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4th year Specific Learning Outcomes > Chemistry May 2015 > Flashcards

Chemistry May 2015 Flashcards

1
Q

What is precipitation?

A

Precipitation is when a solid is formed when two solutions are mixed.

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2
Q

What is the equation for average rate of reaction?

A

Average rate of reaction: change of quantity/ change in time

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3
Q

Describe the atom.

A

The atoms has a very small positively charged nucleus with negatively charged electrons moving around outside the nucleus.

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4
Q

Describe the location and charge of the three sub-atomic particles.

A

Protons- nucleus, 1+
Neutrons- nucleus, neutral (0)
Electrons- electron cloud, 1-

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5
Q

What is the relative mass of the proton, neutron and electron?

A

Proton- 1
Neutron- 1
Electron- Negligable

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6
Q

Ifsodium, Na, has an atomic number of 11 and mass number of 23 and has no overall charge, can you calculate the number of each sub-atomic particle?

A

Proton- same as atomic number, 11
Neutron- mass number-atomic number, 12
Electrons- no overall charge, 11

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7
Q

What is an ion?

A

An atom which has lost or gained electrons.

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8
Q

When are ions formed?

A

Ions are formed when atoms gain electrons to make negative ions or when atoms lose elctrons to form positive ions

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9
Q

If chlorine, Cl has an atomic number of 17, a mass number of 35 and a negative overall charge (Cl-), including ions, calculate the number of each sub-atomic particle?

A

Protons- gained negative charge (not positive), 17
Neutrons- mass- atomic, 18
Electrons- gained electron (negative charge), 18

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10
Q

What is an isotope?

A

Isotopes of an element are atoms with the same number of protons but a different number of neutrons. (same atomic number but different mass number).

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11
Q

What is a common isotope?

A

Chlorine with an atomic number of 17 but mass numbers of 35 and 37.

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12
Q

What happens in a covalent bond?

A

Two positive nuclei are held together by their common attraction for shared pair of electrons

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13
Q

Learn how to draw a diagram to show how the outer electrons form a covalent bond.

A
  • check jotter or summary notes- middle page.
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14
Q

What do ionic structures consist of?

A

Ionic structures consist of a giant lattice of oppositely charged ions.

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15
Q

Why don’t covalent substances conduct electricity?

A

Covalent substances do not conduct electricity since they are made up of molecules which are uncharged.

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16
Q

Why are formula equations balanced? (what does this show)

A

Formula equations can be balanced to show the relative number of moles of reactants and products.

17
Q

What is the gram formula mass of any substance known as?

A

The Mole

18
Q

What is the effect of dilution on the pH of an acid?

A

Diluting an acid will reduce the concentration of the H+ ions (hydrogen ions) , which increases the pH.

19
Q

What is the effect of dilution of the pH of an alkali?

A

Diluting an alkali with reduce the concentration of the OH- ions (hydroxide ions), which decreases the pH.

20
Q

What are the bases used to neutralize acidic solutions?

A

Reactive metals (MAZIT), metal oxide, metal hydroxide and metal carbonate

21
Q

What is a spectator ion?

A

A spectator ion is present during a chemical reaction but does not take part in the reaction.

22
Q

What is the equation for neutralisation with metal oxide?

A

Metal oxide + acid ———> salt + water

23
Q

What is the equation for neutralisation with reactive metals?

A

‘MAZIT’ metal + acid ——–> salt + hydrogen

24
Q

What is the equation for neutralisation with metal carbonate?

A

Metal carbonate + acid ——–> salt + carbon dioxide + water

25
Q

What is the equation for neutralisation with metal hydroxide?

A

Acid + metal hydroxide (Alkali) ——–> salt + water

26
Q

What shape of molecule is water? H20

A

bent, angular or v-shaped (check jotter for diagram)

27
Q

What shape of molecule is ammonia? NH3

A

Pyramidal (check jotter for diagram)

28
Q

What shape of molecule is methane? CH4

A

Tetrahedral (check jotter for diagram)

29
Q

What kind of solution does soluble metal oxides form?

A

Soluble metal oxides for alkaline solutions.

30
Q

What is the equation for titration?

A

C1 x V1/ n1 = C2 x V2/ n2

31
Q

How do you calculate the average burette reading?

A

Take an average of all titrations that took place.

4th year Specific Learning Outcomes (4 decks)

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