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Chemistry Flashcards

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1
Q

What is the mass and charge of protons, neutrons and electrons?

A

Protons - Mass=1 and charge=+1
Neutrons - Mass= 1 and charge=0
Electrons - Mass= 0.0005 and charge=-1

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2
Q

Name the first 20 elements of the periodic table and their charges and the names of Fe, Ni, Cu, Zn, Pb, Ag, Sn, Au, Hg.

A 
Hydrogen H
Helium He
Lithium Li
Beryllium Be
Boron	B	
Carbon C	
Nitrogen	 N	
Oxygen O	
Fluorine F	
Neon Ne	
Sodium Na	
Magnesium Mg	
Aluminium Al	
Silicon Si	
Phosphorus P	
Sulfur	S	
Chlorine	Cl
Argon	Ar	
Potassium	K	
Calcium	Ca	
Iron Fe
Nickel Ni
Copper Cu
Zinc Zn
Lead Pb
Silver Ag
Tin Sn
Gold Au
Mercury Hg
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3
Q

Complete the general rule for Acid + Metal, Acid + Base, Acid + Carbonate reactions.

A

Acid + Metal —> Salt + Hydrogen Gas

Acid + Base —> Salt + Water

Acid + Carbonate —

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4
Q

What are the mass and charge of protons, neutrons and electrons?

A

Protons - mass=1 charge=+1

Neutrons - mass=1 charge=0

Electrons - mass=0.0005 charge=-1

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5
Q

Describe the atomic structure of an ionic compound.

A

At least one metal atom bonded with at least one non-metal atom.

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6
Q

Describe the atomic structure of a covalent compound.

A

At least two non-metal atoms bonded together.

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7
Q

Explain the role of activation energy in chemical reactions.

A

The energy that must be supplied for the chemical reaction to occur.

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8
Q

What is the law of conservation of mass?

A

Matter cannot be created or destroyed therefore, the mass of the product(s) will be the same as the mass of the reactant(s).

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9
Q

List 3 properties of acids.

A
  • they conduct electricity
  • they are corrosive
  • they have a sour taste
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10
Q

List 3 properties of bases.

A
  • they conduct electricity
  • they have a bitter taste
  • they create hydroxide ions in a solution
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11
Q

What number on the PH scale are strong acids, weak acids, neutral, weak bases and strong bases.

A 
Strong acids- 1
Weak acids- 6
Neutral- 7
Weak bases- 8
Strong bases- 14
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12
Q

List 2 examples of strong and weak acids.

A

Strong

  • HCl (hydrochloric)
  • H2SO4 (sulphuric)

Weak

  • HNO2 (nitrous)
  • H3PO4 (phosphoric)
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13
Q

List 2 examples of strong and weak bases.

A 
Strong
- LiOH (Lithium Hydroxide)
- NaOH (Sodium Hydroxide)
Weak
- NH3 (ammonia)
- CH3NH2 (methylamine)
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14
Q

Explain the concept on concentration in terms of acids and bases.

A

The concentration of acids and bases is determined by the amount of Hydrogen to Hydroxide ions there are in a solution. The more Hydrogen ions, the more the solution is acidic in concentration. The more Hydroxide ions, the more the solution is basic in concentration.

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15
Q

What is an indicator?

A

A chemical that changes colour to show whether a substance is acidic, neutral or basic.

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16
Q

Describe the colour changes of Universal Indicator to signify a strong acid, a weak acid, a strong base, a weak base and a neutral solution.

A 
Red- strong acid
Light green- weak acid
Green- neutral
Faint green- weak base
Purple- Strong Base
17
Q

What colour does litmus turn in acid?

A

Red

18
Q

What colour does litmus turn in alkali (base dissolved in water)?

A

Blue

19
Q

Write and word and symbol equation for any acid and base reaction.

A

Hydrochloric Acid + Sodium Hydroxide —> Sodium Chloride + Water

20
Q

Write a word and symbol equation for any acid and metal reaction.

A

Hydrochloric Acid + Sodium —> Sodium Chloride + Hydrogen Gas

21
Q

How would you test a gas to see if it was Hydrogen?

A

The ‘Pop Test’ - Put HCl in a test tube and add a magnesium strip and put another test tube over the original one for a minute. Then take the top test tube away and place a burning match underneath it. If it makes a loud ‘POP’ sound, it is then Hydrogen.

22
Q

Write a word and symbol equation for any acid and carbonate reaction.

A

Hydrochloric Acid + Potassium Carbonate —> Potassium Chloride + CO2 + Water

23
Q

How would you test a gas to see if it was carbon dioxide?

A

The ‘Lime Water’ Test- Pass any gas through limewater. If the solution become cloudy, then the gas is Carbon Dioxide.

24
Q

What is the difference between Exothermic reactions and Endothermic reactions?

A

Exothermic- the temperature of the reaction increases because it requires heat to exit for the reaction to continue.

Endothermic- the temperature of the reaction decreases because it requires heat for the reaction to continue.

25
Q

Define element.

A

Element- a substance made up of only one type of atom.e.g. Hydrogen (H)

26
Q

Define molecule.

A

Molecule- a cluster of atoms that makes up an element or compound.e.g. Nitrogen (N2)

27
Q

Define compound.

A

Compound- a pure substance that is made up of 2 or more different types of atoms chemically joined.e.g. Water (H2O)

28
Q

Define base.

A

Base- a substance that releases hydroxide ions.

29
Q

Define acid.

A

Acid- a substance that releases hydrogen ions into an aqueous solution.

30
Q

Define ionic bonding.

A

Ionic bonding- when cations (positive charged ion) and anions (negative charged ion) are both attracted to one another because of their opposite charges. When they stick together, this is when they’re known as an ionic bond.

31
Q

Define covalent bonding.

A

Covalent bonding- a chemical bond that involves the sharing of electron pairs between atoms.

32
Q

Write a word equation for a combustion reaction.

A

Methane + Oxygen Gas —

33
Q

Write a word equation for an incomplete combustion reaction.

A

Methane + Oxygen Gas —

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