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Chemistry. Flashcards

1
Q

Matter is anything that….

A

Has mass and takes shape.

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2
Q

Pure substances include:

A

Elements and compounds.

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3
Q

Elements are…

A

Pure substances made up of one type of atom.

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4
Q

Compounds are…

A

Pure substances made up of two or more types of atoms bonded together.

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5
Q

Ionic compounds are formed between…

A

A cation (metal, + charge) and an anion (non-metal, - charge).

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6
Q

Mixtures are…

A

Impure substances that can be physically separated, like salt and water or air.

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7
Q

A covalent bond can be defined as…

A

A bond in which two atoms share one or more pairs of electrons.

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8
Q

An ion is…

A

A charged atom.

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9
Q

An ionic bond is…

A

A bond in which the transfer of electrons occurs between a metal and a non metal (or cation and anion).

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10
Q

A lattice is…

A

An interlaced structure pattern.

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11
Q

A metallic bond is…

A

A bond in which free electrons move around metal ions.

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12
Q

A molecule is…

A

The smallest unit of a covalent compound that can take part in a chemical reaction.

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13
Q

Valency is…

A

An element’s power to combine with other atoms.

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14
Q

Describe a covalent bond.

A
  • made of 2 or more non-metals.
  • don’t conduct electricity.
  • gases or liquids at room temperature often occur as covalent bonds.
  • they have the lowest melting point.
  • they are the weakest bond.
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15
Q

Describe an ionic bond.

A
  • Transfer of electrons occurs between metals, which lose electrons (they are called cations) and non-metals, which gain them (called anions).
  • occur due to the electrostatic attraction of the opposite charges (metals are positively charged and non-metals are negatively charged).
  • This is a strong bond.
  • They are solid at room temperature.
  • They conduct electricity only when molten.
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16
Q

Describe metallic bonds.

A
  • occur in only metal elements.
  • sea of delocalised electrons.
  • malleable.
  • strong bond.
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17
Q

Describe lattices, or a covalent network.

A
  • 3D structured lattice.
  • non-metals sharing electrons.
  • highest melting point.
  • example is diamond (carbon lattice).
  • Extremely lustrous.
  • High refraction index.
  • STRONGEST bond.
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18
Q

Naming covalent bonds (see info).

A
  1. 1st element furthest to the left is written in full.
  2. 2nd element furthest to the right ends in ide.
  3. Prefix for 1st element.
  4. Prefix for second element.
  5. If in the same group, element furthest down is named first (e.g. sulfuroxide).
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19
Q

Chemical formula for ammonium is…

A

NH4 +

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20
Q

Chemical formula for carbonate is…

A

CO3 -2

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21
Q

Chemical formula for hydroxide is…

A

OH -

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22
Q

Chemical formula for nitrate is…

A

NO3 -

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23
Q

Chemical formula for nitrite is…

A

NO2 -

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24
Q

Chemical formula for phosphate is…

A

PO4 3-

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25
Q

Chemical formula for sulfate is…

A

SO4 2-

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26
Q

Chemical formula for hydrogen sulfate is…

A

HSO4 -

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27
Q

Chemical formula for sulfate is…

A

SO3 2-

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28
Q

Formula for ammonia is…

A

NH3 (no charge)

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29
Q

Chemical formula for carbon dioxide is…

A

CO2 (no charge)

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30
Q

Formula for chlorine is….

A

Cl2 aq

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31
Q

Formula for glucose is…

A

C6H12O6 aq

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32
Q

Formula for hydrogen is…

A

H2 aq

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33
Q

Formula for ozone is…

A

O3 aq

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34
Q

Formula for water is…

A

H2O aq

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35
Q

Formula for hydrochloric acid is…

A

HCl aq

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36
Q

formula for nitrous acid is…

A

HNO2 aq

37
Q

nitric acid formula…

A

HNO3 aq

38
Q

formula for sulfurous acid…

A

H2SO3 aq

39
Q

Formula for sulfuric acid

A

H2PO4aq

40
Q

Formula for phosphoric acid

A

H3PO4 aq

41
Q

Carbonic acid

A

H2CO3aq OR CO2 (aq)

42
Q

Ethanol acid/acetic acid charge

A

CH3COOH OR HC2H3O2

aq

43
Q

Formula for neutralisation reactions is…

A

Acid + base —> salt + water.

44
Q

Acid metal reaction formula

A

Acid + Metal = salt + hydrogen gas (H2).

45
Q

Acid carbonate reaction

A

Acid + Carbonate —> salt + carbon dioxide (CO2) + water (H2O).

46
Q

combustion reaction

A

hydrocarbon + oxygen —> carbon dioxide + water

(or carbon monoxide and carbon soot)

Or metal + oxygen —> metal oxide

Energy is also released in both cases

47
Q

Formula for corrosion.

A

4Fe + 3O2 —> 2Fe2O3

48
Q

Galvanising is….

A

Coating iron with a layer of zinc. Zinc sacrifices itself by corroding in place of the iron, providing a protective barrier through a process called sacrificial protection.

49
Q

Electroplating is

A

Coating the metal with another metal through an electrochemical process. This adds a layer of a more corrosion-resistant metal on the surface, improving protection.

50
Q

You can prevent corrosion by:

A

Attaching a metal to a more reactive metal: By attaching a less reactive metal to a more reactive one, the less reactive metal serves as a sacrificial anode, corroding instead of the more valuable metal it’s protecting.

Forming an alloy: Mixing two or more metals to create a new material with improved corrosion resistance. The combination of metals in an alloy can make it more resistant to corrosion than the individual components.

Painting the metal: Applying a protective paint layer on the metal surface acts as a barrier, preventing exposure to moisture and oxygen, which are the main causes of corrosion.

Galvanizing: Coating iron with a layer of zinc. Zinc sacrifices itself by corroding in place of the iron, providing a protective barrier through a process called sacrificial protection.

Electroplating: Coating the metal with another metal through an electrochemical process. This adds a layer of a more corrosion-resistant metal on the surface, improving protection.

51
Q

Describe thermal decomposition.

A
  • Started by heat energy.
  • Easy reaction to be seen if reactive metal is burnt over a Bunsen Burner.
  • Decomposes into carbon dioxide.
  • Lime water test can be used.

Example: heating copper carbonate, decomposes into copper oxide and carbon dioxide gas.

52
Q

Describe electrical decomposition.

A
  • Preformed by passing on an electrical current through a liquid reactant.
  • Decomposes into hydrogen.
  • Pop test can be used.

Example: applying electricity to water, decomposes into hydrogen and oxygen.

53
Q

Describe photochemical decomposition.

A
  • Triggered by light energy.
  • Slow reaction.

Example: silver chloride is exposed to light, and slowly decomposes into silver and chlorine ions.

54
Q

Aerobic respiration occurs…

A

when there is plenty of oxygen present. Glucose (from food) reacts with oxygen to produce carbon dioxide, water and energy.

55
Q

Anaerobic respiration occurs…

A

When there is little to no oxygen present. During vigorous exercise, the heart and lungs can’t keep up with the demand of oxygen (aerobic respiration) to your muscles. So the muscles carry out anaerobic respiration, producing lactic acid, which can cause cramps.

56
Q

The energy produced from respiration is stored in a chemical called ATP (adenosine triphosphate). This energy is used for:

A
  • Growth and repair of cells
  • Keeping body temperature constant
  • Sending messages along nerves.
  • Muscular action.
57
Q

What is the function of carbohydrases (enzymes)?

A

They break down carbhydrates.

For example, amylase (in the mouth) beaks down carbohydrates into maltose, which is broke down into glucose in the small intestine.

58
Q

What is the function of proteases (enzymes)?

A

Break down protein molecules.

In the stomach, pepsin breaks down proteins into peptides and some amino acids.

59
Q

What is the function of lipases?

A

Break down lipid (fate) molecules.

In the small intestine, lipase breaks down complex fat molecules into fatty acids and glycerol molecules.

60
Q

What’s photosynthesis and what is the formula of photosynthesis?

A

Photosynthesis is a process which occurs in plants leaves or in chloroplast. It involves two reactions – with & without light.

6CO2 + 6H2O —> C6H12O6 + 6CO2

It is a chemical reaction in living things as a it supplies glucose to organisms.

61
Q

What is sponteneous combustion and when does spontaneous combustion happen?

A

It is when when a substance bursts into flames without external energy being applied.

  • Happens when the internal temperature of the substance increases because of the other chemical reactions.
  • Once the temperature reaches a point at which the substance would catch fire, it can trigger combustion.

Example: coal mines bursting into fire randomly.

62
Q

What is rapid combustion

A

a process in which a large amount of heat and light is released in a very short span of time.

Example: fireworks.

63
Q

What do acids produce when mixed with water, and how is their strength measured?

A

Acids produce hydrogen ions (H+) when mixed with water. The strength of an acid is measured by its pH level, with lower pH values indicating stronger acids.

64
Q

Provide an example of a common acid and its pH level.

A

Lemon juice is a common acid with a pH of 4, while stomach acid has a pH of 2, making it stronger than lemon juice.

65
Q

Name two weak acids and give examples of where they can be found.

A

Two weak acids are citric acid (found in oranges and lemons) and acetic acid (found in vinegar).

66
Q

What are some properties of acids?

A

Properties of acids include the production of hydrogen ions, a pH of less than 7, a sour taste, corrosiveness, and the ability to turn blue litmus paper red.

67
Q

What do bases release in a solution, and how is their pH typically compared to acids?

A

Bases release hydroxide ions (OH-) in a solution. Their pH is typically higher than 7, which is higher than that of acids.

68
Q

Name some properties of bases.

A

Properties of bases include the production of hydroxide ions, a pH greater than 7, a bitter taste, caustic nature, the ability to turn red litmus paper blue, and the ability to conduct electricity.

69
Q

What are the three types of bases based on their chemical composition?

A

The three types of bases are metal hydroxides, metal oxides, and metal carbonates.

70
Q

What is the pH scale, and what does it measure?

A

The pH scale is a range from 0 to 14 that measures the acidity of a solution. (potenial of hydrogen)

71
Q

What does a pH value less than 7 indicate on the pH scale? What about a pH value of 7? And greater than 7?

A

On the pH scale, a pH less than 7 indicates an acidic solution, a pH of 7 is considered neutral, and a pH greater than 7 indicates a basic (or alkaline) solution.

72
Q

How can pH be measured, and provide examples of measurement methods.

A

pH can be measured using indicators, which provide color changes, such as the green color for water with universal indicator, or by using a pH probe, a digital device for accurate measurement, which is considered non-destructive testing.

73
Q

Acids turn blue litmus paper red and bases…

A

turn red litmus paper blue!

74
Q

What is the purpose of carbon capture, and how does it work?

A

Carbon capture is aimed at reducing carbon dioxide emissions. It involves compressing CO2 into a liquid form, which can be stored underground.

75
Q

Name some disadvantages of carbon capture.

A

Disadvantages of carbon capture include it being an expensive process, consuming a lot of energy, and the risk of CO2 leakage from storage sites.

76
Q

What are some alternative methods to carbon capture?

A

Alternative methods include converting gaseous CO2 into solid carbon particles and using materials like Ferrock, which contains steel dust and silica and consumes CO2 instead of producing it.

77
Q

What factors influence decisions about scientific research?

A

Social considerations, ethical considerations, and environmental considerations influence decisions about scientific research.

78
Q

Provide examples of social considerations in scientific research.

A

Social considerations involve thinking about the impact on society and how people or organizations might behave as a result of the research.

79
Q

What is the role of ethical considerations in scientific research?

A

Ethical considerations address the moral aspects of research, such as whether it is morally right to use a new material or technology.

80
Q

In what way do environmental considerations influence scientific research?

A

Environmental considerations focus on the potential impact of new technologies on the environment and whether they might make environmental conditions better or worse.

81
Q

What is the role of a biochemist in the field of chemistry?

A

A biochemist is a scientist who studies the chemical processes in living organisms, with a focus on understanding the chemistry of biological items like medicines, cosmetics, and food.

82
Q

What is industrial chemistry, and how is it related to biochemistry?

A

Industrial chemistry involves using chemical processes on an industrial scale, often in producing materials. Biochemistry is related because it involves the industrial-scale production and development of biological items.

83
Q

Where do chemists work, and what are some of their tasks?

A

Chemists work in a variety of industries, including pharmaceuticals, forensics, chemical plants, and laboratories. Their tasks may involve discovering new medicines, analyzing criminal cases forensically, or producing building materials and paints.

84
Q

What are the primary responsibilities of chemical engineers?

A

Chemical engineers focus on solving problems related to chemical processes. They are involved in the design, development, and manufacture of chemical products and materials and work in various industries such as oil and gas, energy, water treatment, and food and drink.

85
Q

What do biochemists study, and in which industries do they typically work?

A

Biochemists study chemical processes in living organisms to understand reactions in tissues and the effects of medicines. They often work in pharmaceutical and biotechnology industries, food technology, toxicology, and vaccine production.

86
Q

What is the process of carbon capture?

A

Here’s how carbon capture works:

Capture: This is the first step. Carbon capture technology captures CO2 emissions produced from the use of fossil fuels in electricity generation and industrial processes before it is released into the atmosphere. There are several methods for capturing CO2:

Post-combustion capture: This method involves capturing CO2 after a fuel, like coal or natural gas, has been burned to generate power or heat.

Pre-combustion capture: This captures CO2 before the fuel is burned. It’s often used in integrated gasification combined cycle (IGCC) power plants.

Oxy-fuel combustion: In this process, fuel is burned in pure oxygen instead of air, which produces a concentrated CO2 stream that can be captured more easily.

Transport: After capture, the CO2 needs to be transported to a suitable storage location. This is typically done via pipelines, ships, or other means of transportation.

Storage: The captured CO2 is then injected into deep geological formations such as depleted oil and gas reservoirs, saline formations, or unmineable coal seams. These underground locations are chosen for their stability and impermeable rock layers that prevent the CO2 from leaking back into the atmosphere.

87
Q

What is the aim of carbon capture?

A

The aim of carbon capture is to prevent large amounts of CO2 from being released into the atmosphere, where it contributes to climate change. It’s particularly important for industries and power plants that are challenging to decarbonize completely through other means.

88
Q

What are the challenges associated with carbon capture?

A

Carbon capture is considered one of the technologies that can help in the transition to a low-carbon or net-zero emissions future. However, it’s worth noting that there are challenges associated with carbon capture, including the high cost of implementation, the energy required to run the capture process, and ensuring the long-term integrity of the storage sites. As of my last knowledge update in January 2022, research and development in this field are ongoing to improve the efficiency and cost-effectiveness of carbon capture technologies.

89
Q
A

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