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grade 9 chemistry > finals 1 > Flashcards

finals 1 Flashcards

1
Q

what happens if you mix a metal with one or more elements

A

you can change its properties

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2
Q

alloy:

A

mixture of metal with other elements

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3
Q

how are the properties of metals improved

A

mixing

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4
Q

what are the most chemical reactions of metals

A

with oxygen water and acids

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5
Q

difference between a physical and chemical property

A

physical: deals with the appearance and aspects of metal
chemical: deals with the reaction and rate of reaction

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6
Q

elaborate on the reaction of metal and oxygen

A

metals react with oxygen. the shiny surface of the metal becomes dull and this is caused by the slow chemical reaction between the metal surface and oxygen. there is one product: a surface coating of the metal oxide

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7
Q

activation energy

A

necessary energy for starting a reaction

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8
Q

e.g of activation energy

A

heating

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9
Q

what is magnesium used for

A

flash bulbs and distress flares

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10
Q

what are gold and platinum ideal for

A

making jewelry because they dont react with oxygen so they stay shiny

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11
Q

what are the products of potassium sodium or calcium with cold water

A

metal hydroxide and hydrogen gas

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12
Q

what does heating do to a reaction

A

increases the rate of the reaction

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13
Q

why are potassium and sodium stored under oil

A

they are so reactive and this prevents them from coming in contact with water and oxygen so they stay longer

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14
Q

why is copper a good choice of metal for hot water pipes

A

it doesnt react with boiling water and is cheaper

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15
Q

reactivity series

A

the list of metals in order of how quickly they react

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16
Q

what can the reactivity series be used for

A

to make predictions about other reactions of metals

17
Q

e.g of chemical reaction

A

iron nail is placed in a solution of copper sulphate

18
Q

displacement reaction

A

when a higher reactive metal eliminates the other metal in a combination

19
Q

when does a displacement reaction occur

A

when the metal being added is more reactive than the metal in the salt solution

20
Q

thermit reaction

A

a reaction that’s very fast and gives out alot of heat

21
Q

decomposition reaction

A

a reaction in which heat breaks down compounds

22
Q

why are some metals found in compounds

A

they are more reactive and react with substances around them

23
Q

e.g of why metals are found in compounds

A

most metals react with oxygen and sulfur forming metal oxides and sulphides

24
Q

what do most ores contain

A

oxide sulphide or carbonate of the metal oxides

25
Q

native metal

A

metal thats found uncombined in nature

26
Q

e.g of a native metal

A

platinum and silver

27
Q

ore

A

a rock from which metals can be extracted from

28
Q

mention three ores with the metal that gets extracted from it

A

haematite –> iron (oxide)
bauxite –> aluminum (oxide)
galena –> lead (oxide)

29
Q

why is the extraction of metal considered a reduction reaction

A

the ore is reduced to release to metal

30
Q

two steps for obtaining a metal from its ore

A

mining and collecting the ore
decomposition of the compounds in the ore

31
Q

three methods for reducing metal ores and extracting metals

A

heat alone (low reactive metals)
heat with carbon (middle reactive metals)
electrolysis (high reactive metals)

32
Q

how are mercury and silver extracted

A

thermal decomposition

33
Q

how are mercury and silver extracted

A

thermal decomposition

34
Q

which metals are extracted by heating with carbon

A

zinc iron nickel tin lead and copper

35
Q

endothermic:

A

gains heat/energy to make the reaction

36
Q

why is extraction by heating with carbon a reduction reaction

A

the metal oxide is reduced to release the metal

37
Q

electrolysis

A

splitting up the compound to extract the metal by passing electricity through a molten metal

38
Q

which metals are extracted by electrolysis

A

potassium sodium calcium magnesium and aluminum

39
Q

name 3 metals extracted by electrolysis

A

potassium sodium and magnesium

grade 9 chemistry (1 decks)

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