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POA > chem > Flashcards

chem Flashcards

1
Q

Lithium

A

Li⁺

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2
Q

Sodium

A

Na⁺

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3
Q

Potassium

A

K⁺

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4
Q

Calcium

A

Ca²⁺

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5
Q

Magnesium

A

Mg²⁺

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6
Q

Aluminium

A

Al³⁺

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7
Q

Gallium

A

Ga³⁺

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8
Q

Copper (II)

A

Cu²⁺

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9
Q

Iron (II)

A

Fe²⁺

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10
Q

Iron (III)

A

Fe³⁺

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11
Q

Lead (II)

A

Pb²⁺

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12
Q

Lead (IV)

A

Pb⁴⁺

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13
Q

Zinc

A

Zn²⁺

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14
Q

Silver

A

Ag⁺

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15
Q

Ammonium

A

NH₄⁺

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16
Q

Fluoride

A

F⁻

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17
Q

Chloride

A

Cl⁻

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18
Q

Bromide

A

Br⁻

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19
Q

Oxide

A

O²⁻

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20
Q

Sulfide

A

S²⁻

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21
Q

Hydroxide

A

OH⁻

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22
Q

Nitrate

A

NO₃⁻

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23
Q

Carbonate

A

CO₃²⁻

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24
Q

Sulfate

A

SO₄²⁻

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25
Q

Phosphate

A

PO₄³⁻

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26
Q

Manganate (VII)

A

MnO₄⁻

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27
Q

Hydrochloric Acid

A

HCL

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28
Q

Nitric Acid

A

HNO₃

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29
Q

Sulfuric Acid

A

H₂SO₄

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30
Q

Ethanoic Acid

A

CH₃COOH

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31
Q

What does acid produce when dissolved in water?

A

H⁺ ions

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32
Q

Acids what a what kind of taste

A

Sour

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33
Q

Acids turn what colour litmus paper to what colour

A

Blue to Red

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34
Q

When acid dissolved in water, can it conduct electricity.

A

Yes

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35
Q

What are strong acids

A

Acids when dissolved in water are fully ionised to produce a solution with high concentration of H⁺ ions

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36
Q

What are weak acids

A

Acids when dissolved in water are partially ionised to produce a solution with a low concentration of H⁺ ions

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37
Q

Metal + Acids =

A

Salt + Hydrogen gas

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38
Q

Carbonates + Acids =

A

Salt + Carbon dioxide gas + Water

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39
Q

Base + Acids =

A

Salt + Water

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40
Q

Test for Hydrogen gas

A

Insert a lighted splint into the gas, and the lighted splint extinguishes with a ‘pop’ sound

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41
Q

Test for Carbon dioxide

A

Bubble the gas into limewater and white precipitate will form in the limewater.

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42
Q

Another name for acid + base reaction

A

Neutralisation

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43
Q

Use of hydrochloric acid

A

Removes impurities such as rust and limescale from metals and aluminium alloys

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44
Q

Phosphoric acid

A

H₃PO₄

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45
Q

Use for phosphoric acid

A

Added to food to give a sour taste

46
Q

What is the use of Ethanoic acid

A

Acts as food preservative and flavour enhancer

47
Q

Types of bases

A

Metal oxides and metal hydroxides

48
Q

What does alkali produce when dissolved in water

A

OH⁻

49
Q

Texture of alkali

A

Soapy

50
Q

Taste of alkali

A

Bitter

51
Q

Alkalis turn what litmus paper into what colour?

A

red to blue

52
Q

What is ionic equation

A

Simplify everything that can be simplified into ion and then remove the spectator ions.

53
Q

Alkali + Ammonium salt

A

Salt + water + ammonia gas

54
Q

test for ammonia gas

A

place a damp red limes paper near the gas and it will turn blue.

55
Q

use of magnesium oxide

A

it relieves gastric pain and it is used for making refractory bricks

56
Q

use of sodium hydroxide

A

used in the making of soap

57
Q

Use of calcium hydroxide

A

reduces acidity in soil

58
Q

Use of ammonia

A

used in making fertilisers

59
Q

ph value is determined by what

A

amount of OH⁻ present in the substance. The more, the higher the ph level, the more alkaline it is.

60
Q

Ways to measure ph

A

universal indicator, ph meter, and ph probe attached to a data logger

61
Q

litmus paper in acid

A

red

62
Q

what ph level with litmus change

A

5-8

63
Q

litmus paper in alkaline

A

blue

64
Q

methyl orange in acid

A

red

65
Q

what ph level with litmus charge

A

3-5

66
Q

methyl orange in alkaline

A

yellow

67
Q

screened methyl orange in acid

A

purple/violet

68
Q

what ph level will screened methyl orange change

A

3-5

69
Q

screened methyl orange in alkaline

A

green

70
Q

what is liming

A

adding alkaline (calcium carbonate) to reduce the acidity in the soil

71
Q

acidic oxide is metallic or non-metallic

A

non-metallic

72
Q

acidic oxide dissolve in water turn into what

A

acid

73
Q

basic oxide is metallic or non-metallic

A

metallic

74
Q

acidic oxide at room temp what state

A

gas

75
Q

basic oxide at room temp what state

A

solid

76
Q

what are insoluble basic oxides

A

bases

77
Q

what are soluble basic oxides

A

alkalis

78
Q

acidic oxides react with what get salt and water

A

bases / alkalis

79
Q

basic oxides react with what get salt and water

A

acids

80
Q

amphoteric oxides is metallic or non-metallic

A

metallic

81
Q

when amphoteric oxides react with acids, they are what

A

bases

82
Q

when amphoteric oxides react with alkalis and bases, they are what

A

acid

83
Q

what are the three amphoteric oxides

A

zinc oxide (ZnO), aluminium oxide (Al₂O₃), and lead (II) oxide (PbO)

84
Q

neutral oxides are metallic or non-metallic

A

non-metallic

85
Q

are neutral oxides acid or base

A

no its useless

86
Q

what are the three neutral oxides

A

water (H₂O), carbon monoxide (CO), nitrogen monoxide (NO)

87
Q

what is ionic bonding

A

transfer of electrons from a metal to a non-metal. they create strong electrostatic forces of attraction between positive and negative ions in ionic compounds.

88
Q

structure of ionic compounds

A

arranged in giant ionic lattice structures.

89
Q

why ionic compounds have high melting and boiling points

A

Large amount of energy is needed to overcome the strong electrostatic forces of attraction (strong ionic bonds) between oppositely charged ions.

90
Q

why solid ionic compounds cannot conduct electricity

A

There is an absence of mobile ions in the solid state. Hence, ionic compounds are not able to conduct electricity.

91
Q

why molten and aqueous ionic compounds can conduct electricity

A

There is the presence of mobile ions in the molten and aqueous states enable ionic compounds to conduct electricity in these states.

92
Q

why is ionic compounds hard yet brittle

A

A large amount of energy is required to overcome the strong electrostatic forces of attraction between oppositely charged ions (strong ionic bonds) in the giant ionic lattice structure. Hence, ionic compounds are strong.
When a force is exerted, ions of the same charge are forced next to one another. These ions repel one another, causing the ionic lattice structure to break and be brittle.

93
Q

can ionic compounds dissolve in organic solvents

A

no

93
Q

can ionic compounds dissolve in water

A

yes

94
Q

what can covalent substance exist as

A

simple molecular structures

95
Q

why is covalent substances melting and boiling points so low

A

A small amount of energy is required to overcome the weak intermolecular forces of attraction.

96
Q

can covalent substance dissolve in water

A

no

97
Q

can covalent substance dissolve in organic solvent

A

yes

98
Q

why does covalent substance don’t conduct electricity in all states

A

There is an absence of mobile charge carriers to conduct electricity.

99
Q

what are alloys

A

mixture of metals

100
Q

what is the arrangement of a metal

A

Atoms in a metal are all of the same size.
Hence, copper atoms are regularly arranged.

101
Q

what is the arrangement of alloys

A

Atoms of the elements in an alloy are of a different size. Hence, the regular arrangement of copper atoms in pure copper metal is disrupted by the randomly distributed tin atoms in bronze. This leads to an irregular arrangement of atoms in an alloy.

102
Q

what is malleability

A

the ability of substances to be bent/ flattened into different shapes without breaking

103
Q

what is ductility

A

the ability of a substance being pulled into wires without breaking.

104
Q

what is the strength of metal

A

In a metal, the regularly arranged metal atoms are of the same size. When enough force is applied, the metal atoms can slide over one another easily. Hence, metals are malleable and ductile.

105
Q

what is the strength of alloy

A

In an alloy, the irregularly arranged atoms are of different sizes. The atoms are not able to slide over one another easily. Alloys are harder and stronger than the pure metals that they are made from.

106
Q

why metal has high fixed m/b points

A

as copper is pure

107
Q

why alloys have a range of m/b points

A

as bronze is a mixture

108
Q

why both metal and alloys are good at conducting electricity and heat

A

Both have free-moving/ delocalised valence electrons from the metal atoms that can act as charge carriers or assist in the transfer of
thermal energy.

109
Q

what is element

A

a pure substance that cannot be broken down into two or more simpler substances by chemical methods. fixed melting and boiling points

110
Q

what is compound

A

a pure substance containing two or more elements that are chemically combined in a fixed ratio. can be separated into its constituents by chemical methods (e.g., thermal decomposition, electrolysis). has different properties from its constituent elements. fixed melting and boiling points

111
Q

what is mixture

A

consists of elements and/or compounds that are physically combined in varying ratios. can be separated into its constituents by physical methods (e.g., filtration, chromatography, distillation). usually has similar properties to its constituent elements. melts and boils over a range of temperatures

POA (2 decks)

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