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Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is an atom?

A

An atom is the smallest part of an element that can exist.

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2
Q

What do atoms have?

A

Protons, neutrons and electrons

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3
Q

Whats in an atoms nucleus?

A

Protons and neutrons.

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4
Q

What charge is the nucleus?

A

Positive because of the protons

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5
Q

What are electrons?

A

They move around the nucleus in electron shells, orbiting. they are negatively charged.

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6
Q

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

A

Protons is 1, neutrons is 1 and electrons is 0.

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7
Q

What are the relative charges of protons, neutrons and electrons?

A

protons are positively charged (+1), Neutrons have no charge (neutral) and electrons are negatively charged (-1)

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8
Q

What is an ion?

A

An ion is an atom that has either lost or gained electrons.

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9
Q

What does the atomic number tell you?

A

Tells you the number of protons and the number of electrons.

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10
Q

What does the mass number tell you?

A

Mass number tells you the number of protons and neutrons.

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11
Q

How to find the number of neutrons in an element?

A

you do mass number (neutrons + protons) - atomic number (protons) = neutrons.

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12
Q

What do the number of protons in the nucleus decide?

A

What type of atom it is. For example an atom with one proton in its nucleus is hydrogen and an atom with two protons is helium.

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13
Q

What is an element?

A

Its a substance that contains atoms with the same number of protons. So all atoms of a particular element have the same number of protons

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14
Q

Roughly how many elements are there?

A

100 elements.

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15
Q

How are elements arranged?

A

in the periodic table.

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16
Q

What are isotopes?

A

Isotopes are different forms of the same element, with the same number of protons but a different number of neutrons.

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17
Q

isotopes have the same atomic number but different -

A

mass numbers

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18
Q

give an example of an isotope and explain it?

A

carbon 12 and carbon 13.
in carbon 12 there are 6 protons, 6 neutrons and 6 electrons because the atomic number is 6 and mass number is 12.
However in carbon 13 there are 6 protons, 7 neutrons and 6 electrons because the atomic number is 6 but the mass number is 13.

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19
Q

What is relative atomic mass?

A

Relative atomic mass is an average mass taking in account the different masses and abundances of all isotopes that make up the element.

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20
Q

What is the formula for relative atomic mass?

A

Relative atomic mass (Ar) = (isotope abundance 1 * isotope mass number 1) + (isotope abundance 2 * isotope mass number 2) / sum of abundances of all isotopes (100)

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21
Q

Copper has two stable isotopes. Cu-63 has an abundance of 69.2 percent and Cu-65 has an abundance of 30.8 percent. Calculate the relative atomic mass of copper to 1 dp.

A

(6369.2) + (6530.8) / 30.8 + 69.2 (100)

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22
Q

What are compounds?

A

when elements react, atoms combine with other atoms to form compounds. Compounds are substances formed from two or more elements held together by chemical bonds.

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23
Q

How to make bonds?

A

Atoms giving away, taking, or sharing electrons. Only electrons are involved.

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24
Q

How to separate the original elements of a compound out again?

A

Chemical reaction

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25
Q

What is ionic bonding?

A

when a metal and non metal react. the metal loses electrons to form positive ions and non metal gains electrons to form negative ions. the opposite charges of the ions help them attract together.

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26
Q

what is covalent bonding?

A

when non metals share electrons with another.

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27
Q

What are molecules on the left hand side of a reaction called?

A

Reactants because they react together

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28
Q

What are molecules on the right hand side of a reaction called?

A

products because they have been produced from reactants.

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29
Q

Explain c+02 - c02

A

Carbon plus oxygen is carbon dioxide (carbon and 2 oxygen)

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30
Q

How to balance an equation?

A

find the number of atoms in the reactants and products. they must match up. if not place numbers in front.

31
Q

what are mixtures?

A

mixtures are two or more elements or compounds mixed together, without a chemical bond between.

32
Q

what is an example of a mixture.

A

Air can be a mixture of gases like oxygen and carbon dioxide.

33
Q

What is paper chromatography?

A

Separate compounds out of a mixture.

34
Q

what can paper chromatography be used for?

A

Separating mixtures, like dyes in an ink.

35
Q

How to do paper chromatography?

A

Draw a line near the bottom of a sheet of filter paper. Use pencil as insoluble. add a sport of ink to the line and place in a beaker of solvent like water. the solvent used depends on what’s being tested. Some compounds dissolve well in water.
Make sure the ink isn’t touching the solvent. Place a lid on top to prevent solvent evaporating. The solvent seeps up the paper carrying the ink with it. each different dye in the ink will move up at a different rate so the dyes will separate out. each dye will form a spot in a different place. If any of the dyes of ink are insoluble they will stay on base line. When the solvent has nearly touched the top take paper out and leave to dry. end is called a chromatogram.

36
Q

What does filtration do?

A

Separates insoluble solids from liquids.
pour into a beaker with funnel and filter paper at top. solid will stop at paper, and liquid will go to the beaker.

37
Q

What does evaporation do ?

A

separate soluble solids from solutions. pour solution into an evaporating dish. slowly heat and solvent evaporate and solution will get concentrated. eventually crystals will form. keep heating till you have dry crystals.

38
Q

what is positive and negative of evaporation?

A

Positive is that its fast, negative is that the salt might decompose when heated

39
Q

What is crystallization?

A

Pour solution in evaporating dish, gently heat the solution. Some of the solvent will evaporate and solution will become more concentrated. once started to evaporate, remove dish from heat and make it cool
salt will start to form crystals as it becomes insoluble in the cold.
filter crystals out and dry.

40
Q

what can filtration and crystallization be used to separate?

A

rock salt, grind mixture, dissolve in water, filter, and evaporate.

41
Q

What is simple distillation?

A

separates out solutions.
method -
- the solution is heated. the part of the solution that has the lowest boiling point evaporates first.
- the vapor is then cooled, condenses and is collected.
- the rest of the solution is left in the beaker.

42
Q

what is the problem with simple distillation?

A

you can only use to separate things with very different boiling points. if the temperature goes higher than boiling point of the substances with the the higher boiling point, they will mix again.

43
Q

What is fractional distillation?

A

separating mixtures of liquids with similar boiling points.
you put your mixture in a flask and stick fractional column on tip. then you heat it. the different liquids will all have different boiling points so they will evaporate at different temps. the liquid with lowest will evaporate first. when the temperature of the thermometer reaches the boiling point it will reach the top of the column.
liquids with higher boiling point will start to evaporate but the column is cooler towards the top. so they will only get part of the way up before condensing and running back down. the first liquid will be collected, you raise temp until next one reaches the top.

44
Q

Explain John Dalton’s theory?

A

John Dalton in 19th century said atoms were solid spheres and said that different spheres made up different elements. JJ Thomson concluded that they weren’t solid spheres. He said they contain electrons. The new theory was plum pudding model showed ball of positive charge with electrons stuck on it. then Rutherford showed that the plum pudding was wrong by shooting alpha particles at an extremely thin sheet of gold. expectation was that particles would pass straight through but they were deflected most the time. they came up with the idea that tiny positively charged nucleus at center because particles were deflected at the concentrated bit. otherwise they pass through empty space. Neil Bohr explained that electrons were in shells around the nucleus, and at a fixed distance from the nucleus. Further observations showed existence of protons and neutrons like James Chadwick.

45
Q

Explain JJ Thompsons theory?

A

JJ Thomson concluded that they weren’t solid spheres. He said they contain electrons. The new theory was plum pudding model showed ball of positive charge with electrons stuck on it.

46
Q

Explain Ernest Rutherford’s theory?

A

then Rutherford showed that the plum pudding was wrong by shooting alpha particles at an extremely thin sheet of gold. expectation was that particles would pass straight through but they were deflected most the time. they came up with the idea that tiny positively charged nucleus at center because particles were deflected at the concentrated bit. otherwise they pass through empty space.

47
Q

Explain Neil Bohr’s theory?

A

Neil Bohr explained that electrons were in shells around the nucleus, and at a fixed distance from the nucleus.

48
Q

Explain James Chadwick discovery?

A

Further observations showed existence of protons and neutrons like James Chadwick. Neutral particles in the center.

49
Q

What are some electron shell rules?

A

electrons always occupies shells.
the lowest energy levels are always filled first, the ones closest to nucleus
1st shell, 2 electrons, 2nd shell, 8 electrons, 3rd shell, 8 electrons.
atoms like full outer shell, and if its not full, atoms want to react to make them full.

50
Q

how were elements arranged?

A

By atomic weight and their physical and chemical properies.

51
Q

Who is Dmitri Mendeleev?

A

left gaps and predicted new elements, put elements in order of atomic weight.

52
Q

In the periodic table, the elements are laid out in order of..

A

increasing atomic number (protons)

53
Q

metals are found to the ……. and non metals are found to the ….

A

metals left
non metals right

54
Q

What are vertical columns called and why are they place there.

A

groups and they have similar properties

55
Q

what does group number tell you

A

the amount of electrons on outer shells.

56
Q

why called periodic table

A

as properties are said to occur periodically. Proton number 1, 2, 3 in periods.

57
Q

what are the rows called

A

periods and each new period represents another full shell of electrons.

58
Q

metals are elements that form

A

positive ions.

59
Q

Generally react to form a full outer shell by

A

losing, gaining or sharing electrons

60
Q

Physical properties of metals -

A

strong, can be bent or hammered (malleable), great at conducting heat and electricity, high boiling or melting points

61
Q

Non metal properties physical -

A

dull looking, brittle, aren’t always solids at room temp, don’t conduct electricity.

62
Q

what are transition metals

A

found between group 2 and 3. typical metals, catalysts so speed up reactions.

63
Q

Group 1 elements are

A

alkali metals

64
Q

In group 1 , as you go down the group… why?

A

the reactivity increases of the element. this is because outer electron is more easily lost, lower melting points and boiling points.

65
Q

characteristics of alkali metals -

A

one electron in outer shell, low density , lower melting and boiling points.

66
Q

How to group 1 elements react with non metals?

A

they form ionic compounds, all have 1 electron in their outer shell which they lose.

67
Q

How to group 1 elements with water

A

they react vigorously to produce hydrogen gas and metal hydroxides

68
Q

as you go down group 7……

A

halogens become less reactive, harder to gain an extra electron because they outer shell is further from nucleus
high melting pint and boiling point

69
Q

halogens can form molecular compounds by

A

sharing electrons with covalent bonding and with other non metals so they achieve full outer shell. molecular structures.

70
Q

a more reactive halogen will.. less reactive ones

A

displace

71
Q

a displacement reaction can occur between

A

a more reactive halogen and the salt of a less reactive one

72
Q

group 0 elements are.. and have

A

noble gases and have 8 electrons in outer shell

73
Q

compare group 1 metals with transition metals

A

group 1 and transition are heat and electricity conductors. shiny when polished and form ionic compounds with non metals
transition metals have higher densities and higher melting points. less reactive and harder than group 1.

74
Q

properties of noble gases, trends in properties down group

A

non metals, gases, low boiling points, unreactive, full outer shell
boiling point increases down the group, as the atoms get heavier.

Chemistry (4 decks)

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