Atomic Structure and The Periodic Table Flashcards

1
Q

What subatomic particles are found in the nucleus of an atom?

A

protons and neutrons

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2
Q

What is the relative mass and relative charge of a proton?

A

Relative mass = 1
Relative charge = +1

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3
Q

What is the relative mass and relative charge of a neutron?

A

Relative mass = 1
Relative charge = 0

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4
Q

What is the relative mass and relative charge of an electron?

A

Relative mass = very small
Relative charge = -1

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5
Q

What is an isotope?

A

Different forms of the same element, which have the same number of protons but a different number of neutrons.

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6
Q

What is relative atomic mass?

A

An average mass taking into account the different masses and abundances of all the isotopes that make up an element.

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7
Q

What is the formula for relative atomic mass?

A

Ar = sum of (isotope abundance x isotope mass number) / sum of abundances of all the isotopes

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8
Q

Give the method on how to do paper chromatography.

A
  1. Draw a straight line near the bottom of the paper using a pencil.
  2. Add a spot of ink to the line and place in a beaker of solvent, making sure that the solvent isn’t touching the ink.
  3. The solvent seeps up the paper carrying the ink with it. When the solvent is near the top, take the paper out and leave to dry.
  4. Measure the solvent front (the point the solvent has reached) with a ruler.
  5. The end result is a pattern of spots called a chromatogram.
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9
Q

Give the method for making salts using crystallisation.

A
  1. Use a measuring cylinder to add 40 ml of sulfuric acid in a beaker.
  2. Gently heat the beaker in a water bath for a couple of minutes.
  3. Carefully add a spatula of copper oxide powder to the beaker and stir the solution with a glass rod, add in excess until it no longer disappears.
  4. Filter the mixture using a funnel and filter paper to remove the excess copper oxide.
  5. Then pour the filtrate (the copper sulfate solution) into an evaporating basin
  6. place the evaporating basin above a bunsen burner on a tripod and gauze, and heat the copper sulfate solution to evaporate off half of the water.
  7. Pour the solution into a watch glass and leave on a windowsill or dry area to allow all of the water to evaporate or pat dry.
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10
Q

Explain how filtration and crystallisation can be used to separate rock salt.

A
  1. Grind the mixture to make sure the salt crystals are small so will dissolve easily.
  2. Put the mixture in water and stir.
  3. Using filter paper and a funnel, filter the mixture into a beaker.
  4. Evaporate the water from the salt so that it forms dry crystals.
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11
Q

Explain simple distillation.

A
  1. Used for separating out a liquid from a solution.
  2. The solution is heated. The part of the solution that has the lowest boiling point evaporates first.
  3. The vapour then travels up the flask and is condensed in a condenser back into a liquid.
  4. The liquid is collected in a beaker and the rest of the solution remains in the flask.
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12
Q

Explain fractional distillation.

A

Used to separate a mixture of liquids.
1. Put the mixture in a flask with a fractionating column on top. Heat over a bunsen burner.
2. The different liquids have different boiling points so will evaporate at different temperatures.
3. The liquid with the lowest boiling point evaporates first. The vapour travels up the fractionating column and then condenses into a liquid.
4. Liquids with higher boiling points might also start to evaporate but the column is cooler towards the top so it will only get part way before condensing and running back down the flask.
5. When the liquid has been collected, raise the temperature to collect the next liquid.

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13
Q

How has the theory of atomic structure changed over time?

A

19th Century
- John Dalton described atoms as solid spheres and said different spheres were made of different elements

1897
- JJ Thompson created the plum pudding model consisting of a positively charged mass containing smaller negatively charged electrons

1909
Ernest Rutherford conducted an experiment that concluded that when alpha particles were fired at thin sheets of gold, most particles passed through empty space but a few were deflected by the nucleus.

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14
Q

How did Rutherford show that the plum pudding model was wrong?

A

Alpha particle scattering experiments
- fired charged alpha particles at a thin sheet of gold
- they were expecting particles to pass straight through or be slightly deflected at most however more than expected were deflected or deflected backwards.
- This meant that there was a positively charged nucleus within an atom consisting mostly of empty space

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15
Q

What is the plum pudding model?

A

A positively charged mass containing smaller negatively charged particles called electrons.

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16
Q

What does Bohr’s nuclear model show?

A

Electrons are contained in shells and orbit the nucleus. Each shell is a fixed distance from the nucleus.

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17
Q

How were elements arranged in the early 1800s?

A

By atomic mass.

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18
Q

What did Dmitri Mendeleev arrange the elements in order of?

A

In order of atomic mass but he left gaps to make sure that elements with similar properties stayed in the same group. Some of these gaps indicated the existence of undiscovered elements.

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19
Q

True or false : Most elements in the periodic table are metals.

A

True

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20
Q

What are metals?

A

Elements which can form positive ions when they react.

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21
Q

Where are non-metals located in the periodic table?

A

The top far right.

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22
Q

What does the electronic structure of atoms affect?

A

How they will react.

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23
Q

What are the physical properties of metals?

A
  • Strong but malleable
  • Great at conducting heat and electricity
  • High melting and boiling points
24
Q

What are the physical properties of non-metals?

A
  • Dull looking
  • More brittle
  • Aren’t always solids at room temp
  • Don’t generally conduct electricity
  • Low densities
25
Q

What are transition metals?

A

Typical metals that have typical metal properties:
- good conductors of heat and electricity
- dense
- strong
- shiny

26
Q

Where are the transition metals located in the periodic table?

A

In the centre of the periodic table.

27
Q

Complete the sentence : Transition metals can have more than one _____.

A

ion

28
Q

What type of metal ions are often coloured?

A

Transition metal ions.

29
Q

Complete the sentence: Transition metal compounds often make good _________.

A

catalysts

30
Q

What are the group 1 elements often known as?

A

The alkali metals.

31
Q

Name the alkali metals in order of reactivity.

A

Most reactive
Francium
Caesium
Rubidium
Potassium
Sodium
Lithium
Least Reactive

32
Q

What are the trends for the alkali metals as you go down?

A
  1. Increasing reactivity (the outer electron is more easily lost as further from nucleus)
  2. Lower melting and boiling points
  3. Higher relative atomic mass
33
Q

What do alkali metals form ionic compounds with?

A

non-metals

34
Q

What is the reaction of alkali metals in water?

A
  • Vigorous reaction
  • Hydrogen gas and metal hydroxides produced
  • The most reactive element is the most violent reaction
  • The amount or energy given out by the reaction increases down the group
35
Q

What is the reaction of alkali metals with chlorine?

A
  • Vigorous reaction when heated
  • Metal chloride salts produced
  • Increased reactivity means more vigorous reaction
36
Q

What is the reaction of alkali metals with oxygen?

A
  • Forms metal oxides
  • Type of oxide depends on the metal
37
Q

What are the differences in properties between group 1 metals and transition metals?

A

Group 1
- More reactive
- React more vigorously
- Less dense
- Less strong
- Less hard
- Lower melting points

38
Q

What are the group 7 elements also known as?

A

The Halogens

39
Q

What are the halogens?

A

Non-metals with coloured vapours

40
Q

Which halogen is most reactive?

A

Fluorine

41
Q

Which halogen is least reactive?

A

Astatine or Iodine

42
Q

What colour gas is fluorine?

A

Yellow

43
Q

What colour gas is chlorine?

A

green

44
Q

What colour gas is bromine?

A

red-brown

45
Q

What colour gas is iodine?

A

purple or a dark grey crystalline solid

46
Q

What are the trends as you go down the halogens?

A
  1. Less reactive (harder to gain electron)
  2. Higher melting and boiling points
  3. Higher relative atomic mass
47
Q

What type of compounds can halogens form?

A

molecular

48
Q

How do halogens share electrons?

A

Via covalent bonding

49
Q

What bonds to halogens form with metals?

A

Ionic

50
Q

Complete the sentence : More reactive halogens will displace _______ _________ ________.

A

less reactive halogens

51
Q

What are Group 0 elements also known as?

A

The noble gases.

52
Q

True or false : The noble gases are very reactive.

A

false

53
Q

What are the first three noble gases?

A

Helium, neon and argon

54
Q

What are monatomic gases?

A

Single atoms not bonded to each other.

55
Q

Are noble gases flammable?

A

No they are inert.

56
Q

What happens to the boiling point of the elements as you go down group 0?

A

Increases, along with relative atomic mass