1What type of ions do metals react to form?
Positive ions
2Where are metals typically found on the periodic table?
- To the left and towards the bottom
- To the right and towards the top
- In the center only
- Along the diagonal line
3What do metal atoms do with electrons when forming ions?
Lose electrons
4What are typical physical properties of metals?
- Shiny, dense, and good electrical conductors
- Dull, low density, and poor conductors
- Clear, brittle, and non-conductive
- Gaseous, low melting point, and dull
5What type of ions do non-metals react to form?
Negative ions
6Where are non-metals typically found on the periodic table?
- Towards the right and top
- Towards the left and bottom
- In the middle
- Only in the bottom row
7What do non-metal atoms do with electrons when forming ions?
Gain electrons
8What are typical physical properties of non-metals?
- Dull, poor electrical conductors, and low melting points
- Shiny, dense, and high melting points
- Heavy, malleable, and good conductors
- Magnetic, ductile, and high density
9How are elements ordered in the periodic table?
In order of atomic (proton) number
10What are columns in the periodic table known as?
Groups
11What does the group number of an element represent?
The number of outer shell electrons
12What does the period number of an element represent?
The number of shells of electrons
13Between what types of elements is ionic bonding formed?
A metal and a non-metal
14What happens to electrons during ionic bonding between a metal and a non-metal?
Electrons in the outer shell of the metal atom are transferred to the non-metal
15What holds ionic compounds together?
Strong electrostatic forces of attraction between oppositely charged ions
16What structure do ionic compounds have?
Regular structures (giant ionic lattices)
17Why do ionic compounds have high melting and boiling points?
A lot of energy is required to break the many strong bonds
18Why do ionic compounds conduct electricity when melted or dissolved in water?
The ions are free to move and carry current
19What type of bonding occurs in simple molecules?
Covalent bonding
20What are the particles in simple molecules?
Atoms which share pairs of electrons
21What type of forces exist between simple molecules?
Weak intermolecular forces
22Which forces are broken when simple molecules melt or boil?
Intermolecular forces
23Why do larger simple molecules have higher melting and boiling points?
The intermolecular forces increase with the size of the molecules
24Why don't substances consisting of simple molecules conduct electricity?
Simple molecules do not have an overall electric charge
25What state of matter are substances with giant covalent structures at room temperature?
Solids
26What type of bonds link all the atoms in giant covalent structures?
Strong covalent bonds
27What type of bonding occurs in polymers?
Covalent bonding
28Why are polymers solids at room temperature?
Intermolecular forces between polymer molecules are relatively strong
29What type of bonding occurs in metals?
Metallic bonding
30How are metal atoms arranged in metals?
Giant structures of atoms arranged in a regular pattern
31What are the outer shell electrons in metal atoms described as?
Delocalised
32What gives rise to strong metallic bonds?
The sharing of delocalised electrons
33Why can metals be bent and shaped?
The layers of atoms are able to slide over each other
34What is an ionic bond defined as?
Electrostatic attraction between oppositely charged ions, formed by the transfer of electrons
35What is a covalent bond defined as?
Electrostatic attraction between a shared pair of electrons
36What is a metallic bond defined as?
Electrostatic attraction between positive metal ions and the sea of delocalised electrons
37What is a limitation of dot and cross diagrams?
They do not show the 3D arrangement of molecules
38What is a limitation of ball and stick models?
They do not show the electrons or the chemical symbols
39What do 2D and 3D models generally fail to show simultaneously?
- 2D models don't show 3D arrangements and 3D models don't give details of bonding or electrons
- Both show all bonding details equally
- Neither shows atom symbols
- Both include intermolecular forces
40How many electrons can the first electron shell hold?
Up to 2 electrons
41How many electrons can the second electron shell hold?
Up to 8 electrons
42How many electrons can the third electron shell hold?
Up to 8 electrons
43How many electrons do atoms try to acquire in their outer shell for stability?
8 electrons (unless they only have one shell, which tries for 2)
44In what order did Mendeleev initially order his periodic table?
Atomic mass
45What did Mendeleev do for elements that he thought had not been discovered yet?
Left gaps
46What knowledge made it possible to explain why the order based on atomic weights was not always correct?
Isotopes
47How many covalent bonds can carbon form?
4
48What enables the vast array of natural and synthetic organic compounds to occur?
Carbon's ability to form families of similar compounds, chains, and rings
49How many other carbon atoms is each carbon joined to covalently in diamond?
4
50What are the physical properties of diamond?
- Very hard, very high melting point, and does not conduct electricity
- Soft, slippery, low melting point, and conducts electricity
- Soft, high density, and good conductor
- Gaseous, low melting point, and dull
51How many other carbon atoms is each carbon covalently bonded to in graphite?
3
52What shape do the carbon atoms form in layers within graphite?
Hexagonal rings
53Why can layers in graphite slide over each other?
Because there are no covalent bonds between the layers, only weak intermolecular forces
54What makes graphite soft and slippery?
The layers sliding over each other due to weak intermolecular forces
55What is special about one electron from each carbon atom in graphite?
It is delocalised
56Why can graphite conduct electricity unlike diamond?
Because it has delocalised electrons
57What are fullerenes?
Molecules of carbon atoms with hollow shapes based on hexagonal rings
58What was the first fullerene to be discovered?
Buckminsterfullerene C60
59What is the shape of Buckminsterfullerene C60?
Spherical
60What are carbon nanotubes?
Cylindrical fullerenes with very high length to diameter ratios
61What is graphene?
A single layer of graphite
62During which changes of state is energy transferred TO a compound?
Melting and boiling
63During which changes of state is energy transferred FROM a compound?
Condensing and freezing
64How strong are covalent and ionic bonds?
Very strong
65Why are simple molecules melted or boiled easily?
Because weak intermolecular forces are overcome, not the covalent bonds
66Why do macromolecular substances have very high melting points and are hard to break down?
Because covalent bonds must be overcome
67What is the state of a substance at a temperature below its melting point?
Solid
68What is the state of a substance at a temperature between its melting and boiling points?
Liquid
69What is the state of a substance at a temperature above its boiling point?
Gas
70Why do materials have different properties compared to their bulk chemical form?
Because of their high surface area to volume ratio
71What is the size range of nanoparticles across?
1 to 100 nanometers
72How many atoms do nanoparticles typically contain?
A few hundred atoms
73What are fine particles PM2.5 diameters between?
100 and 2500 nm (1x10^-7 m and 2.5x10^-6 m)
74What are coarse particles PM10 also commonly referred to as?
Dust
75What happens to the surface area to volume ratio as the side of a cube decreases by a factor of 10?
It increases by a factor of 10
76Why are nanoparticles more reactive than center atoms in bulk material?
Atoms on the surface are often more reactive, and nanoparticles have a very large surface area to volume ratio
77Why do nanoparticles make good catalysts?
They have a high surface area to volume ratio
78What are potential uses of carbon nanotubes in building materials?
Making stronger, lighter building materials
79Why are nanoparticles used in cosmetics like sun tan cream and deodorant?
They make no white marks
80How are nanoparticle lubricant coatings used?
To reduce friction in artificial joints and gears
81Why can carbon nanotubes be used in small electrical circuits for computers?
Because they conduct electricity
82Why are the full risks of nanoparticulate materials not fully known yet?
Because they are still being created and tested
83What is a major potential medical risk associated with nanoparticulate materials?
Problems with how they interact with our cells
84What does the law of conservation of mass state about mass in a chemical reaction?
No atoms are lost or made, so the mass of the products equals the mass of the reactants
85What is stoichiometry in a chemical reaction?
The balancing numbers in front of compounds and elements in reaction equations
86What is the name of the reactant that is completely used up and limits the amount of products formed?
The limiting reactant
87What is an exothermic reaction?
A reaction that transfers energy to the surroundings so the temperature of the surroundings increases
88What is an endothermic reaction?
A reaction that takes in energy from the surroundings so the temperature of the surroundings decreases
89What is activation energy?
The minimum amount of energy that particles must have to react
90What happens to energy during bond breaking and bond making in a chemical reaction?
Energy is taken in to break bonds, and energy is released when bonds are formed
91What type of energy change occurs if the energy needed to break bonds is greater than the energy released?
Endothermic
92What does the acronym OIL RIG stand for in chemistry?
- Oxidation Is Loss, Reduction Is Gain
- Oxidation Is Gain, Reduction Is Loss
- Oxygen Is Lost, Reduction Is Gained
- Overall Ion Loss, Reaction Ion Gain
93What do acids form when they dissolve in water?
Hydrogen ions (H+)
94What do solutions of alkalis contain or release when dissolved in water?
Hydroxide ions (OH-)
95What is neutralisation defined as?
Acid reacting with an alkali or a base to form a salt plus water
96What is the ionic equation for any reaction of an acid with an alkali?
H+ + OH- -> H2O
97What are the products when an acid reacts with a metal carbonate?
Salt + water + carbon dioxide
98What are the products when an acid reacts with a metal?
Salt + hydrogen gas
99What type of salt does hydrochloric acid produce?
Chlorides
100What type of salt does nitric acid produce?
Nitrates
101What type of salt does sulfuric acid produce?
Sulfates
102What is a strong acid?
An acid that is completely ionised in aqueous solution
103What is a weak acid?
An acid that is partially ionised in aqueous solution
104What happens to the hydrogen ion concentration as the pH decreases by one unit?
It increases by a factor of 10
105What does the pH scale measure?
The acidity or alkalinity of a solution
106What is the pH value of a neutral solution?
7
107What color does methyl orange turn in acidic solutions?
Red
108What color does phenolphthalein turn in alkaline solutions?
Pink
109What color does red litmus paper turn in alkaline solutions?
Blue
110What color does blue litmus paper turn in acidic solutions?
Red
111During electrolysis using inert electrodes, where are metals or hydrogen formed?
At the cathode
112During electrolysis using inert electrodes, where are non-metals formed?
At the anode
113What happens to positive ions (cations) at the cathode during electrolysis?
They receive electrons and are reduced
114What happens to negative ions (anions) at the anode during electrolysis?
They lose electrons and are oxidised
115In the electrolysis of an aqueous ionic solution, what is produced at the cathode if the metal is more reactive than hydrogen?
Hydrogen
116In the electrolysis of an aqueous ionic solution, what is produced at the anode if the solution contains halide ions?
The halogen
117What electrode process occurs at the anode?
Loss of electrons (oxidation)
118What electrode process occurs at the cathode?
Gain of electrons (reduction)
119Why are inert electrodes used in electrolysis?
To prevent unwanted reactions between the electrodes and the solution when the products are reactive
120What is the formula to calculate moles from mass and relative formula mass?
Moles = Mass / Relative formula mass (Mr)
121What is the numerical value and definition of the Avogadro constant?
6.02x10^23 atoms, molecules, or ions per mole
122What do the state symbols s, l, g, and aq represent in chemical equations?
Solid, liquid, gas, and aqueous
123Why does the mass of a metal appear to increase when it reacts with oxygen in an open system?
Because oxygen from the air is added, making the mass of the metal oxide product greater than the starting metal
124What are everyday examples of exothermic reactions?
- Self-heating cans and hand warmers
- Sports injury packs and thermal decomposition
- Melting ice and evaporation
- Photosynthesis and thermal cracking
125What are examples of endothermic reactions?
- Thermal decomposition and the reaction of citric acid with sodium hydrogencarbonate
- Combustion and neutralisation
- Oxidation of metals and respiration
- Precipitation of salts
126How is the overall energy change of a reaction calculated using bond energies?
Sum of energy to break bonds minus sum of energy released by forming bonds
127What organic substance is formed when ethanol is oxidised?
Ethanoic acid
128What color are methyl orange indicator solutions in acidic, neutral, and alkaline conditions?
- Red in acidic, yellow in neutral, and yellow in alkaline
- Colourless in acidic and pink in alkaline
- Red in acidic and blue in alkaline
- Yellow in acidic and red in alkaline
129What color does phenolphthalein turn in alkaline solutions?
Pink
130What are the products of the electrolysis of a sodium chloride solution using inert electrodes?
Hydrogen gas at the cathode and chlorine gas at the anode
131What are the products of the electrolysis of a copper sulfate solution using inert electrodes?
Solid copper at the cathode and oxygen gas at the anode
132Why are non-inert electrodes used during the purification of copper?
To use pure and impure copper electrodes where material is transferred from the impure electrode to the pure one
133What is the diameter size range for fine particles PM2.5?
100 to 2500 nm (1x10^-7 m and 2.5x10^-6 m)
134What are coarse particles PM10 commonly referred to as?
Dust
135What are the properties of Group 1 alkali metals due to their outer shell?
They have a single electron in their outer shell
136How do Group 1 alkali metals react with water?
Vigorously to create an alkaline solution and hydrogen
137What do Group 1 metals form when they react with oxygen?
An oxide
138What do Group 1 metals form when they react with chlorine?
A white precipitate
139What happens to the reactivity of Group 1 elements as you go down the group?
It increases
140How many electrons do Group 0 noble gases have in their outer shell?
8 electrons (except helium which has 2)
141Why are Group 0 noble gases unreactive?
Because they have a stable arrangement of electrons
142What happens to the boiling points of noble gases going down the group?
They increase with increasing relative atomic mass
143How many electrons do Group 7 halogens have in their outer shell?
7 electrons
144What type of molecules do halogens consist of?
Pairs of atoms
145What charge does a halide ion carry when halogens react with metals to form ionic compounds?
-1 charge
146What can a more reactive halogen do in an aqueous solution of its salt?
Displace a less reactive halogen
147Why do halogens become less reactive as you go down the group?
Because the higher the energy level of the outer electrons, the less easily electrons are gained
148Compared to Group 1 metals, how do transition metals compare in hardness and strength?
They are harder and stronger
149What is the exception to transition metals having higher melting points than Group 1?
Mercury
150What are typical properties of transition metal compounds?
- Ions with many different charges, form coloured compounds, and act as catalysts
- Low melting points, highly reactive, and white compounds
- Single charge ions, colourless solutions, and poor catalysts
- Gaseous state at room temperature and neutral pH
151What does the group number of an element in the periodic table indicate?
How many electrons are in its outer shell
152What is the general word equation for the reaction of a metal with a dilute acid?
Metal + dilute acid -> salt + hydrogen
153What is the general word equation for the reaction of most metals with water?
Metal + water -> metal hydroxide + hydrogen
154How can you determine the order of reactivity of metals experimentally?
By observing the vigour of their reactions with water or dilute acids
155What is the test and positive result for carbon dioxide gas?
Bubble the gas through limewater (calcium hydroxide) and it turns milky or cloudy
156What is the test and positive result for chlorine gas?
Put damp litmus paper into the gas and it is bleached and turns white
157What is the test and positive result for hydrogen gas?
Hold a burning splint at the open end of a test tube and it creates a squeaky pop sound
158What is the test and positive result for oxygen gas?
Insert a glowing splint into a test tube and the splint relights
159What color precipitate forms when sodium hydroxide is added to a calcium solution?
White precipitate
160What color precipitate forms when sodium hydroxide is added to a copper (II) solution?
Blue precipitate
161What color precipitate forms when sodium hydroxide is added to an iron (II) solution?
Green precipitate
162What color precipitate forms when sodium hydroxide is added to an iron (III) solution?
Orange-brown precipitate
163What happens to the white precipitate formed when excess sodium hydroxide is added to a zinc solution?
The precipitate re-dissolves
164How do carbonate ions react with dilute acids?
They react to create carbon dioxide gas
165What reagents are added first to test for halide ions?
Dilute nitric acid followed by silver nitrate solution
166What color precipitate does a chloride ion give with silver nitrate?
White precipitate
167What color precipitate does a bromide ion give with silver nitrate?
Cream precipitate
168What color precipitate does an iodide ion give with silver nitrate?
Yellow precipitate
169What reagents are added first to test for sulfate ions?
Dilute hydrochloric acid followed by barium chloride solution
170What is the positive result for sulfate ions using barium chloride?
A white precipitate forms
171How is a flame test performed?
Take a sample of the metal on a spatula in a Bunsen burner flame and observe the colour
172What flame test color does lithium produce?
Crimson
173What flame test color does sodium produce?
Yellow
174What flame test color does potassium produce?
Lilac
175What flame test color does copper (II) produce?
Green
176What flame test color does calcium produce?
Orange-red
177What are the advantages of instrumental methods of analysis?
They are accurate, sensitive, and rapid
178What is the formula relating concentration, moles, and volume in solution?
Moles = concentration x volume (mol = mol/dm3 x dm3)
179What effect does a smaller volume or larger number of moles have on solution concentration?
Higher concentration
180What effect does a larger volume or smaller number of moles have on solution concentration?
Lower concentration
181What are the steps of titration to measure reacting volumes of acid and alkali?
Add acid to burette, add known volume of alkali and indicator to conical flask, place on white tile, add acid to end point, calculate titre, and repeat for concordant titres
182What is the conversion between cubic decimetres and cubic centimetres?
1 dm3 = 1000 cm3
183What volume does one mole of any gas occupy at room temperature and pressure (RTP)?
24 dm3
184What is the formula to calculate the volume of a gas in dm3 at RTP from moles?
Volume in dm3 at RTP = moles x 24
185What is the formula to calculate the volume of a gas in cm3 at RTP from moles?
Volume in cm3 at RTP = moles x 24000
186What is the formula for percentage yield?
Percentage yield = (amount of product produced / maximum amount of product possible) x 100
187What is atom economy a measure of?
The amount of reactants that become useful products or the efficiency of a reaction
188What is the formula to calculate atom economy?
Atom economy = (Mr of desired product / sum of Mr of all reactants) x 100
189What factors should be considered when choosing a reaction pathway for a product?
Atom economy, yield, rate, equilibrium position, and usefulness of by-products
190What are the two equations to calculate the rate of reaction using reactants or products?
Rate = amount of reactant used / time OR amount of product formed / time
191What are common units for the rate of reaction?
g/s, cm3/s, or mol/s
192What apparatus can be used to measure the volume of a gas produced in a reaction?
Gas syringe, upside-down measuring cylinder, or burette
193What does the gradient of a rate of reaction graph represent?
The rate of reaction
194What factors increase the rate of reaction when increased?
Temperature, pressure, concentration, or surface area
195How does increasing temperature affect particle collisions and rate?
Increases particle speed, frequency, and energy of collisions, increasing rate
196How does increasing concentration or pressure affect collisions and rate?
Increases the frequency of collisions
197How does increasing the surface area to volume ratio affect the rate of reaction?
Provides more surfaces for reaction, increasing collision frequency and rate
198What is a catalyst?
A substance that speeds up chemical reactions without being changed or used up
199How do catalysts increase the rate of reaction?
By providing an alternative pathway with a lower activation energy
200What are enzymes?
Biological catalysts
201What is a reversible reaction?
A reaction where products can react to produce the original reactants
202When does dynamic equilibrium occur in a closed system?
When the rates of forward and reverse reactions are equal
203What does Le Chatelier's principle state?
If a system is at equilibrium and a condition is changed, the system responds to counteract the change
204What happens to the position of equilibrium if the concentration of reactants is increased?
Shifts towards products (right)
205What happens to the position of equilibrium if the concentration of products is increased?
Shifts towards reactants (left)
206In gaseous reactions, what does an increase in pressure favour?
The reaction that produces the least number of molecules (fewer moles)
207What happens to equilibrium when temperature is increased?
Equilibrium moves in the direction of the endothermic reaction
208What happens to equilibrium when temperature is decreased?
Equilibrium moves in the direction of the exothermic reaction