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Chemistry Flashcards

Section 1 of Exam

1
Q

What is the first group on the periodic table known as?

A

Alkali Metals

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2
Q

What is the second group on the periodic table known as?

A

Alkaline Earth Metals

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3
Q

What is group seven on the periodic table known as?

A

Halogens

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4
Q

What is group eight on the periodic table known as?

A

Noble gases

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5
Q

What is shell shielding?

A

The more shells in-between the electrons and the nucleus the weaker the bond and the more shell shielding.

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6
Q

What charge do neutrons have?

A

No charge (neutral)

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7
Q

What charge do electrons have?

A

Negative charge (-)

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8
Q

What charge do protons have?

A

Positive (+)

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9
Q

What is the atomic number?

A

The number of protons in an atom.

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10
Q

What is the atomic weight?

A

The number of protons + neutrons.

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11
Q

How do you find then number of electrons?

A

It is the same number as protons.

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12
Q

How do you find the number of neutrons?

A

Atomic weight - Atomic number.

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13
Q

How do you find the number of protons?

A

The atomic number.

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14
Q

How are elements arranged on the periodic table?

A

In atomic number order.

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15
Q

What is all matter made up of?

A

Atoms.

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16
Q

What subatomic particles are found in the nucleus?

A

Neutrons and protons.

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17
Q

What subatomic particle orbits the nucleus?

A

Electrons.

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18
Q

Who invented the Solid Ball model?

A

Democritus.

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19
Q

What model did Democritus invent?

A

The Solid Ball model.

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20
Q

Who invented the Plum Pudding Model?

A

JJ Thompson.

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21
Q

What model did JJ Thompson invent?

A

The Plum Pudding model.

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22
Q

Who invented the Nuclear model?

A

Ernst Rutherford.

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23
Q

What model did Ernst Rutherford invent?

A

The Nuclear model.

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24
Q

Who invented the Planetary model?

A

Neils Bohr.

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25
Q

What model did Neils Bohr invent?

A

The Planetary model.

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26
Q

Who discovered neutrons?

A

James Chadwick.

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27
Q

What subatomic particle did James Chadwick discover?

A

Neutrons. (Planetary model with neutrons)

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28
Q

True or False :The atom as the smallest unit of an element and that can be represented by a symbol

A

True ;)

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29
Q

Periods go: (across/down)
Groups go:
(across/down)

A

Periods go across.
Groups go down.

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30
Q

What is the period number also equal to?

A

The period number is equal to the number of shells on the atom.

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31
Q

What is the group number also equal to?

A

The group number is equal to the number of valence electrons.

32
Q

What are valence electrons?

A

The electrons on the outermost shell.

33
Q

What is an ion?

A

A charged particle that has lost or gained electrons.

34
Q

Describe an electron configuration.

A

There can only ever be 2 electrons in the first shell and then 8 in each shell for the rest of them.
2, 8, 8, …. (Write like this)

35
Q

What happens as you go down group one?

A

The elements become more reactive because there is more shell shielding, and they all only have to lose one electron to become stable.

36
Q

Why is group 8 not reactive/stable? (Noble gases)

A

Elements in group 8 are stable/non reactive as they have full valence shells (all electron spots full).

37
Q

What happens as you go down group 7? (Halogens pattern of reactivity)

A

The elements become more reactive because there is more shell shielding, and they all only have to gain one electron to become stable.

38
Q

The periodic table is split into 2 sides, Metals and Non-metals, which side is which?

A

Metals are on the LEFT side and Non-metals are on the RIGHT.

39
Q

True or False: Chemical reactions involve rearranging atoms to form new substances;
during a chemical reaction mass is not created or destroyed.

A

True ;)

40
Q

When does a chemical change occur?

A

When old bonds between atoms are broken, the atoms are rearranged, and new bonds are formed.

41
Q

True or False: Atoms can be destroyed and created.

A

False ;)

42
Q

Ionic Bonding can only form between a _____ and a _____

A

Metal and a Non-Metal.

43
Q

Covalent bonds can from between a _____ and a _____

A

2 Non-Metals.

44
Q

Define an acid.

A
  • Have a ph of less than 7
  • (Strongest acids have a ph of 0)
  • Acids contain H+ ions (Hydrogen)
45
Q

Define an alkali/base.

A
  • Have a ph of more than 7
  • (Strongest bases have a ph of 14)
  • Bases that are soluble (dissolve in water) are called (an) alkali’s
  • Bases contain OH- ions (hydroxide)
46
Q

Define a salt.

A
  • A Neutral substance
    -Substance produced by the reaction of an acid and a base.
47
Q

What’s the difference between an alkali and a base?

A

Alkalis are bases that are soluble. (Can be dissolved in water)

48
Q

What is the ph Scale?

A

A measure of how acidic or alkaline a solution is.
- Scale ranges from 0-14.

49
Q

List 3 common acids. Include their chemical formula names.

A
  • Hydrochloric Acid
    HCl
    -Nitric Acid
    HNO3
    -Sulphuric Acid
    H2SO4
50
Q

List 3 common bases/alkali’s.
Include their chemical formula names.

A
  • Calcium hydroxide
    Ca(OH)2
  • Sodium Hydroxide
    NaOH
  • Magnesium Hydroxide
    Mg(OH)2
51
Q

Acid + Alkali ➔ _____ + _____

A

Salt + Water

52
Q

_____ + _____ ➔ Salt + Water

A

Acid + Alkali

53
Q

Acid + Metal ➔ ______ + ______

A

Salt + Hydrogen

54
Q

_____ + _____ ➔ Salt + Hydrogen

A

Acid + Metal

55
Q

Acid + Metal Oxide ➔ _____ + ______

A

Salt + Water

56
Q

_____ + ______ ➔ Salt + Water

A

Acid + Metal Oxide

57
Q

Acid + Metal Hydroxide ➔ ______ + _______

A

Salt + Water

58
Q

____ + ____ ➔ Salt + Water

A

Acid + Metal Hydroxide

59
Q

Acid + Carbonate ➔ _____ + _____ + _____

A

Carbon Dioxide + Water + Salt

60
Q

_____ + _______ ➔ Carbon Dioxide + Water + Salt

A

Acid + Carbonate

61
Q

Balance this Equation:
Zn + O2 → ZnO

A

2Zn + O2 → 2ZnO

62
Q

Balance this Equation:
NaOH + H3PO4 → Na3PO4 + H2O

A

3NaOH + H3PO4 → Na3PO4 + 3H2O

63
Q

Balance this Equation:
H2SO4 + KOH → K2SO4 + H2O

A

H2SO4 + 2KOH→ K2SO4 + 2H2O

64
Q

Name a very common antacid used to neutralize stomach acids.

A

Eno.

65
Q

What is an antacid?

A

A type of medication that neutralizes stomach acid to relieve discomfort caused by acid-related conditions.

66
Q

How do Antacids work?

A

Antacids work by raising the pH level in the stomach, making it less acidic.

67
Q

What is the test for Carbon Dioxide? Outline.

A

The Limewater test:
-To test gases for CO2 you pass it through Limewater.
Limewater = calcium hydroxide, Ca(OH)₂)
-The presence of CO2 is confirmed if the limewater turns milky or cloudy
-This is due to presence of calcium carbonate. (CaCO₃), which is insoluble in water and precipitates out, causing the cloudy appearance.

68
Q

What is the test for Hydrogen?

A

The Pop test:
- Hydrogen exposed to a flame makes a distinct popping sound.
-This occurs because hydrogen gas reacts explosively with oxygen in the air, forming water.

69
Q

Explain an Endothermic Reaction:

A
  • Heat transfers onto the object.
  • The object is cooler than its surroundings.
  • The object is left with more energy than when it started.
  • Taking in heat = Taking in energy.
70
Q

Explain an Exothermic Reaction:

A
  • Heat transfers out from the object.
  • The object is hotter than its surroundings.
  • The object has less energy than when it started.
  • Radiating heat = Losing energy.
71
Q

Name 2 examples of an endothermic reaction:

A
  • Ice Cube Melting
  • Evaporation of Water
72
Q

Name 2 examples of an exothermic reaction:

A
  • Combustion of fuels
  • Mixing Calcium Chloride with water.
73
Q

Explain how cold packs work:

A

When ammonium nitrate (NH4NO3) is dissolved in water, it absorbs heat from the surroundings, causing the solution to feel cold. This reaction is commonly used in instant cold packs.

74
Q

Explain how hot packs work:

A

Iron powder and water. Iron powder reacts with oxygen in the air, producing iron oxide (rust) and releasing heat in the process.

75
Q

What are the 4 state symbols?

A

(l) Liquids
(g) Gases
(s) Solids
(aq) Aqueous

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