A

S2-

76
Q

What is the ionic symbol for fluorine/fluoride?

A

F-

77
Q

What is the ionic symbol for chlorine/chloride?

A

Cl-

78
Q

What is the ionic symbol for bromine/bromide?

A

Br-

79
Q

What is ionic bonding?

A

Result of electrons being transferred from a metal to a non-metal

80
Q

What is the result of a strong electrostatic charge between cations and anions?

A

Ionic bonding

81
Q

What are ionic compounds?

A

Rigid solids composed of regular, repeating 3-dimensional arrangement of alternating positive and negative ions (ionic lattice)

82
Q

Where is the superscript for ionic compounds?

A

Lower corner, with the number of each that is needed to balance out. Use brackets to be even

83
Q

What is the compound name for iodine?

A

Iodide

84
Q

What is the compound name for hydrogen?

A

Hydride

85
Q

What is the compound name for sulfur and oxygen?

A

Sulfate

86
Q

What is the compound name for carbon and oxygen?

A

Carbonate

87
Q

What is the compound name for nitrogen and oxygen?

A

Nitrate

88
Q

What is the compound name for chlorine and oxygen?

A

Chlorate

89
Q

What do ionic compounds form?

A

Crystals

90
Q

How do ions arrange themselves?

A

In the most stable configuration. Oppositely charged ions are as close together as possible, while ions of hte same charge are as far apart as possible

91
Q

What does the shape of the crystal and strength of ionic bonding depend on?

A

Size and charge of ions

92
Q

What are the properties of ionic compounds?

A

Brittle
Crystalline solids
Electrically conductive as a solid but can conduct electricity when molten or in an aqueous solution
Hard
High melting points
High boiling points

93
Q

Why do ionic compounds have high melting and boiling points?

A

Large amounts of energy are required to break the strong electrostatic attractions between ions

94
Q

What does a substance need in order to be able to conduct electricity?

A

Free-moving, charged particles

95
Q

What happens when ionic compounds become molten or aqueous?

A

The positive and negative ions are free to conduct electricity

96
Q

Why can ionic compounds not conduct electricity when they are solid?

A

The ions are fixed in their place in the lattice, so are not free moving

97
Q

Why are ionic compounds not easily scratched?

A

A strong force is needed to disrupt the strong electrostatic forces

98
Q

Why are ionic compounds brittle?

A

When sufficient force is applied to distort the lattice, ions of like charges become adjacent and repel each other

99
Q

What are the characteristics of metals?

A

Dense
Malleable/ductile
Good conductor of heat
Shiny (lustruous)
Heats quickly
Hard

100
Q

How does metallic bonding occur?

A

Metals lost valence electrons to form cations. The cations are repelling each other so form a 3D lattice, as this allows them to be as far away from each other as possible. The valence electrons are then attracted to these ions, so form a sea of delocalised electrons.

101
Q

How do metals stay together?

A

Electrostatic attraction exists between the cations and the sea of delocalised electrons, keeping them together

102
Q

Why are metals good electrical conductors?

A

The delocalised electrons are free moving and charged, so can carry a current. The electrons move to a positive electrode because they are attracted

103
Q

Why are metals good heat conductors?

A

The heat causes vibrtions and the electrons are free-moving and able to move through the lattice transferring heat (b/c not fixed). The lattice is close toghether which allows for effective heat transfer

104
Q

Why do metals have high melting and boiling points?

A

Lots of energy is required to break the strong bonds between them.

105
Q

Why are metals malleable and ductile?

A

When a force is applied, the layers of cations move past each other. Electrons are free to move with the cations easily. This means the electrostatic attraction bond is still strong. Electrons act like lubricating glue

106
Q

Why do metals have high density?

A

Cations are packed together closely

107
Q

Why are metals lustrous?

A

Electrons reflect light

108
Q

Why are metals hard?

A

Very strong metallic bonds hold it together

109
Q

What are some signs of a chemical change?

A

New substance, colour change, gas, smell, precipitate, heat

110
Q

What are the state symbols?

A

State symbols show the physical state of the substance in a chemical reaction.
solid (s), liquid (l), gas (g), or dissolved in water (aq)

111
Q

Describe the structure of a metal?

A

Metallic lattice: Regular, repeating, 3-dimensional arrangement metal cations surrounded by a sea of electrons

112
Q

What happens at the join between two metal crystals?

A

Rows of cations do not necessarily align, so there’s a gap between crystals.

113
Q

What does the gap between crystals lead to?

A

This point reduces the ease with which a metal will bend and introduces a point of weakness

114
Q

What is annealing?

A

When metals are heated until they are red hot and then cooled slowly

115
Q

What is the effect of annealing?

A

Larger metal crystals are formed with less gaps between crystals, so the metal produced will be softer and more ductile

116
Q

What is quenching?

A

When metals are heated until they are red hot and forced to cool quickly in cold water

117
Q

What is the effect of quenching?

A

Smaller crystals are formed with more gaps, making the metal harder and more brittle

118
Q

What is tempering metals?

A

When quenched metals (heated until red hot and then cooled with ice water) are warmed again to a lower temperature and then allowed to cool slowly

119
Q

What is the effect of tempering metals?

A

Reduces the brittleness of the metal while retaining the hardness. Mix between malleable and hard

120
Q

What heat modification would you use for horseshoes?

A

Quenched: hard as possible to avoid flattening. Doesn’t need to resist bending and twisting, so brittleness is not an issue

121
Q

What heat modification is used for swords/axes/lathes/chisels/rock drills?

A

Tempered: need to be hard, but not too brittle to prevent snapping.

122
Q

Which metal is the exception for a high melting point?

A

Mercury, which is liquid at room temperature

123
Q

Which metals are magnetic?

A

Cobalt, iron, nickel

124
Q

Which metals are soft?

A

Lithium, sodium, gold

125
Q

With the same degree of heat modification, will all metal samples have the same hardness and malleability?

A

No because different starting points

126
Q

What is a solution?

A

A substance dissolved in a solvent

127
Q

What is a solute?

A

Substance dissolved into a solvent. May be a solid/liquid/gas

128
Q

What state is the solvent nearly always in?

A

Liquid

129
Q

What do many ionic compounds dissolve in?

A

Water

130
Q

What is a solution called when water is the solvent?

A

Aqueous

131
Q

What is a native metal?

A

A metal that is in its pure form, without reacting with any other metals (stable)

132
Q

What is reactivity?

A

How vigorously an element combines with other elements
A measure of how easily a metal loses electrons to form positive ions

133
Q

What is the order of the metal reactivity scale?

A

K: potassium
Na: sodium
Ca: calcium
Li: lithium
Mg: magnesium
Al: aluminium
Zn: zinc
Fe: iron
Sn: Tin
Cu: copper
Ag: silver

134
Q

What happens in a displacement reaction?

A

A piece of solid metal is placed in a solution containing a dissolved ionic compound. If the solid metal is more reactive than the metal in the solution, the metals will swap places

135
Q

What will happen when a more reactive metal is already in the solution?

A

No displacement reaction will occur

136
Q

How to spot a displacement reaction?

A

The metals will swap

137
Q

What are some native metals?

A

Gold, silver, platinum

138
Q

Why do native metals remain unreactive?

A

They are unreactive, so have not reacted with other elements

139
Q

What are minerals?

A

What is formed when reactive metals are combined with other elements

140
Q

What are ores?

A

Minerals when they are mined

141
Q

What metal is extracted from bauxite?

A

Aluminium

142
Q

What are the steps of turning an ore into a metal?

A

Mining -> separation and concentration -> extraction

143
Q

What is the process of turning bauxite into aluminium?

A

7 tonnes of Darling Range bauxite refines to 2 tonnes fo Alumina smelts (uses electricity) to 1 tonne of aluminium

144
Q

Which metals can be recycled?

A

Aluminium, iron (steel)

145
Q

Why is it better to recycle than to extract a new metal from ore?

A

Metals are non renewable
Recycling uses less energy and reduces waste in landfill

146
Q

What is electrolysis?

A

Use of electricity to extract a metal from its ore

147
Q

What extraction method is used for low reactivity metals (gold and silver)?

A

None. Occurs naturally

148
Q

What extraction method is used for extracting copper?

A

Roasting in air

149
Q

What extraction method is used for Zinc-Lead?

A

Smelting

150
Q

What extraction method is used for Potassium-Aluminium?

A

Electrolysis

151
Q

What is the symbol for electrons in chemical equations?

A

e-

152
Q

What is leaching?

A

Dissolving a metal into an acid

153
Q

What should happen after leaching?

A

Sedimentation: solids that aren’t the desired metal settle

154
Q

What is cementation?

A

The process in which dissolved metal ions displace other metalsm to form solid metals (e.g. copper solution becomes cemented copper on steel. T)

155
Q

What is electrowinning?

A

Using electricity to turn a cation into an atom again. The metal ions will become solid metal atoms on the negative electrode

156
Q

What is covalent bonding?

A

Bonding between non-metals

157
Q

How do non-metal atoms reach a full outer shell?

A

Sharing electrons

158
Q

How is a molecule formed by covalent bonds?

A

A small number of non-metal atoms are held together by covalent bonds

159
Q

What is the name for a shared pair of electrons?

A

Covalent bonds

160
Q

Which atom is placed in the middle when a molecule involves more than two atoms?

A

The atom with the most bonding electrons

161
Q

What is an ione pair?

A

Non-bonding electrons that are drawn in apirs around the bonding

162
Q

What is an octet?

A

An element having 8 valence electrons.

163
Q

What is a duet?

A

AN element having 2 valence electrons

164
Q

What is used to draw a covalent bond?

A

A line (or a series of parallel lines)

Science Semester Two (2 decks)

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