GCSE OCR Chemistry B Paper 1 Automarked

#1. Complete the following half equation for a reaction the cathode during electrolysis of molten zinc chloride. Zn²⁺ + ….. → Zn

2e

Zn

e

ZnO

#2. What is the chemical symbol for mercury?

#3. Ernest Rutherford fired positive particles at a thin gold foil and showed that most of atoms is empty space. Which particles did he fire at the gold foil?

beta particles

gamma rays

alpha particles

#4. Why does the temperature of a material stay constant during the transition from liquid to gas?

the particles are figuring out what to do

the temperature is not relevant to states of matter

the particles are breaking the bonds with surrounding particles - this takes energy

#5. What state of matter has particles which are far apart and move around independently?

solids

liquids

gases

#6. What is the symbol for relative atomic mass?

Aᵣ

AMᵣ

Mᵣ

Gᵣ

#7. What evidence supports the notion that human activities are contributing to climate change?

Gradual climate warming has occurred since the evolution of our species

Correlation between increases in atmospheric temperatures and historic releases of greenhouse gases, due to combustion of fossil fuels

#8. Are non-metals usually malleable or brittle?

Malleable

Brittle

#9. Iron is turned into iron oxide when exposed to the air. This is a process also known as rusting. Is the rate of reaction fast or slow in rusting?

Slow

Fast

#10. Which description best describes mixtures?

contains more than one type of atoms, chemically bonded together

contains only a particular type of atoms

contains more than one type of atoms, but not chemically bonded together

#11. Can Rf values be higher than 1?

Yes

No

Under certain conditions

#12. Solutions of more than pH 7 are?

alkaline

acidic

neutral

#13. True or false – You cannot use physical processes to separate mixtures into different substances.

False

True

#14. Temperature affects the rate of reaction. Which of the following is the correct description of what happens when temperature changes?

As temperature increases, rate of reaction increases

As temperature increases, rate of reaction decreases

Rate of reaction is highest at very high and very low temperatures

#15. Paper chromatography is used to separate which types of materials?

separating soluble compounds

separate soluble materials from insoluble materials

separate different types of liquids

#16. What is the formula for potassium hydroxide?

HNO₃

KOH

HCL

Ca(OH)₂

H₂SO₄

NaOH

#17. Calculate the relative formula mass of copper oxide (CuO) to 2 decimal places. Copper Aᵣ = 63.5, Oxygen Aᵣ = 16.

#18. What is the charge of a proton?

-1

0

+1

#19. Which of the following is the chemical test for oxygen?

An audible squeaky pop is heard when a lit splint is exposed to a test tube full of oxygen

Oxygen is bubbled through limewater and it turns cloudy when oxygen is present

A glowing splint is relit in a test tube filled with oxygen

#20. What is the chemical symbol for sodium?

#21. Why is graphite softer than diamond?

Graphite is softer because the covalent bonds are weaker between atoms of carbon in graphite than in diamond

Graphite is arranged in sheets with weak intermolecular forces holding them together. These can easily slide, making graphite soft.

Graphite is actually harder than diamond

#22. Which type of reaction is photosynthesis?

Exothermic

Ectothermic

Endothermic

#23. What is the current composition of the Earth’s atmosphere?

78% nitrogen, 21% oxygen, 0.9% argon, and 0.1% other gases

78% carbon dioxide, 21% oxygen, 0.9% argon, and 0.1% other gases

78% oxygen, 21% nitrogen, 0.9% argon, and 0.1% other gases

#24. Which of the following are properties of ionic compounds?

conduct electricity as solids

conduct electricity when molten or dissolved

usually insoluble

usually soluble

high melting and boiling points

low melting and boiling points

#25. What is the name of the force that holds together ions in ionic compounds?

gravity

electrostatic force

strong nuclear force

weak nuclear force

#26. Complete the following equation: MgO (s) + H₂SO₄ (aq) → …. + ….

Select all that apply:

H₂O (l)

MgSO₄ (aq)

HO (l)

MgS₂

MgS (g)

Neutralisation reactions follow the general structure –

metal oxide acid = salt water

the acid produces hydrogen ions and the metal oxide produces oxide ions – these combine to make the water

the salt is comprised of the remaining products – the metal and the other element from the acid

in this case, the other element is chlorine

The naming convention is to put the metal first for the salt created

#27. In aqueous solutions such as sodium chloride solution, there will be negatively charged ions from the salt (Cl⁻) as well as hydroxide ions (OH⁻). What is the rule that determines which will be discharged at the anode.

Always the hydroxide, unless a halide (group 7) is present.

Always the other ions and never the hydroxide

Always the hydroxide regardless of the other ions

#28. Fill in the gap. Metal atoms bond forming a giant ……… of ions.

Ball

Lattice

Lettuce

Anchor

#29. Why is magnesium a better electrical conductor than sodium?

Group 2 magnesium has two spare electrons to donate to the delocalised pool, whereas, sodium atoms only have one electron to donate. This means there are more electrons to carry the charge

Group 1 sodium is less electrically conductive because it quickly forms impurities that prevent efficient conduction

#30. Will endothermic reactions continue if there is no energy input?

No, even if there are still reactants

Yes, until reactants run out

#31. During a neutralisation reaction which salt is formed from sulfuric acid?

Sulfate

Carbonate

Nitrate

Chloride

Borate

#32. Increasing the concentration of solutions increases the rate of reaction, why is this the case?

When solutions are more concentrated, the intermolecular forces become weaker and bonds are more easily broken

When solutions are dilute, there are more particles in the same volume

More collisions take place because there are more particles in the same volume

#33. Oxygen is in group 6 and fluorine is in group 7. How many fluorine atoms bond with one oxygen atom?

#34. Where is most of the mass of an atom?

in the nucleus

orbiting the nucleus in the electrons

#35. What method can we use to separate multiple types of liquids?

#36. When using inert electrodes to perform electrolysis with sodium sulfate solution, which products will be produced at the anode and cathode?

Cathode: Hydrogen (H₂) Anode: Sulfate (SO₄²⁻)

Cathode: Hydrogen (H₂) Anode: Hydroxide (OH⁻)

Cathode: Sodium (Na) Anode: Hydroxide (OH⁻)

#37. What is the chemical symbol for oxygen?

#38. Can compounds be pure, for example, carbon dioxide?

no

yes

#39. During Ernest Rutherford’s experiments with gold foil, why did some of the particles bounce back?

He fired electrons at the gold foil and when they met protons they were reflected back

Alpha particles are positively charged, they were deflected when they met the positively charged protons in the nucleus

Alpha particles behave in unpredictable ways and can randomly change direction due to quantum effects

#40. Do metals usually have a high or low density?

Low density

High density

#41. Which of the following descriptions matches the Mᵣ of a compound?

The sum of the relative atomic masses of all of the atoms or ions in its formula

The simplest whole number ratio of atoms

The mean mass of an atom compared with carbon-12

#42. Which of the following descriptions matches the Aᵣ of an element?

The sum of the relative atomic masses of all of the atoms or ions in its formula

The mean mass of an atom compared with carbon-12

The simplest whole number ratio of atoms

#43. Which description most accurately describes covalent bonding

electrons are transferred between atoms

electrons are shared between atoms

#44. What is the chemical symbol for carbon?

#45. Which of the following are the main sources of drinking water in the UK?

Select all that apply:

rivers

seawater

lakes

aquifers

#46. Isotopes of atoms have different numbers of which particles?

Protons

Neutrons

#47. What is the formula for the polyatomic ion nitrate?

NO₃⁻

SO₃²⁻

CO₃²⁻

OH⁻

NH₄⁺

SO₄²⁻

#48. What do we use fullerenes for?

as fuel in high performance internal combustion engines and in electric car batteries

nanoelectronics, delivery of medicines within the body and strengthening tennis racket frames

#49. What is a simple molecular structure?

a giant structure where each atom has a covalent bond to its neighbour

a compound which contains atoms covalently bonded together, but with weak intermolecular forces between molecules

Ionically bonded substances such as sodium bromide

#50. During electrolysis which electrode do anions and cations migrate to?

Anions to the cathode, cations to the anode

Anions to the anode, cations to the cathode

#51. The table shows 3 substances and their melting points. What common substance, in particular, could substance Z be?

#52. When using inert electrodes to perform electrolysis with molten lead bromide, which products will be produced at the anode and cathode?

Cathode: Bromine (Br₂) (g) Anode: Lead (Pb) (s)

Cathode: Hydrogen (H₂) (g) Anode: Lead (Pb) (s)

Cathode: Lead (Pb) (s) Anode: Bromine (Br₂) (g)

#53. How could we accurately monitor the rate of a reaction? ? Three answers

Select all that apply:

By measuring the changes in mass of reactants and products

By measuring the temperature throughout a reaction

By measuring the concentration of reactants and products throughout a reaction

By measuring the changes in volume of reactants and products

#54. What is the name of the phase change from gas to solid?

deposition

melting

condensation

evaporation/boiling

sublimation

freezing

#55. What is the name of the apparatus used for distillation?

#56. Greenhouse effect 1) Fill in the blanks: Energy from the sun in the form of …….. hits the Earth’s surface and ……. are emitted back towards the atmosphere.

Sound waves, ocean waves

Gravitational waves, ultraviolet waves

Visible/infrared waves, infrared waves

#57. What are negative ions called?

#58. Which type of reaction takes in energy, making the surroundings cooler?

Exothermic

Ectothermic

Endothermic

#59. Lead has 4 stable isotopes. ²⁰⁴Pb (abundance – 1.4%), ²⁰⁵Pb (abundance – 24.1%), ²⁰⁷Pb (abundance – 22.1%) and ²⁰⁸Pb (abundance – 52.4%). Calculate the Aᵣ of lead. Answer to 2 decimal places.

#60. Copper can be purified using electrolysis of copper sulfate solution. For this process we use the setup in the image below. Complete the half equation for the reaction at the anode. Cu → ….. + …..

Cu⁺ + e

Cu²⁺ + 2e

SO₃²⁻ + 2e

#61. What is the mass number of an element?

the total number of subatomic particles in an atom

the number of protons plus neutrons

#62. What is the charge of an electron?

+1

0

-1

#63. What is the chemical symbol for phosphorus?

#64. Energy is transferred between the environment and reactants during a chemical reaction. What form is this energy usually in?

Chemical

Electrical

Thermal

#65. Is water an example of a covalent compound?

Yes

No

#66. What is the formula for the compound calcium nitrate which is made of calcium and nitrate ions (NO₃⁻)?

Ca(NO₂)₂

CaNO₂

Ca(NO₃)₂

#67. Which types of atoms can be found in a pure piece of gold?

Select all that apply:

trace amounts of other elements

carbon atoms

gold atoms

#68. Which of the following was the Rutherford Model of atomic structure?

A central nucleus containing protons and neutrons, surrounded by electrons

A mass of positively charged material with negatively charged electrons distributed throughout it

#69. During a neutralisation reaction which salt is formed from nitric acid?

Chloride

Sulfate

Nitrate

Carbonate

Borate

#70. Which of these is a problem with metallic models?

The model does not show that the ions will be constantly vibrating

The model shows the atoms as being too far apart and there are no sticks

They do not show how the structure formed and suggest that the electrons in different atoms are different, but they are actually the same

#71. In aqueous solutions such as sodium chloride solution, there will be positively charged ions from the salt (Na⁺) as well as hydrogen ions (H⁺). What is the rule that determines which will be discharged at the cathode.

The most reactive ions

Always the ions from the salt e.g. Na⁺

The least reactive ions

#72. What is the name of the phase change from liquid to gas?

melting

evaporation/boiling

deposition

sublimation

condensation

freezing

#73. Which of these is the mobile phase in paper chromatography?

the solvent

the paper

the ink

#74. Fractional distillation is used to separate which types of materials?

separating soluble compounds

separate soluble materials from insoluble materials

separate different types of liquids

#75. Why is there a minimum energy required for reactions to occur?

High collision energies are more likely to break chemical bonds

High energies cause spontaneous rearrangement of particles without impacts between them

#76. What is the chemical symbol for iron?

#77. What is the relative mass of an electron?

1

0 or 1/1840

2

#78. Complete the equation: H₂SO₄(aq) + ZnO(s) → …. + ….

Select all that apply:

HZnO₄ (s)

H₂O (l)

H₂SO₄ (l)

H₂SO₄ (aq)

ZnSO₄ (aq)

#79. In an experiment to measure the rate of photosynthesis of pondweed in a test tube, the number of bubbles (oxygen) produced per minute is used to determine the rate of reaction. What is this experiment actually measuring?

The concentration of the products of the reaction

The mass of the reactants of the reaction

The mass of the products of the reaction

The volume of the reactants of the reaction

The volume of the products of the reaction

#80. What is the chemical symbol for chlorine?

#81. Calculate the relative formula mass of carbon monoxide (CO) to 2 decimal places. Carbon Aᵣ = 12, Oxygen Aᵣ = 16.

#82. What is the approximate radius of an atom?

1 x 10⁻¹⁵

1 x 10⁻³

1 x 10⁻¹⁰

1 x 10⁻³

#83. Which of the following are strong acids?

Select all that apply:

ethanoic acid

carbonic acid

boric acid

hydrochloric acid

sulfuric acid

nitric acid

#84. How many sulfur atoms will react with two lithium atoms to form an ionic compound?

1

3

2

#85. Do non-metals usually have a high or low melting point?

Low

High

#86. Complete the equation: NaOH(aq) → Na⁺(aq) + ….

HO⁻(aq)

OH⁻(aq)

NO⁻(aq)

#87. Covalent compounds typically form between which two types of material?

non-metal and non-metal

metal and metal

metal and non-metal

#88. Complete the equation: H⁺(aq) + OH⁻(aq) → ….

2H₂O(l)

OH₂(aq)

CO₂(g)

H₂O(l)

Remember:

acids produce an excess of hydrogen ions

alkalis produce an excess of hydroxide ions

hydrogen ions and hydroxide ions come together to make water which is neutral.

#89. Do metals usually have a high or low melting point?

Low

High

GCSE OCR Chemistry B Paper 1

Good Luck!

Results

#1. Complete the following half equation for a reaction the cathode during electrolysis of molten zinc chloride. Zn²⁺ + ….. → Zn

#2. What is the chemical symbol for mercury?

#3. Ernest Rutherford fired positive particles at a thin gold foil and showed that most of atoms is empty space. Which particles did he fire at the gold foil?

#4. Why does the temperature of a material stay constant during the transition from liquid to gas?

#5. What state of matter has particles which are far apart and move around independently?

#6. What is the symbol for relative atomic mass?

#7. What evidence supports the notion that human activities are contributing to climate change?

#8. Are non-metals usually malleable or brittle?

#9. Iron is turned into iron oxide when exposed to the air. This is a process also known as rusting. Is the rate of reaction fast or slow in rusting?

#10. Which description best describes mixtures?

#11. Can Rf values be higher than 1?

#12. Solutions of more than pH 7 are?

#13. True or false – You cannot use physical processes to separate mixtures into different substances.

#14. Temperature affects the rate of reaction. Which of the following is the correct description of what happens when temperature changes?

#15. Paper chromatography is used to separate which types of materials?

#16. What is the formula for potassium hydroxide?

#17. Calculate the relative formula mass of copper oxide (CuO) to 2 decimal places. Copper Aᵣ = 63.5, Oxygen Aᵣ = 16.

#18. What is the charge of a proton?

#19. Which of the following is the chemical test for oxygen?

#20. What is the chemical symbol for sodium?

#21. Why is graphite softer than diamond?

#22. Which type of reaction is photosynthesis?

#23. What is the current composition of the Earth’s atmosphere?

#24. Which of the following are properties of ionic compounds?

#25. What is the name of the force that holds together ions in ionic compounds?

#26. Complete the following equation: MgO (s) + H₂SO₄ (aq) → …. + ….

#27. In aqueous solutions such as sodium chloride solution, there will be negatively charged ions from the salt (Cl⁻) as well as hydroxide ions (OH⁻). What is the rule that determines which will be discharged at the anode.

#28. Fill in the gap. Metal atoms bond forming a giant ……… of ions.

#29. Why is magnesium a better electrical conductor than sodium?

#30. Will endothermic reactions continue if there is no energy input?

#31. During a neutralisation reaction which salt is formed from sulfuric acid?

#32. Increasing the concentration of solutions increases the rate of reaction, why is this the case?

#33. Oxygen is in group 6 and fluorine is in group 7. How many fluorine atoms bond with one oxygen atom?

#34. Where is most of the mass of an atom?

#35. What method can we use to separate multiple types of liquids?

#36. When using inert electrodes to perform electrolysis with sodium sulfate solution, which products will be produced at the anode and cathode?

#37. What is the chemical symbol for oxygen?

#38. Can compounds be pure, for example, carbon dioxide?

#39. During Ernest Rutherford’s experiments with gold foil, why did some of the particles bounce back?

#40. Do metals usually have a high or low density?

#41. Which of the following descriptions matches the Mᵣ of a compound?

#42. Which of the following descriptions matches the Aᵣ of an element?

#43. Which description most accurately describes covalent bonding

#44. What is the chemical symbol for carbon?

#45. Which of the following are the main sources of drinking water in the UK?

#46. Isotopes of atoms have different numbers of which particles?

#47. What is the formula for the polyatomic ion nitrate?

#48. What do we use fullerenes for?

#49. What is a simple molecular structure?

#50. During electrolysis which electrode do anions and cations migrate to?

#51. The table shows 3 substances and their melting points. What common substance, in particular, could substance Z be?

#52. When using inert electrodes to perform electrolysis with molten lead bromide, which products will be produced at the anode and cathode?

#53. How could we accurately monitor the rate of a reaction? ? Three answers

#54. What is the name of the phase change from gas to solid?

#55. What is the name of the apparatus used for distillation?

#56. Greenhouse effect 1) Fill in the blanks: Energy from the sun in the form of …….. hits the Earth’s surface and ……. are emitted back towards the atmosphere.

#57. What are negative ions called?

#58. Which type of reaction takes in energy, making the surroundings cooler?

#59. Lead has 4 stable isotopes. ²⁰⁴Pb (abundance – 1.4%), ²⁰⁵Pb (abundance – 24.1%), ²⁰⁷Pb (abundance – 22.1%) and ²⁰⁸Pb (abundance – 52.4%). Calculate the Aᵣ of lead. Answer to 2 decimal places.

#60. Copper can be purified using electrolysis of copper sulfate solution. For this process we use the setup in the image below. Complete the half equation for the reaction at the anode. Cu → ….. + …..

#61. What is the mass number of an element?

#62. What is the charge of an electron?

#63. What is the chemical symbol for phosphorus?

#64. Energy is transferred between the environment and reactants during a chemical reaction. What form is this energy usually in?

#65. Is water an example of a covalent compound?

#66. What is the formula for the compound calcium nitrate which is made of calcium and nitrate ions (NO₃⁻)?

#67. Which types of atoms can be found in a pure piece of gold?

#68. Which of the following was the Rutherford Model of atomic structure?

#69. During a neutralisation reaction which salt is formed from nitric acid?

#70. Which of these is a problem with metallic models?

#71. In aqueous solutions such as sodium chloride solution, there will be positively charged ions from the salt (Na⁺) as well as hydrogen ions (H⁺). What is the rule that determines which will be discharged at the cathode.

#72. What is the name of the phase change from liquid to gas?

#73. Which of these is the mobile phase in paper chromatography?

#74. Fractional distillation is used to separate which types of materials?

#75. Why is there a minimum energy required for reactions to occur?

#76. What is the chemical symbol for iron?

#77. What is the relative mass of an electron?