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Year 10 MMS > Chemistry - Overall Study > Flashcards

Chemistry - Overall Study Flashcards

1
Q

Define aqueous

A

A physical state of natter which means dissolved in water.

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2
Q

Define agitating

A

Stirring or shaking a mixture

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3
Q

Define activation energy

A

The maximum energy required for a successful collision and therefore to start a reaction

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4
Q

How does a catalyst speed up a chemical reaction?

A

A catalyst helps speed up the chemical reaction by making it easier for particles to reach the activation energy

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5
Q

Why does increasing the temperature of a chemical reaction increase the frequency of successful collisions?

A

The particles are moving at higher speeds, causing them to collide more often and reach the reaction’s activation energy

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6
Q

When heat is applied to a chemical reaction, what energy is it converted into?

A

Kinetic energy

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7
Q

Why does stirring a mixture increase the reaction rate?`

A

Stirring allows particles to collide with one another easier; it increases the rate of collisions

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8
Q

Why does increasing the surface area of a reactant increase reaction rate?

A

More particles are exposed to whatever it needs to react with.

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9
Q

Give two ways that the surface area of a solid can be increased.

A

Cutting up the pieces; grinding into a powder

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10
Q

Why does increasing the pressures of solid and liquid reactants not effect reaction rate?

A

Liquid and solid particles are nearly impossible to compress

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11
Q

TRUE or FALSE

Increasing the concentration of a reactant only affects the frequency of collisions.

A

True

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12
Q

TRUE or FALSE

A dilute solution contains a large number of reactant particles in a given volume

A

False

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13
Q

Give two requirements for a successful chemical reaction

A

Particles must collide; Collide with the right amount of energy

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14
Q

What are the units of relative rate when measuring the production of a solid in a reaction?

A

g/s; grams per second

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15
Q

What are the units of rate when measuring the loss of mass in a reaction?

A

g/s; grams per second

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16
Q

What are the units of rate when measuring the volume of gas produced?

A

mL/s; Milliliters per second

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17
Q

Why is a gas syringe better than using an upturned measuring cylinder?

A

Gas syringes are more accurate

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18
Q

Name two uses of CFCs

A

Refrigerants; propellants in aerosol cans (there are more if y’all wanna add them)

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19
Q

Name the method of preventing the formation of rust

A

Galvanising

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20
Q

Name the reactants used in the final reaction which produces sulfuric acid

A

Sulfur trioxide and water

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21
Q

What is the name of fuels that are made by fermenting sugars?

A

biofuel

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22
Q

Name the micro-organism needed to break down sugars in fermentation

A

yeast

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23
Q

Why are plastics called polymers?

A

because plastics are made up of monomers

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24
Q

Describe an equation that is unbalanced

A

An unbalanced equation does not have the same number of atoms on both sides

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25
Q

What is the main advantage of a molecular equation?

A

You can see how atoms are bonded together

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26
Q

What are molecular diagrams?

A

A visual representation of the arrangements of atoms

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27
Q

Why is salt water described as an aqueous solution?

A

Because aqueous describes a solution dissolved in water ie: salt water

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28
Q

Chlorine is a diatomic molecule. What does this mean?

A

Chlorine contains two atoms bonded together

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29
Q

Give two uses for sulfuric acid

A

Phosphates; metal processing; fibres; hydrofluoric acid; paints; pigments; pulp; paper; phosphate fertilisers.

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30
Q

Name the products of the reaction in a blast furnace

A

Metal used (generally iron) and carbon dioxide (CO2)

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31
Q

How can the pressure of a gas be increased?

A

Either increase the number of particles or decrease the volume of a container

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32
Q

Give the name of the protocol signed by all countries to combat the depletion of the ozone layer by CFCs

A

Montreal Protocol; Montreal Protocol on Substances that Deplete the Ozone Layer

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33
Q

Does covalent bonding involve donation or sharing electrons?

A

Sharing electrons

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34
Q

Why do certain elements form cations and others anions?

A

Elements prefer to have 8 electrons in their outer shell so they either tend to lose or gain electrons, causing them to be charged.

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35
Q

Why are group 1 metals also known as alkali metals?

A

Because they form an alkaline solution when they react to water

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36
Q

Why do alkali metals form +1 ions when they react with other substances?

A

Because they want to give away their single valence electron, causing them to be positively charged.

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37
Q

Why are alkali metals shiny on the inside and dull on the outside?

A

Because alkali metals react to oxygen, forming a dull exterior

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38
Q

List four of the alkaline earth metals

A

Beryllium (Be); Magnesium (Mg); Calcium (Ca); Strontium (Sr); Barium (Ba); Radium (Ra)

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39
Q

Which metal is the most reactive in group 1?

A

Francium (Fr)

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40
Q

What charge do alkali earth metals tend to form when they react?

A

+2

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41
Q

Name three elements in group 17.

A

Fluorine (F); Chlorine (Cl); Bromine (Br); Iodine (I)

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42
Q

Give the charge of a group 17 ion

A

-1

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43
Q

State one trend that can be observed going down group 17

A

The reactivity decreases as you move down the group

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44
Q

Name three elements in group 18

A

Helium (He); Neon (Ne); Argon (Ar); Krypton (Kr); Xenon (Xe)

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45
Q

Why don’t noble gases form ions?

A

They have a full outer shell so they don’t need to gain or lose electrons to be stable

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46
Q

What other name is given to noble gases?

A

inert gases

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47
Q

Name a metal that can be extracted by reacting with carbon

A

Zinc (Zn); Iron (Fe); Lead (Pb); Nickel (Ni); Tin (Sn); Copper (Cu)

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48
Q

Name a metal that can be extracted by electrolysis

A

Potassium (K); Calcium (Ca); Sodium (Na); Magnesium (Mg); Aluminium (Al)

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49
Q

How can we identify the type of element present when electrons are excited?

A

We can use the colour of light to identify elements

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50
Q

What type of energy is emitted when electrons return to ground state?

A

Light energy

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51
Q

What is the reactivity of a chemical element determined by?

A

The valence electron(s)

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52
Q

What is the atomic number of an element with 18 electrons?

A

18

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53
Q

What is the name for atoms when they are at their lowest energy level?

A

Ground state

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54
Q

What is the maximum number of electrons that can be housed in the fourth shell?

A

32

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55
Q

What is the maximum number of electrons that can be housed in the third shell?

A

18

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56
Q

What is the maximum number of electrons that can be housed in the second shell?

A

8

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57
Q

What is the maximum number of electrons that can be housed in the first shell?

A

2

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58
Q

What is the name of the structure in an atom that houses electrons?

A

shell

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59
Q

TRUE or FALSE

Mercury is the only metal that is liquid at room temperature.

A

True

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60
Q

TRUE or FALSE

There are more non-metals than metals

A

False

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61
Q

TRUE or FALSE

Almost all non-metals are liquid

A

False

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62
Q

TRUE or FALSE

Metals have high melting points

A

True

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63
Q

The name given to elements which behave like metals and non-metals is ______

A

Metalloids

64
Q

On which side of the periodic table are metals located?

A

Left side

65
Q

TRUE or FALSE

Lanthanides and actinides are inner transition metals.

A

True

66
Q

What are the block of elements in the middle of the periodic table, containing groups 3 to 12, called?

A

Transition metals

67
Q

TRUE or FALSE

Lithium is in period 1

A

False

68
Q

TRUE or FALSE

Periods are the horizontal rows in the periodic table.

A

True

69
Q

TRUE or FALSE

As strontium is in the same group as silicon, it will have similar properties

A

True*
*note: they are not in the same group so do not use your periodic table as a reference. A better example would be Beryllium and Magnesium as they are both in group 2

70
Q

TRUE or FALSE

Groups are the vertical columns in the periodic table

A

True

71
Q

The discovery of the element _____ proved that Mendeleev’s predictions were correct

A

Germanium

72
Q

How did Mendeleev make his predictions?

A

He made predictions of future elements based off of the properties of known elements

73
Q

What causes electrons to become excited and move up energy levels?

A

When electrons gain energy eg: a flame or a spark

74
Q

Name a metal that can only be extracted through electrolysis

A

Potassium (K); Sodium (Na); Calcium (Ca); Magnesium (Mg); Aluminium (Al)

75
Q

Which metal is at the top of the activity series?

A

Potassium (K)

76
Q

Explain ionic bonding

A

The strong bond between a positively charged cation and negatively charged anion

77
Q

What is the difference between the absorption spectrum and emission spectrum?

A

The absorption spectrum shows gaps in the continuous spectrum where light has been absorbed. The emission spectrum is the inverse of this.

78
Q

Construct a word equation to show the displacement reaction of iron sulfate with zinc.

A

Iron sulfate + zinc —> Sulfate + iron

79
Q

Recall the name of Johann Dobereiner’s groupings in his attempt at organising the elements

A

Dobereiner triads

80
Q

What properties do non-metals have?

A

dull, brittle, low melting & boiling points, poor conductors

81
Q

What properties do metals have?

A

Shiny, high melting & boiling points, malleable, ductile, good conductors

82
Q

What is another name for lanthanides?

A

Rare earth metals

83
Q

What are the special groups of elements?

A

Alkali metals (group 1), Alkaline earth metals (group 2), halogens (group 17), noble gases (group 18)

84
Q

What happens to the reactivity of an element as you move down groups 1 &2? Why?

A

The reactivity increases as it is easier to remove the valence electron

85
Q

Why are alkali metals called this?

A

When they react with water they create an alkaline solution

86
Q

Explain covalent bonding

A

When two non-metals bond together, neither want to lose electrons so they share.

87
Q

How many electrons within an outer shell is considered stable for elements?

A

8

88
Q

What elements do lanthanides include (atomic numbers)?

A

Elements with atomic numbers 58 to 71

89
Q

What elements do actinides include (atomic numbers)?

A

Elements with atomic numbers from 89 to 103

90
Q

What type of elements mostly make up actinides?

A

Synthetic elements

91
Q

What are the lanthanides and actinides?

A

Elements that make up the inner transition metals

92
Q

How many groups are there in the periodic table?

A

18

93
Q

What are ‘groups’ within the periodic table?

A

The vertical columns of the periodic table

94
Q

What are ‘periods’ within the periodic table?

A

The horizontal rows of the periodic table

95
Q

What properties do metalloids have?

A

Generally look like a metal but behave like a non-metal

96
Q

Define group

A

The vertical columns in the periodic table

97
Q

Name two native metals

A

Silver; Gold

98
Q

How can the rate of solid production be measured?

A

Collecting precipitate and measuring it; Placing a cross beneath a conical flask and measuring the time it takes for the cross to disappear.

99
Q

Give one method of monitoring reaction rates.

A

Measuring the quantity of reactant used up; quantity of product formed over time

100
Q

What is the law of conservation of mass?

A

Mass cannot be gained or lost, rather conserved

101
Q

State the three ways gas production can be measured

A

Upturned measuring cylinder, gas syringe, rate off mass loss

102
Q

What is polymerisation

A

The name of the reaction when monomers join together to make a polymer

103
Q

Briefly explain the process of making sulfuric acid

A
  1. Sulfur is extracted
  2. Reacted with oxygen to make sulfur dioxide
  3. Reacted with oxygen to make sulfur trioxide
  4. Reacted with water
104
Q

TRUE or FALSE

Almost all metals are extracted from their ores by a chemical reaction.

A

True

105
Q

Give the two equations for measuring reaction rate.

A

reaction rate = quantity of reactant used up / time

reaction rate = quantity of product formed / time

106
Q

TRUE or FALSE

The steeper the gradient on the graph, the slower the reaction rate

A

False

107
Q

What does CFCs stand for?

A

Chlorofluorocarbons

108
Q

List three factors that can affect reaction rates.

A

Concentration; pressure; stirring (agitation); surface area; temperature; catalyst

109
Q

How can the rate of solid consumption be measured?

A

If the solid pieces can be observed then the time taken for the solid to disappear can be observed

110
Q

Name three diatomic elements on the periodic table.

A

Hydrogen; nitrogen; oxygen; fluorine; chlorine; bromine; iodine

111
Q

What is the state symbol for most acids & alkalis?

A

(aq); aqueous

112
Q

What does the term valency refer to?

A

Valency refers to the combining power of an element with other atoms

113
Q

What is the name of the monomer that is used to make polyethene?

A

ethene monomers

114
Q

Define ionic bond

A

a strong bond between an anion and a cation formed via electron donation

115
Q

Define transitional metals

A

The block of metals containing the elements in groups 3 to 12 and in the period 4 to 7 in the periodic table

116
Q

Create a word equation that produces a gas

A

Hydrochloric acid + calcium carbonate –>

calcium sulfate + carbon dioxide + water

117
Q

Define biofuel

A

a fuel that comes from living materials

118
Q

Define catalyst

A

Speeds up a chemical reaction by lowering the activation energy and does not get used up in the process

119
Q

Define chlorofluorocarbons

A

Chemicals containing atoms of carbon, chlorine and fluorine that are rotoxic and non-flammable

120
Q

Define coefficients

A

the large numbers placed before molecules in a chemical equation to ensure that it is balanced

121
Q

Define collisions

A

particles must collide for a chemical reaction to occur

122
Q

Define concentrated solution

A

a solution which contains a large amount of solute compared to solvent

123
Q

Define concentration

A

the amount of substance in a given space

124
Q

Define diatomic

A

two atoms bonded together

125
Q

Define dilute solution

A

a solution which contains a small amount of solute compared to solvent

126
Q

Define formula equation

A

a chemical reaction written using the formulas of the reactants and products involved

127
Q

Define galvanising

A

coating iron or steel with a protective layer of zinc

128
Q

Define molecular equation

A

a chemical reaction written using the bonding structure of the reactants and products involved

129
Q

Define monatomic

A

one atom

130
Q

Define monomers

A

single units that when joined together repeat to produce a polymer

131
Q

Define polymer

A

a long chained molecule made of repeating sub units called monomers

132
Q

Define products

A

the chemicals produced in a reaction

133
Q

Define reactants

A

the chemicals which react together in a reaction

134
Q

Define reaction rate

A

the quantity of reactant or product used up or made per unit time: how fast the reaction goes

135
Q

Define surface area

A

the area of the outer part or surface of an object

136
Q

Define word equation

A

a chemical reaction written using the names of the reactants and products involved

137
Q

Define activity series

A

a series of metals ordered by their reactivity from highest to lowest

138
Q

Define alkali metals

A

Group 1 metals that form an alkaline solution when they react with water

139
Q

Define alkaline earth metals

A

group 2 metals that form an alkaline solution when they react with water

140
Q

Define anion

A

a negatively charged ion formed from the gain of electrons

141
Q

Define cation

A

a positively charged ion formed from the loss of electrons

142
Q

Define covalent bond

A

a strong bond almost always between two non-metals who share electrons forming a molecule

143
Q

Define displacement reaction

A

when a more reactive metal removes a less reactive metal from its compound

144
Q

Define electron

A

smallest sub-atomic particle in an atom arranged around the nucleus in shells (negatively charged)

145
Q

Define electron shell

A

Houses the electrons which orbit the nucleus of an atom

146
Q

Define electronic configuration

A

the arrangement of an atom’s electrons in the shells around the nucleus

147
Q

Define element

A

a species of atoms that have the same number of protons

148
Q

Define ground state

A

the lowest energy level of an atom

149
Q

Define halogens

A

group 17 elements

150
Q

Define inert

A

unreactive

151
Q

Define ion

A

a charged version of an atom, formed from the loss or gain of electrons

152
Q

Define metalloids

A

elements in the periodic table that are situated close to the border between metals and non-metals; they share properties and appearance characteristics with both metals and non-metals

153
Q

Define native metals

A

Elements that are formed in their pure states in the envirionment

154
Q

Define noble gases

A

group 18 elements

155
Q

Define period

A

the horizontal rows in the periodic table

156
Q

Define valence electrons

A

the electrons in the outer shell of an element

Year 10 MMS (6 decks)

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