Atoms 2 (Brett) Flashcards

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1
Q

Are all metals as reactive as others?

A

No

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2
Q

Effects of a metal being more reactive

A

Higher tendency to become another compound with another substance

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3
Q

Metal + Acid –>

A

Salt + Hydrogen

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4
Q

Proof tests for hydrogen

A

Squeaky pop test (light a match in hydrogen to make it combust, and hence you hear a squeaky pop

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5
Q

Salt combination

A

Metal + Non-Metal

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6
Q

Reactivity Series (names)

A

1.Potassium
2.Sodium
3.Calcium
4.Magnesium
5.Aluminum
6.Carbon
7.Zinc
8.Iron
9.Tin
10.Lead
11.Hydrogen
12.Copper
13.Silver
14.Gold
15.Platinum

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7
Q

Reactivity series (symbols)

A

1.K
2.Na
3.Ca
4.Mg
5.Al
6.C
7.Zn
8.Fe
9.Sn
10.Pb
11.H
12.Cu
13.Ag
14.Au
15.Pt

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8
Q

relationship with electron shielding and electrons

A

The more shielding, the more reactive and easier it is to lose electrons since they have less traction with the nucleus

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9
Q

Displacement Reactions

A

Occurs when one element replaces the other in a compound, the more reactive substance replaces the less reactive one

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10
Q

What do chemicals need to react together

A

Kinetic energy

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11
Q

Methods of increasing likelihood of reactions

A

1.Increase concentration
2.Increase temperature
3.Increase surface area
4.catalyst

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12
Q

How increasing concentration helps

A

More particles to react and collide together

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13
Q

How increasing temperature helps

A

Particles become more energized and move faster, hence meaning more collisions

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14
Q

How increasing surface area helps

A

More of the substance is exposed with the other substance, hence more particles and more collisions

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15
Q

How catalysts help

A

They lower the activation energy needed for a reaction to happen

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16
Q

RoR

A

Rate of Reaction

17
Q

How to analyze a rate of reaction graph

A

The steeper the line, the faster the rate of reaction

18
Q

Endothermic reaction

A

when the energy of products is more than the energy of reactants, so energy is absorbed hence making it cold

19
Q

Exothermic reaction

A

When the energy of the products is less than the energy of the reactants, so energy is released making it hot

20
Q

Activation energy

A

The amount of energy needed for the reaction to begin

21
Q

Energy absorbed

A

The amount of energy the reactants absorb when forming new products

22
Q

Energy released

A

The amount of energy the reactants release when forming new products

23
Q

iron extraction method

A

1.Rocks of iron ore are found
2.These contain iron oxide
3.These are placed in a fire and heated up
4.Wood of charcoal is added so that carbon is present
5.Carbon displaces iron from iron oxide
6.Carbon dioxide and iron are formed
7.The pure iron can now be used

24
Q

Electrolysis

A

a process that extracts metals in their pure state by melting them down to a liquid state and the running electricity through them

25
Q

Elements that are extracted using electrolysis

A

Potassium (K), Sodium (Na), Calcium (Ca), Magnesium (Mg), Aluminum (Al)

26
Q

Elements that are extracted from their ores with a displacement reaction

A

Zinc (Zn), Iron (Fe), Lead (Pb), Platinum (Pt)

27
Q

Bauxite

A

aluminum oxide

28
Q

Hematite

A

Iron oxide

29
Q

Malachite

A

Copper carbonate

30
Q

Copper & Carbon method

A

1.Put 1 spatula of copper oxide powder in the crucible. Add one spatula of charcoal powder and mix the two together
2.Sprinkle 1 spatula of charcoal powder over the mixture. Put the lid on the crucible
3.Put the crucible, a pipe - clay triangle on a tripod. Put the Bunsen burner under the crucible
4.Heat the crucible strongly for 5 minutes
5.Turn off the Bunsen and wait. don’t remove the lid until the crucible has cooled down