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Year 10 Science > Chem year 10 for exam > Flashcards

Chem year 10 for exam Flashcards

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1
Q

Periods

A

Across: number of electron shells

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2
Q

Groups

A

Down: number of valence electrons

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3
Q

Isotopes

A

Atoms of the same element, different number of neutrons in the nucleus

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4
Q

Group 1 elements

A

Alkali metals

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5
Q

Group 2 elements

A

Alkali earth metals

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6
Q

Group 17 elements

A

Halogens

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7
Q

Group 18 elements

A

Noble gases

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8
Q

Mass number

A

Number of protons and neutrons

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9
Q

Atomic number

A

Number of protons

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10
Q

Characteristics of metals

A

-Solid at room temperature
-Polished to produce a high shine/lustre
-Good conductors of electricity
-Malleable
-Can be made into a wire; ductile
-Usually melt at high temperatures (mercury is the exception)

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11
Q

Characteristics of non-metals

A

-Cannot be polished to produce a shine
-Brittle; shatter when hit
-Cannot be bent into shape; not malleable
-Usually, poor conductors of electricity and heat
-Usually melt at low temperatures
-Many are gases at room temperatures

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12
Q

The number of electrons per shell

A

2n^2

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13
Q

Flame test: ground state

A

Lowest energy state of an atom

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14
Q

Flame test: excited state

A

Highest energy state of an atom

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15
Q

Positively charged ions

A

Cations

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16
Q

Negatively charged ions

A

Anions

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17
Q

Electrostatic attraction

A

The attraction between two oppositely charged bodies

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18
Q

Covalent bond

A

A shared pair of electrons holding two atoms together

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19
Q

Activity series

A

Place elements in decreasing order of reactivity

20
Q

Aqueous solution

A

Solution in which water is the solvent

21
Q

Precipitate

A

Solid product of a chemical reaction that is insoluble in water

22
Q

Relative atomic mass

A

A number that compares the mass of atoms to an agreed mass of carbon-12 isotope

23
Q

Characteristics of alkali metals

A

All react strongly with water to form basic (alkaline) solutions, very reactive metals

24
Q

Characteristics of alkali earth metals

A

Reactive metals

25
Q

Characteristics of halogens

A

Brightly coloured elements, non-metals

26
Q

Characteristics of noble gases

A

Inert, meaning they do not readily react with other substances, because they have a full valence shell

27
Q

Characteristics of transition metal block

A

Block of metallic elements in the middle of the periodic table

28
Q

Redox reactions

A

Chemical reactions involving oxidation and reduction; that is, electron transfer

29
Q

OIL

A

Oxidation is Loss

30
Q

RIG

A

Reduction is Gain

31
Q

XY –> X + Y

A

Decomposition

32
Q

X + Y –> XY

A

Combination

33
Q

Acid + Base –> Salt + Water

A

Neutralisation

34
Q

Methane + Oxygen –> Carbon Dioxide + Water

A

Combustion

35
Q

Aqueous + Aqueous –> Solid + Aqueous

A

Precipitation (Double displacement)

36
Q

A + BC –> AC + B

A

Single Displacement

37
Q

Law of conservation of mass

A

Mass is neither created nor destroyed

38
Q

Atomic radius =

A

Decrease left to right (have a bigger charge)
Increase top to bottom (More valence shells)

39
Q

Isotope (nuclide) notation

A

Mass number Element
Atomic Number Element

40
Q

Ion means

A

With full valence shell when written is eg. Na+

41
Q

Valency

A

The valency is the number of electrons that each atom needs to gain, lose or share to fill its outer shell (for example, the valency of both chlorine and sodium is 1, whereas the valency of carbon is 4).

42
Q

Electrovalency

A

The electrovalency of an element is equal to the charge on the ion (for example, the electrovalency for chlorine is –1 and sodium is +1).

43
Q

Electrovalency is associated with

A

Ionic

44
Q

Valency is associated with

A

Covalent

45
Q

Is valency or electrovalency affected by charge

A

Electrovalency

Year 10 Science (3 decks)

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