Chemistry - Overall Study Flashcards
1
Q
Define aqueous
A
A physical state of natter which means dissolved in water.
2
Q
Define agitating
A
Stirring or shaking a mixture
3
Q
Define activation energy
A
The maximum energy required for a successful collision and therefore to start a reaction
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
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
6
Q
When heat is applied to a chemical reaction, what energy is it converted into?
A
Kinetic energy
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
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.
9
Q
Give two ways that the surface area of a solid can be increased.
A
Cutting up the pieces; grinding into a powder
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
11
Q
TRUE or FALSE
Increasing the concentration of a reactant only affects the frequency of collisions.
A
True
12
Q
TRUE or FALSE
A dilute solution contains a large number of reactant particles in a given volume
A
False
13
Q
Give two requirements for a successful chemical reaction
A
Particles must collide; Collide with the right amount of energy
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
15
Q
What are the units of rate when measuring the loss of mass in a reaction?
A
g/s; grams per second
16
Q
What are the units of rate when measuring the volume of gas produced?
A
mL/s; Milliliters per second
17
Q
Why is a gas syringe better than using an upturned measuring cylinder?
A
Gas syringes are more accurate
18
Q
Name two uses of CFCs
A
Refrigerants; propellants in aerosol cans (there are more if y’all wanna add them)
19
Q
Name the method of preventing the formation of rust
A
Galvanising
20
Q
Name the reactants used in the final reaction which produces sulfuric acid
A
Sulfur trioxide and water
21
Q
What is the name of fuels that are made by fermenting sugars?
A
biofuel
22
Q
Name the micro-organism needed to break down sugars in fermentation
A
yeast
23
Q
Why are plastics called polymers?
A
because plastics are made up of monomers
24
Q
Describe an equation that is unbalanced
A
An unbalanced equation does not have the same number of atoms on both sides
25
What is the main advantage of a molecular equation?
You can see how atoms are bonded together
26
What are molecular diagrams?
A visual representation of the arrangements of atoms
27
Why is salt water described as an aqueous solution?
Because aqueous describes a solution dissolved in water ie: salt water
28
Chlorine is a diatomic molecule. What does this mean?
Chlorine contains two atoms bonded together
29
Give two uses for sulfuric acid
Phosphates; metal processing; fibres; hydrofluoric acid; paints; pigments; pulp; paper; phosphate fertilisers.
30
Name the products of the reaction in a blast furnace
Metal used (generally iron) and carbon dioxide (CO2)
31
How can the pressure of a gas be increased?
Either increase the number of particles or decrease the volume of a container
32
Give the name of the protocol signed by all countries to combat the depletion of the ozone layer by CFCs
Montreal Protocol; Montreal Protocol on Substances that Deplete the Ozone Layer
33
Does covalent bonding involve donation or sharing electrons?
Sharing electrons
34
Why do certain elements form cations and others anions?
Elements prefer to have 8 electrons in their outer shell so they either tend to lose or gain electrons, causing them to be charged.
35
Why are group 1 metals also known as alkali metals?
Because they form an alkaline solution when they react to water
36
Why do alkali metals form +1 ions when they react with other substances?
Because they want to give away their single valence electron, causing them to be positively charged.
37
Why are alkali metals shiny on the inside and dull on the outside?
Because alkali metals react to oxygen, forming a dull exterior
38
List four of the alkaline earth metals
Beryllium (Be); Magnesium (Mg); Calcium (Ca); Strontium (Sr); Barium (Ba); Radium (Ra)
39
Which metal is the most reactive in group 1?
Francium (Fr)
40
What charge do alkali earth metals tend to form when they react?
+2
41
Name three elements in group 17.
Fluorine (F); Chlorine (Cl); Bromine (Br); Iodine (I)
42
Give the charge of a group 17 ion
-1
43
State one trend that can be observed going down group 17
The reactivity decreases as you move down the group
44
Name three elements in group 18
Helium (He); Neon (Ne); Argon (Ar); Krypton (Kr); Xenon (Xe)
45
Why don't noble gases form ions?
They have a full outer shell so they don't need to gain or lose electrons to be stable
46
What other name is given to noble gases?
inert gases
47
Name a metal that can be extracted by reacting with carbon
Zinc (Zn); Iron (Fe); Lead (Pb); Nickel (Ni); Tin (Sn); Copper (Cu)
48
Name a metal that can be extracted by electrolysis
Potassium (K); Calcium (Ca); Sodium (Na); Magnesium (Mg); Aluminium (Al)
49
How can we identify the type of element present when electrons are excited?
We can use the colour of light to identify elements
50
What type of energy is emitted when electrons return to ground state?
Light energy
51
What is the reactivity of a chemical element determined by?
The valence electron(s)
52
What is the atomic number of an element with 18 electrons?
18
53
What is the name for atoms when they are at their lowest energy level?
Ground state
54
What is the maximum number of electrons that can be housed in the fourth shell?
32
55
What is the maximum number of electrons that can be housed in the third shell?
18
56
What is the maximum number of electrons that can be housed in the second shell?
8
57
What is the maximum number of electrons that can be housed in the first shell?
2
58
What is the name of the structure in an atom that houses electrons?
shell
59
TRUE or FALSE
| Mercury is the only metal that is liquid at room temperature.
True
60
TRUE or FALSE
| There are more non-metals than metals
False
61
TRUE or FALSE
| Almost all non-metals are liquid
False
62
TRUE or FALSE
| Metals have high melting points
True
63
The name given to elements which behave like metals and non-metals is ______
Metalloids
64
On which side of the periodic table are metals located?
Left side
65
TRUE or FALSE
| Lanthanides and actinides are inner transition metals.
True
66
What are the block of elements in the middle of the periodic table, containing groups 3 to 12, called?
Transition metals
67
TRUE or FALSE
| Lithium is in period 1
False
68
TRUE or FALSE
| Periods are the horizontal rows in the periodic table.
True
69
TRUE or FALSE
| As strontium is in the same group as silicon, it will have similar properties
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
TRUE or FALSE
| Groups are the vertical columns in the periodic table
True
71
The discovery of the element _____ proved that Mendeleev's predictions were correct
Germanium
72
How did Mendeleev make his predictions?
He made predictions of future elements based off of the properties of known elements
73
What causes electrons to become excited and move up energy levels?
When electrons gain energy eg: a flame or a spark
74
Name a metal that can only be extracted through electrolysis
Potassium (K); Sodium (Na); Calcium (Ca); Magnesium (Mg); Aluminium (Al)
75
Which metal is at the top of the activity series?
Potassium (K)
76
Explain ionic bonding
The strong bond between a positively charged cation and negatively charged anion
77
What is the difference between the absorption spectrum and emission spectrum?
The absorption spectrum shows gaps in the continuous spectrum where light has been absorbed. The emission spectrum is the inverse of this.
78
Construct a word equation to show the displacement reaction of iron sulfate with zinc.
Iron sulfate + zinc ---> Sulfate + iron
79
Recall the name of Johann Dobereiner's groupings in his attempt at organising the elements
Dobereiner triads
80
What properties do non-metals have?
dull, brittle, low melting & boiling points, poor conductors
81
What properties do metals have?
Shiny, high melting & boiling points, malleable, ductile, good conductors
82
What is another name for lanthanides?
Rare earth metals
83
What are the special groups of elements?
Alkali metals (group 1), Alkaline earth metals (group 2), halogens (group 17), noble gases (group 18)
84
What happens to the reactivity of an element as you move down groups 1 &2? Why?
The reactivity increases as it is easier to remove the valence electron
85
Why are alkali metals called this?
When they react with water they create an alkaline solution
86
Explain covalent bonding
When two non-metals bond together, neither want to lose electrons so they share.
87
How many electrons within an outer shell is considered stable for elements?
8
88
What elements do lanthanides include (atomic numbers)?
Elements with atomic numbers 58 to 71
89
What elements do actinides include (atomic numbers)?
Elements with atomic numbers from 89 to 103
90
What type of elements mostly make up actinides?
Synthetic elements
91
What are the lanthanides and actinides?
Elements that make up the inner transition metals
92
How many groups are there in the periodic table?
18
93
What are 'groups' within the periodic table?
The vertical columns of the periodic table
94
What are 'periods' within the periodic table?
The horizontal rows of the periodic table
95
What properties do metalloids have?
Generally look like a metal but behave like a non-metal
96
Define group
The vertical columns in the periodic table
97
Name two native metals
Silver; Gold
98
How can the rate of solid production be measured?
Collecting precipitate and measuring it; Placing a cross beneath a conical flask and measuring the time it takes for the cross to disappear.
99
Give one method of monitoring reaction rates.
Measuring the quantity of reactant used up; quantity of product formed over time
100
What is the law of conservation of mass?
Mass cannot be gained or lost, rather conserved
101
State the three ways gas production can be measured
Upturned measuring cylinder, gas syringe, rate off mass loss
102
What is polymerisation
The name of the reaction when monomers join together to make a polymer
103
Briefly explain the process of making sulfuric acid
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
TRUE or FALSE
| Almost all metals are extracted from their ores by a chemical reaction.
True
105
Give the two equations for measuring reaction rate.
reaction rate = quantity of reactant used up / time
| reaction rate = quantity of product formed / time
106
TRUE or FALSE
| The steeper the gradient on the graph, the slower the reaction rate
False
107
What does CFCs stand for?
Chlorofluorocarbons
108
List three factors that can affect reaction rates.
Concentration; pressure; stirring (agitation); surface area; temperature; catalyst
109
How can the rate of solid consumption be measured?
If the solid pieces can be observed then the time taken for the solid to disappear can be observed
110
Name three diatomic elements on the periodic table.
Hydrogen; nitrogen; oxygen; fluorine; chlorine; bromine; iodine
111
What is the state symbol for most acids & alkalis?
(aq); aqueous
112
What does the term valency refer to?
Valency refers to the combining power of an element with other atoms
113
What is the name of the monomer that is used to make polyethene?
ethene monomers
114
Define ionic bond
a strong bond between an anion and a cation formed via electron donation
115
Define transitional metals
The block of metals containing the elements in groups 3 to 12 and in the period 4 to 7 in the periodic table
116
Create a word equation that produces a gas
Hydrochloric acid + calcium carbonate -->
| calcium sulfate + carbon dioxide + water
117
Define biofuel
a fuel that comes from living materials
118
Define catalyst
Speeds up a chemical reaction by lowering the activation energy and does not get used up in the process
119
Define chlorofluorocarbons
Chemicals containing atoms of carbon, chlorine and fluorine that are rotoxic and non-flammable
120
Define coefficients
the large numbers placed before molecules in a chemical equation to ensure that it is balanced
121
Define collisions
particles must collide for a chemical reaction to occur
122
Define concentrated solution
a solution which contains a large amount of solute compared to solvent
123
Define concentration
the amount of substance in a given space
124
Define diatomic
two atoms bonded together
125
Define dilute solution
a solution which contains a small amount of solute compared to solvent
126
Define formula equation
a chemical reaction written using the formulas of the reactants and products involved
127
Define galvanising
coating iron or steel with a protective layer of zinc
128
Define molecular equation
a chemical reaction written using the bonding structure of the reactants and products involved
129
Define monatomic
one atom
130
Define monomers
single units that when joined together repeat to produce a polymer
131
Define polymer
a long chained molecule made of repeating sub units called monomers
132
Define products
the chemicals produced in a reaction
133
Define reactants
the chemicals which react together in a reaction
134
Define reaction rate
the quantity of reactant or product used up or made per unit time: how fast the reaction goes
135
Define surface area
the area of the outer part or surface of an object
136
Define word equation
a chemical reaction written using the names of the reactants and products involved
137
Define activity series
a series of metals ordered by their reactivity from highest to lowest
138
Define alkali metals
Group 1 metals that form an alkaline solution when they react with water
139
Define alkaline earth metals
group 2 metals that form an alkaline solution when they react with water
140
Define anion
a negatively charged ion formed from the gain of electrons
141
Define cation
a positively charged ion formed from the loss of electrons
142
Define covalent bond
a strong bond almost always between two non-metals who share electrons forming a molecule
143
Define displacement reaction
when a more reactive metal removes a less reactive metal from its compound
144
Define electron
smallest sub-atomic particle in an atom arranged around the nucleus in shells (negatively charged)
145
Define electron shell
Houses the electrons which orbit the nucleus of an atom
146
Define electronic configuration
the arrangement of an atom's electrons in the shells around the nucleus
147
Define element
a species of atoms that have the same number of protons
148
Define ground state
the lowest energy level of an atom
149
Define halogens
group 17 elements
150
Define inert
unreactive
151
Define ion
a charged version of an atom, formed from the loss or gain of electrons
152
Define metalloids
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
Define native metals
Elements that are formed in their pure states in the envirionment
154
Define noble gases
group 18 elements
155
Define period
the horizontal rows in the periodic table
156
Define valence electrons
the electrons in the outer shell of an element
