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Chemistry > Atomic structure and the periodic table > Flashcards

Atomic structure and the periodic table Flashcards

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1
Q

What is the radius of an atom?

A

0.1 nanometers

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2
Q

What does the nucleus of an atom contain?

A

protons and neutrons

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3
Q

What is the charge of a nucleus of an atom?

A

positive

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4
Q

What is the relative masses of the subatomic particles?

A

proton- 1
neutron-1
electron- very small

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5
Q

What are the charges of the subatomic particles?

A

proton- +1
neutron- 0
electron- -1

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6
Q

Whats the overall charge of an atom and why?

A

neutral because it has the same amount of protons as electrons

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7
Q

What is the atomic number?

A

how many protons there are in an atom

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8
Q

What is the mass number?

A

the number of neutrons and protons in an atom

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9
Q

What is an atoms element determined by?

A

the number of protons in its nucleus

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10
Q

What are isotopes?

A

different forms of the same element, which have the same number of protons and a different number of neutrons

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11
Q

What is the equation for relative atomic mass?

A

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

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12
Q

What is a compound?

A

two or more elements chemically bonded together

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12
Q

What is a mixture?

A

two or more elements that aren’t chemically bonded

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12
Q

What are some examples of mixtures?

A
  • air
  • crude oil
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13
Q

Describe the process of paper chromatography

A
  1. Draw a line near the bottom of a sheet of filter paper
  2. add a spot of the ink to the line and place the sheet in a beaker of solvent
  3. make sure the ink isn’t touching the solvent
  4. place a lid on the container to stop the solvent evaporating
  5. solvent seeps up the paper, carrying the ink with it
  6. each different dye in the ink moves up the paper at different so the dyes separate out
  7. If any of the dyes in the ink are insoluble they’ll stay on the baseline
  8. when the solvent has near reached the top of the paper take it out the solvent and leave it to dry
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14
Q

What can filtration be used for?

A
  • separating the soluble from solutions
  • for purification
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15
Q

What are the two ways to separate soluble solids from solutions?

A
  • evaporation
  • crystallisation
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16
Q

Describe the process of evaporation

A
  1. pour the solution into an evaporating dish
  2. slowly heat the solution. the solvent will evaporate and the solution will get more concentrated
  3. crystals will start to form
  4. keep heating the evaporating dish until all is left is dry crystals
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17
Q

When should you use crystallisation instead of evaporation?

A

if the salt decomposes when it’s heated

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18
Q

Describe the process of crystallisation

A
  1. pour the solution into an evaporating dish and gently heat the solution until some of the solvent evaporates and solution becomes more concentrated
  2. when crystals start to form, remove the dish from the heat and leave the solution to cool
  3. filter the crystals out and leave them in a warm place to dry
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18
Q

Describe the process of filtration

A
  1. grind the mixture to make sure the salt crystals are small, so will dissolve easily
  2. put mixture in water and stir, the salt will dissolve and the sand won’t
  3. filter the mixture- the salt will pass through the filter paper but the sand won’t
  4. evaporate the water from the salt so that it forms dry crystals
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19
Q

What is simple distillation used for?

A

separating out a liquid from a solution

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20
Q

Describe the process of simple distillation

A
  1. solution is heated- the part of the solution with the lowest boiling point evaporates first
  2. vapour is then cooled, condenses and is collected
  3. rest of the solution is left in the flask
21
Q

What can you use simple distillation for?

A

to get pure water from sea water

22
Q

What’s the problem with simple distillation?

A

you can only use it to separate things with very different boiling points

23
Q

Describe the process of fractional distillation

A
  1. put the mixture in a flask and stick a fractionating column on top and heat it
  2. the different liquids have different boiling points so evaporate at different temperatures
  3. liquid with the the lowest boiling point evaporates first- when the temperature on the thermometer matches the boiling point of the liquid, it will reach the top of the column
  4. liquids with higher boiling points might also start to evaporate but the column is cooler towards the top - so they will only get part way up before condensing and running back down the flask
  5. when the first liquid has been collected, you raise the temperature until the next one reaches the top
24
Q

What was John Dalton’s theory on atoms and when?

A

he describe atoms as solid spheres and said that different spheres make up different elements- start of 19th century

25
Q

Who made the plum pudding model and when?

A

JJ Thomson in 1897

26
Q

How did JJ Thomson conclude the plum pudding model?

A

he did some experiments and the measurements of charge and mass showed that an atom must contain electrons.

27
Q

What is the plum pudding model?

A

shows the atom as ball of positive charge with electrons stuck in it

28
Q

Who conducted the alpha particle scattering experiments and when?

A

Ernest Rutherford and his student Ernest Marsden in 1909

29
Q

What was the alpha particle scattering experiment?

A

They fired positively charged alpha particles at a thin sheet of gold

30
Q

What happened in the alpha particle scattering experiment?

A

they were expecting the particles to pass straight through but whilst most of the particles did go straight through but some were deflected more then expected.

31
Q

What was Rutherford’s nuclear model?

A

a tiny positive nucleus at the centre and a ‘cloud’ of negative electrons surrounds the nucleus

32
Q

Why was Rutherford’s nuclear model wrong?

A

because the negative ‘cloud’ around the nucleus would be attracted to the nucleus, causing the atom to collapse

33
Q

What is Bohr’s nuclear model?

A

electrons orbit the nucleus in fixed shells and aren’t anywhere in between.

34
Q

who discovered the protons?

A

Rutherford

35
Q

Who discovered the neutron?

A

James Chadwick

36
Q

In what order were the subatomic particles discovered?

A
  1. electrons
  2. protons
  3. neutrons
37
Q

In the early 1800s how were elements arranged?

A

by atomic weight

38
Q

When did Mendeleev create the periodic table?

A

1869

39
Q

What proved that Mendeleev was correct to not place elements in a strict order of atom weight but to also take their properties into consideration?

A

the discovery of isotopes

40
Q

how is the modern periodic table arranged?

A

increasing atomic number

41
Q

what ions do metals form?

A

positive ions

42
Q

why is it more difficult for non-metals to form in non-metals?

A

they have lots of electrons to lose to get a full outer shell- the electrons have a stronger attraction to the nucleus- easier for them to gain electrons to get a full outer shell

43
Q

What are the physical properties of metals?

A
  • strong
  • malleable
  • good conductors
  • high melting and boiling points
44
Q

What are the physical properties of non-metals?

A
  • dull looking
  • brittle
  • aren’t always solids at room temp
  • don’t generally conduct electricity
  • low density
45
Q

What are transition metals special properties?

A
  • they can have more than one ion
  • often coloured
  • good catalysts
46
Q

How do group one metals react with water?

A
  • react vigorously to produce hydrogen gas and metal hydroxides
  • amount of energy given out increases down the group
47
Q

How do group one metals react with chlorine?

A
  • react vigorously when heated in chlorine gas to form white metal chloride salts
48
Q

how do group one metals react with oxygen?

A
  • form metal oxides
49
Q

what do the different group one metals form when reacted with oxygen?

A
  • lithium- lithium oxide
  • sodium- mixture of sodium oxide and sodium peroxide
    potassium- mixture of potassium peroxide and potassium superoxide
49
Q

what are the ions formed by halogens called?

A

halides

50
Q

Describe all the halogens

A
  • Fluorine- very reactive, poisonous yellow gas
  • Chlorine- fairly reactive, poisonous dense green gas
  • Bromine- dense poisonous, red-brown volatile liquid
  • Iodine- dark grey crystalline solid or purple vapour
51
Q

What do group 0 elements exist as?

A

monatomic gases

52
Q

What are group 0 elements known as?

A

noble gases

53
Q

Why do noble gases’s boiling points increase down the group?

A

due to an increase in the number of electrons in each atom leading to greater inter molecular forces between them which need to be overcome.

Chemistry (7 decks)

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