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chemistry > atomic structure and the periodic table (paper 1) > Flashcards

atomic structure and the periodic table (paper 1) Flashcards

1
Q

chemical properties in group one metals

A

react with non metals to form compounds
very reactive
only forms ions with a 1+ charge
react with oxygen quickly
react with water vigorously
react with halogens easily

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2
Q

physical properties of group one metals

A

good thermal conductors
good electrical conductors
shiny and silver
low melting and boiling points
low densities
not as strong,soft

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3
Q

chemical properties of transition metals

A

react with non metals to form compounds
can form coloured compounds
not very reactive
forms ions with different charges
react with oxygen slowly
react with water slowly
react with halogens slowly
used as catalysts

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4
Q

physical properties of transition metals

A

good thermal conductors
good electrical conductors
high melting and boiling points
high densities
strong and hard

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5
Q

formula for atom economy

A

relative formula mass of desired product
———————————————— X100
the sum of relative formula masses of
all reactants

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6
Q

what is atom economy

A

a measure of the amount of starting materials that end up as useful products

when there is only one product we have 100% atom economy

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7
Q

why are group 0 elements not reactive

A

because they have a full outer shell

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8
Q

what is an isotope

A

atoms of the same element with the same no. of protons and electrons but a different no. of neutrons

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9
Q

what happens to the melting and boiling points as you go down in group seven

A

they increase

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10
Q

what are the halogens

A

a group of poisonous non metals

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11
Q

what happens to group 1 metals boiling and melting points as you go down the group

A

they decrease

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12
Q

why are alkali metals called that

A

the metal hydroxide they produce is alkaline and turns universal indicator purple

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13
Q

what does a metal and water produce when reacted

A

metal hydroxide + hydrogen

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14
Q

conclusions from alpha particle experiment

A

atoms must be mostly empty space ( most particles passed through)

must be a central concentration of mass, a nucleus (some particles bounced back)

the nucleus most have a positive charge (particles were deflected)

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15
Q

group zero name

A

noble gases
they get more reactive as you go down

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16
Q

group one name

A

alkali metals
they increase in reactivity as you go down

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17
Q

relative atomic mass formula

A

(isotope 1 x abundance) + (isotope 2 x abundance)
——————————————————
100

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18
Q

solvent

A

the liquid that the solid is dissolved into

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19
Q

solute

A

a solid which can dissolve

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20
Q

reactivity trend in group one

A

reactivity increases
more electrons
more shells
distance between the outer electron and the nucleus increases
more shielding by inner electrons
it’s easier to loose an electron

21
Q

reactivity trend in group 7

A

reactivity decreases
more shells
more electrons
distance between the outer electron and the nucleus increases
more shielding by inner electrons
more difficult to gain an electron

22
Q

percentage of an element formula

A

no. of atoms of element x
relative atomic mass of element
—————————————. X100
relative formula mass of compound

23
Q

radius of an atom

A

1 x 10 ^-10

24
Q

radius of a nucleus

A

1 x 10^-14

25
Q

john daltons theory of atomic structure - 1800s

A

described atoms as solid spheres and said that different spheres made up the different elements

26
Q

JJ thompson theory of atomic structure - 1897

A

concluded from his experiments that atoms weren’t solid spheres
his measurements of charge and mass showed that an atom must contain smaller negatively charged particles called electrons

created the plum pudding model which showed the atom as a ball of positive charge with electrons stuck in it

27
Q

alpha particle scattering experiment conclusions - 1910

A

most of the atom is empty space - most of the atoms went straight through the gold foil

the nucleus has a large positive charge - some were deflected through a big angle

the nucleus of the atom is very small - only a very small number rebounded

28
Q

ernest rutherford theory of atomic structure - 1911

A

made a new model which had a solid positively charged nucleus and the negatively charged electrons in ‘orbits’ around it

29
Q

neils bohr atomic structure theory - 1914

A

came up with the theory that the electrons must be orbiting the nucleus at set distances which he called shells

30
Q

james chadwick theory - 1932

A

he proved that there was a third particle that made up the atom called a neutron and that is particle was found in the nucleus

31
Q

how were elements originally ordered in the og period table

A

by atomic weight and did not take into account their properties

32
Q

physical properties of metals

A

they’re strong but can be bent or hammered into different shapes

they’re good at conducting heat and electricity

they have high boiling and melting points

33
Q

lithium reacting with oxygen observation

A

a pinkish red flame

a white powder is made

34
Q

sodium reacting with oxygen observations

A

see a yellow flame

made a white solid (sodium oxide)

35
Q

potassium reacting with oxygen observation

A

a purple flame which is vigorous

white powder is made

36
Q

lithium reacting with water observation

A

fizzed

stayed on the surface of the water

37
Q

sodium reacting with water observation

A

orange flame

fizzed

moves around quickly on the surface of the water and turned into a sphere

38
Q

potassium reacting with water observation

A

burned with a lilac flame

fizzed

exploded quickly

39
Q

metal + water

A

metal hydroxide + hydrogen

40
Q

percentage of an element equation

A

no. of atoms of the element x RAM of element
————————————————-
relative formula mass of compound
X100

41
Q

atom economy equation

A

relative formula mass of desired product
——————————————————-
sum of relative formula masses of all reactants

X100

42
Q

method for evaporation

A
  1. pour the solution into an evaporating dish
  2. slowly heat the solution, the solvent will evaporate and the solution will et more concentrated. eventually, crystals will start to form
  3. keep heating until the evaporating dish until all you have left are dry crystals
43
Q

method for crystallisation

A
  1. pour the solution into an evaporating dish and gently heat the solution, some of the solvent will evaporate and the solution will et more concentrated
  2. once some of the solvent has evaporated or when you see crystals start to form remove the dish from the heat and leave the solution to form
  3. the salt should start to form crystals as it becomes insoluble in the cold, highly concentrated solution
  4. filter the crystals out of the solution, and leave them in a warm place to dry
44
Q

what is the method for simple distillation

A
  1. used for separating out a liquid from a solution
  2. the solution is heated, the part of a solution that has the lowest boiling point evaporates first
  3. the vapour is then cooled, condenses and is collected
  4. the rest of the solution is left behind in the flask
45
Q

what is the problems with simple distillation

A

you can only use it to separate thins with very different boiling points - if the temperature goes higher than the boiling point of the substance with the higher boiling point, they will mix again

46
Q

what is the method for fractional distillation

A
  1. you put your mixture in a flask and stick a fractionating column on top, then you heat it
  2. the different liquids will all have different boiling points - so they will evaporate at different temperatures
  3. the liquid with the lowest boiling point evaporates first. when the temperature on the thermometer matches the boiling point of this 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 of the way up before condensing and running back down towards the flask
  5. when the first liquid has been collected you raise the temperature until the next one reaches the top
47
Q

how did Mendeleev order elements

A

put the elements mainly ion order of atomic weight but did switch that order if the properties meant it should be changed e.g. this happened with tellurium and iodine

48
Q

why did Mendeleev leave gaps in the table

A

to make sure that elements with similar properties stayed in the same groups - some of these gaps indicated the existence of undiscovered elements and allowed Mendeleev to predict what their properties may be

49
Q

what are the patterns in the properties of noble gases

A

boiling points increase as you go down the group - because there is an increase in the number of electrons in each atom leading to greater intermolecular forces between them which need to be overcome

chemistry (11 decks)

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