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Chemistry Yr 10 > Year Exam Revision > Flashcards

Year Exam Revision Flashcards

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1
Q

Define an acid

A

An acid is defined as a substance which forms hydrogen ions in a solution.

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2
Q

What are the properties of an acid

A

Acids have a pH less than 7, react with metals, bases, and carbonate salts, can be corrosive, solutions of a compound dissolved in water and conduct electricity. In addition to acids produces H+ ions when they dissociate.

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3
Q

Examples of acids

A

Hydrochloric acid, nitric acid, sulphuric acid, ethanoic acid and carbonic acid

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4
Q

Define a base

A

A base is a substance which reacts only with an acid to form salt or water only.

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5
Q

What are the properties of a base

A

Bases can be solid or aqueous, conduct electricity, have a pH above 7, soapy and slippery feel, bitter taste, corrosive and caustic.

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6
Q

What are the three types of bases

A

Ionic hydroxides (eg. NaOH, Ca(OH)₂, Mg(OH)₂), ionic oxides (eg. Na₂O, CaO, MgO) and ammonia solution (NH₃)

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7
Q

Define an alkali

A

A base that is soluble in water and produces hydroxide ions (OH-) is called an alkali.

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8
Q

How can hydroxide ions be produced

A

They can be produces by one of two methods:
* Hydroxides dissociates to produce hydroxide ions.
* Oxides and ammonia react with water to produce hydroxide ions.

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9
Q

What is the difference between acids and bases

A

The difference between acids and bases is that all acids release hydrogen ions (H⁺) in a solution, whereas soluble bases release hydroxide ions (OH⁻).

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10
Q

How does the litmus indicator work

A

When the litmus colour meets an acid it will change colour, however when it meets bases the colour will stay the same.

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11
Q

Define neutral substances

A

A neutral substance is any substance that is neither an acid nor a base. In fact, when acids and bases mix, they react to form neutral substances.

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12
Q

What are the properties of a neutral substance

A

Neutral substances are not corrosive, have no taste, dissolve in water and have a pH of 7.

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13
Q

Why are acids an alkalis conductive

A

Both are soluble bases that undergo dissociation when added to water, which means that individual ions are free to move through the solution.

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14
Q

How is a solution concentrated

A

Concentrated solutions have a large mass of solute dissolved in a given volume of water.

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15
Q

How is a solution dilute

A

Dilute solutions have only a small mass of solute dissolved in a given volume of water.

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16
Q

Define concentration

A

Concentration is defined as the amount of solute which is dissolved in a given quantity of solvent.

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17
Q

Define a solvent

A

The medium which dissolves in the solute is known as the solvent.

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18
Q

Define a solute

A

Dissolved particles in a solution are known as the solute.

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19
Q

Define a solution

A

The result of the solute dissolving is known as a solution.

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20
Q

What is the formula for concentration

A

C= n/V

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21
Q

What are two ways to increase the concentration of a solution

A

There are two ways of increasing the concentration of a solution:
* Increase the amount of solute.
* Decrease the amount of solvent.

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22
Q

What are two ways to decrease the concentration of a solution

A

There are two ways to decrease the concentration of a solution:
* Decrease the amount of solute.
* Increase the amount of solvent.

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23
Q

What is saturation

A

At a certain point when adding solute to a solvent, no more solute will dissolve into the solvent, and it will remain as a sediment in the beaker. At this point, the concentration of solution remains constant. When a solution reaches this point, we call it saturated. Before this it is unsaturated.

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24
Q

What are the three types of saturated solutions

A
  • Saturated solution
  • Unsaturated solution
  • Supersaturated solution
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25
Q

What is a saturated solution

A

a solution containing the maximum amount if solute for a given amount of solvent at a given temperature and pressure.

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26
Q

What is an unsaturated solution

A

a solution that contains less solute than a saturated solution at a given temperature and pressure.

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27
Q

What is a supersaturated solution

A

a solution that contains more solute than it can theoretically hold at a given temperature; excess solute precipitates if the solution is disturbed.

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28
Q

What happens when strong acids and alkalis are dissolved in water

A

all of the molecules separate into ions.

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29
Q

What happens when weak acids and alkalis are dissolved in water

A

only partially ionise, and many molecules do not dissociate.

30
Q

Name the general reactions

A

ACID + BASE → SALT + WATER
ACID + CARBONATE → SALT + WATER + CARBON DIOXIDE
ACID + METAL → SALT + HYDROGEN

30
Q

What is ocean acidification

A

As carbon dioxide gas dissolves in sea water, it forms carbonic acid (H2CO3), a weak acid that dissociates into bicarbonate (HCO3-) and hydrogen ions (H+). Increased hydrogen ions mean an increase in the acidity of the ocean would occur.

30
Q

Impact of the ocean becoming more acidic

A

Dissolved CO2 molecules combine with water to form carbonic acid, which in turn combines with carbonate to form hydrogen carbonate. When the carbon dioxide in the atmosphere increases, carbonate in the ocean decreases and its harder to form shells,

30
Q

What are alkenes

A

are the most basic organic molecules and often referred to as hydrocarbons. Only contains carbon and hydrogen atoms and are single bonded. Suffix of “-ane”

30
Q

What is an isomer

A

an organic molecule with the same molecular formula but a different structured formula is called an “isomer”.

30
Q

What are alkenes

A

only contain hydrogen and carbon atoms and are double bonded. Suffix of “-ene”

30
Q

What are alkynes

A

only contains carbon and hydrogen and contain a triple bond. Suffix of “-yne”

31
Q

What are alcohols

A

contains hydrogen, carbon, and oxygen atoms. contains hydroxyl (-OH) functional group. All single bonds and has the suffix of “-ol”

32
Q

What are aldehydes

A

contain carbon, hydrogen, and oxygen. contains carbonyl functional group at the end of a carbon chain which is a oxygen double bonded to a carbon. Suffix of “-al”.

33
Q

What are ketones

A

contains carbon, hydrogen, and oxygen atoms. Functional group is when a carbon has a double bond to an oxygen and that carbon is bonded to two other carbons.

34
Q

What are carboxylic acids

A

contains carbon, hydrogen, and oxygen atoms. The functional group attached to one of the carbons has to be doubled bonded to an oxygen and an OH group attached to that same carbon.

35
Q

What are cis and trans isomers

A

Cis and trans isomers are types of geometric isomers, where the functional group is placed differently with regards to the double bond. In general, a cis isomer has molecules on one side of the double bond. A trans isomer has molecules on the other side of the double bond.

36
Q

What are cis isomers

A

A cis isomer has molecules on one side of the double bond. A trans isomer has molecules on the other side of the double bond.

37
Q

What are trans isomers

A

A trans isomer has molecules on the other side of the double bond.

38
Q

Define an atom

A

the smallest particles of an element that retains its identity during a chemical reaction.

39
Q

Define a molecule

A

a neutral group of non-metals covalently bonded (together by chemical bonds)

40
Q

Define an element

A

a substance that is made up of one type of atom, defined by it’s atomic number.

41
Q

Define a compound

A

a substance that is made up of atoms of different elements joined together by chemical bonds in a fixed ratio.

42
Q

Define mass number

A

the total number of protons and neutrons of an atom.

43
Q

Define an ion

A

an atom or molecule that had gained or lost one or more electrons.

43
Q

Define atomic number

A

the number the protons in the nucleus of an atom of an element.

44
Q

Define a polyatomic ion

A

a tightly bonded group of atoms that behave as a unit and has a positive or negative charge.

45
Q

What is a proton

A

A large subatomic particle with a positive charge located in the nucleus .

46
Q

What is an electron

A

a very small subatomic particle with a negative charge located in the electron cloud.

47
Q

What is the nucleus

A

the central part of an atom with an overall positive charge.

48
Q

What is a neutron

A

a large subatomic particle with no charge located in the nucleus.

49
Q

What is an energy level

A

the outermost part of ab stop that determines the chemical properties of an element.

50
Q

electron configuration

A

the arrangement of electron in the energy levels/shells around the atoms nucleus.

51
Q

what are valence electrons

A

an electron on the outermost occupied energy level of an atom.

52
Q

What is a metal

A

a shiny, malleable element that conducts heat or electricity.

52
Q

What is a non-metal

A

a dull, brittle element that does not conduct heat or electricity.

53
Q

What different ways the periodic is arranged

A
  • metal and nonmetals
  • in order of increasing atomic number
  • as the periods increases so do the number of energy levels in the electron configuration
54
Q

Define ionic bonds

A

ionic bonds are formed by one metal and one non-metal transferring atoms to become stable. It has a lattice structure

55
Q

Define covalent bonds

A

covalent bonds are formed by two non-metals, as they share electrons to become stable. have a discrete structure.

55
Q

Define metallic bonds

A

metallic bonds are formed by two metals in a sea of electrons. Also has a lattice structure.

56
Q

Recall the rules to follow in writing formulas

A

ionic - metal first and add -ide
covalent - prefixes (if needed) than add -ide
metallic - add -ide

57
Q

What are the properties of an ionic substance

A

ionic substances are made up of ions that form charges particles when an atom gains or losses electrons.

58
Q

What are the properties of a covalent substance

A

covalent substances is a molecule formed by covalent bonds in which the atoms share one or more pairs of valence electrons.

59
Q

Define precipitate

A

an insoluble solid formed when tie soluble ionic substances react

60
Q

How is a net ionic equation different to a neutral species equation

A

a neutral species equation contains all products and reactants in a balanced equation and a net ionic equation only contains the ions that react.

61
Q

Recall how to use the activity series to determine if a reaction will take place

A

the reactivity series of metals ranks the metals from most reactive (top) to least reactive (bottom). When a solid metal is added to an ionic solution, if the metal is higher on the reactivity series it will “replace” the metal ion in the solution.

Chemistry Yr 10 (1 decks)

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