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chemistry 101 > atomic structure and the periodic table > Flashcards

atomic structure and the periodic table Flashcards

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1
Q

what is the nucleus in terms of atoms?

A

its the middle of the atom and it contains protons and neutrons

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2
Q

what is an electron?

A

it moves around the nucleus in electron shells, its negatively charged. it has virtually no mass

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3
Q

what are the charges and relative mass of a proton, neutron and electron?

A 
charge
       proton: +1
       neutron:0
       electron:-1
relative mass
       proton: 1
       neutron:1
       electron:very small
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4
Q

why is an atom neutral?

A

it has the same number of protons ad electrons, the charges are the same but opposite so they cancel each other out

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5
Q

why do ions have an overall charge?

A

because the number of protons doesn’t equal the number of electrons

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6
Q

what does the atomic number and the mass number of an atom tell you?

A

atomic number: proton number

mass number: total number of protons and neutrons

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7
Q

how do you get the number pf neutrons?

A

atomic number - mass number

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8
Q

what is an element?

A

a substance made up of elements that all have the same number of protons in their nucleus

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9
Q

what decides what type of atom it will be?

A

the number of protons

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10
Q

what is an isotope?

A

Different form of the same element which has the same number of protons but a different number of neutrons

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11
Q

name an example of an isotope

A

carbon -12 carbon-13
6 protons 6 protons
6 electrons 6 electrons
6 neutrons 7 neutrons

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12
Q

because many elements exist with a number of isotopes, what is used instead of the mass number to refer to an element?

A

relative atomic mass(Ar)

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13
Q

how do you calculate relative atomic mass?

A

sum of (isotope abundance x isotope mass number)
Ar= ————————————————————————–
sum of abundance of all the isotopes

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14
Q

copper has two stable isotopes. Cu-63 which has an abundance of 69.2% and Cu-65 which has an abundance of 30.8%. calculate the relative atomic mass of copper to 1 d.p

A

sum of (isotope abundance x isotope mass number)
Ar= ————————————————————————-
sum of abundance of all the isotopes

  (69.2 x 63)+(30.8 x 65)     4359.6+2002     6361.6 Ar= --------------------------------  = --------------------- = ---------  =63.6
      69.2 + 30.8                            100                  100
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15
Q

what is a compound?

A

a substance formed from two or more elements held together by a chemical bond

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16
Q

what does bonding include?

A

giving away, taking or sharing electrons

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17
Q

what do you call a compound which is formed from a metal and non metal bonding?

A

ion

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18
Q

how does ionic bonding happens?

A

the metal atom loses electrons to form a positive ion and the non metal atom gains electrons to form negative ion, the opposite charges of the ions means that they’re strongly attracted to each other

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19
Q

how is the compound NaCl formed in terms of ionic bonding?

A

sodium is in group 1 so it has one outer electron and chlorine is in group 7 so it has 7 outer electrons
an atom needs a full outer shell, so sodium will lose one electron to chlorine and become a positive ion and chlorine will become negative ion and the opposite charges will have a strong attraction

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20
Q

what does a compound formed from non-metals consists of?

A

molecules

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21
Q

what happens during covalent bonding?

A

each atoms shares an electron with each other

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22
Q

name an example of a compound that is bonded covalently

A

any of theses:
hydrogen chlorine gas
carbon monoxide
water

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23
Q

balance this equation:

H²SO4 + NaOH —> Na²So4 + H²O

A

there isn’t enough H atoms on the right hand side,, so you add 2H²O:
H²SO4 + NaOH →Na²So4 + 2H²O
there’s too many H and O atoms on the RHS now, so to balance the LHS, put 2NaOH

H²SO4 + 2NaOH → Na²So4 + 2H²O

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24
Q

what is a mixture?

A

a material made up of two or more different substances which are not joined chemically and can be separated

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25
Q

name one way you can separate a mixture out

A 
any of these:
filtration
crystallization
simple distillation/fractional distillation
chromatography
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26
Q

describe how does paper chromatography work?

A

1) you draw a line near the bottom of a sheet of filter paper
2) add a spot of ink to the line and place the sheet in a beaker of solvent
3) the bottom of the paper not the ink has to be touching the solvent
4) solvent seeps up the paper carrying the ink up the paper
5) each different dye in the ink will move up the paper at a different rate so the dyes will separate out, each dye will form a spot in a different place
6) when the solvent has almost reached the top, take the paper out and leave to dry

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27
Q

how do you calculate the Rf ( Retention factor)?

A

distance traveled by solute( dye)
Rf=——————————————
distance traveled by solvent

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28
Q

how does filtration work?

A

it separates insoluble solids from liquids

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29
Q

describe how evaporation work?

A

1) pour a solution into an evaporating dish
2) slowly heat the solution. the solvent will evaporate and the solution will get more concentrated. eventually crystals will form
4) keep heating the dish till the only thing left is dry crystals

30
Q

describe how crystallization works?

A

1) pour the solution into an evaporating dish and gently heat the solution, the solution will get more concentrated. eventually crystals will form
2) once some of the solvent has evaporated, or when you see crystals forming, remove the dish from the heat and leave the dish to cool
3) the salt should start to form crystals as it becomes insoluble in the cool, highly concentrated solution
4) filter the crystals out of the solution, leave them to in a warm place to dry.

31
Q

what is simple distillation used for?

A

to separate mixtures which contain liquids

32
Q

how does simple distillation work?

A

1) the solution is heated. the part of the solution that has the lowest boiling points evaporates first
2) the vapour is then cooled, condensed and is collected
3) the rest of the solution is left in the flask

33
Q

name one use for simple distillation

A

to get pure water from seawater

34
Q

name one problem of simple distillation

A

it only works to separate things with very different boilings points

35
Q

what is fractional distillation used for?

A

its used to separate a mixture of liquids

36
Q

how does fractional distillation work?

A

1) you put a mixture into a flask and stick a fractional column on top. Then you heat it
2) the different liquids will have different boiling points, so they will evaporate at different temperatures
3) the liquids with the lowest boiling point will evaporate first. When the temp on the thermometer matches the boiling point of this liquid, it will reach the top of the column
4) when the first liquid has been collected, you raise the temp until the next one reaches the top

37
Q

what did John Dalton think the atom looked like?

A

a solid sphere

38
Q

who invented the plum pudding model and how did he discover it and what did it look like?

A

J.J Thomson, his measurements of charges and mass showed that an atom must contain even smaller, negatively charged particles. The plum pudding model showed a ball of positive charge with electrons stuck in it

39
Q

who proved the plum pudding model wrong and how?

A

Ernest Rutherford, by conducting an alpha particle scattering experiment. They fired positively charged alpha particles at a thin sheet of gold, they were deflected so the plum pudding model couldn’t be right

40
Q

what did Rutherford’s nuclear model look like

A

a tiny, positively charged nucleus at the centre (most of the mass is concentrated here). A ‘cloud’ of negative electrons surrounds it- so its mostly empty space

41
Q

who came up with the idea of electrons being in shells around the nucleus?

A

Neils Bohr

42
Q

what are the rules of the electron shell?

A

only a certain number of electrons is allowed in each shell, 1st shell: 2 2nd shell: 8 3rd shell: 8
atoms want a full outer shell

43
Q

what is the electronic structure of

1) magnesium
2) calcium
3) Neon

A

1) 2,8,2
2) 2,8,8,2
3) 2,8

44
Q

who created the early period table and how was it arranged?

A

Dmitri Mendeleev and it was arranged by order of atomic mass

45
Q

why were there gaps in the early period table?

A

to make sure that elements with similar properties stayed in the same group

46
Q

why was Mendeleev correct not to put the elements in a strict order of atomic mass?

A

the discovery of isotopes with different atomic masses but the same chemical properties

47
Q

how are the elements arranged in the modern periodic table?

A

in order of increasing atomic(proton) number

48
Q

chlorine and bromine react in a similar way. suggest a reason why

A

they are both in group 7

49
Q

what ions do metals form when they react?

A

positive

50
Q

state the two differences between metals and non-metals

A 
any of these two:
metals are strong, but can be malleable
they are great at conducting heat and electricity
high melting and boiling points 
non-metals are brittle and not malleable
don't conduct electricity 
low melting and boiling points
51
Q

what metals are in group 1?

A

alkali metals

52
Q

why are group 1 metals the most reactive?

A

they have one electron in their outer shell

53
Q

name one trends of group 1 metals as you go down?

A

any of these:
increasing reactivity
lower melting and boiling point
higher relative atomic mass

54
Q

what happens when you place group 1 element sodium in water?

A

float and move around the surface fizzing furiously

55
Q

what gas is produced when group 1 elements react with water

A

hydrogen

56
Q

finish the equation for water reacting with sodium

2Na(s) + 2H²O(l) —–>

A

a hydroxide is formed

2Na(s) + 2H²O(l)→ 2NaOH(aq) + H²(g)

57
Q

what do group 1 metals reacting with chlorine gas form?

A

a salt (metal chloride)

58
Q

finish the equation for chlorine gas reacting with sodium

2Na(s) + Cl²(g) ——->

A

2Na(s) + Cl²(g) →2NaCl(s)

59
Q

what do group 1 metals reacting with oxygen form?

A

metal oxide

60
Q

finish the equation for the mixture formed by oxygen reacting with sodium
2Na(s) + O(g) ——->

A

2Na(s) + O(g) → Na²O (sodium oxide0

→ Na²O²(sodium peroxide)

61
Q

what are group 7 elements called?

A

the halogen

62
Q

what colour vapour do these halogens produce?

1) fluorine
2) chlorine
3) bromine
4) iodine

A

1) fluorine - yellow
2) chlorine - dense green
3) bromine - red-brown volatile
4) iodine - purple

63
Q

name two trends of group 7 elements as you go down

A

any two of these:
less reactive
higher melting and boiling point
higher relative atomic mass

64
Q

what type of compound do halogens reacting with non-metals make? give an example

A

molecular compounds , HCl

65
Q

what ion does a halogen form when bonding with a metal?

A

1-ion called halides

66
Q

what are group 0 elements called?

A

noble gases

67
Q

why are they nonreactive?

A

they already have 8 electrons in their outer shell (apart from helium)

68
Q

name the two patterns of noble gases as you go down

A

the boiling point and the relative atomic mass increases

69
Q

neon is a gas at 25 degrees. predict what state helium is at this temp

A

helium has a lower boiling point than neon so helium is also gas at 25ºC

70
Q

radon and krypton have a boiling point of -62 and -153. predict the boiling point of xenon

A

xenon comes between radon and krypton
(-153)+(-62)= -215
-215/2 = -107.5 round up to -108
(xenon’s actual boiling point is -108)

chemistry 101 (2 decks)

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