the periodic table Flashcards

1
Q

before the 20th century, what could scientist measure regarding elements

A

relative atomic mass

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2
Q

what was noticed after arranging elements in order of mass

A

properties of elements where repeated at regular intervals

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3
Q

what are some problems with the early periodic tables

A

not all elements had been discovered so not compleate

ended up in the wrong group as they where placed in order of relative atomic mass

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4
Q

what did Dmitri Mendeleev do

A

1869
left gaps
mainly in order of atomic mass
but switched order of some elements
so elements with the same properties ended up in the same groups
the gaps allowed predictions to be made about undiscovered elements

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5
Q

what did the discovery of isotopes do

A

isopotops of the same elemnt have different atomic masses but the same chemical propeties so occopy the same place on the pt so mendeelev was right to leave gaps

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6
Q

what is the modern periodic table measured in

A

incresing atomic number

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7
Q

what does the period number tell you

A

how many electron shells

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8
Q

what does the group number tell you

A

how many electrons in the outer shell

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9
Q

what are metals

A

elements that form positive ions when they react

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10
Q

why cant non metals form positive ions

A

right of pt where they have lots of electrons to remove gto form a full outer shell or near the top where the outer shell elecrons have a strong force of attraction towards the nucleus.

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11
Q

physical properties of metals

A

strong
malible
great conductors of heat and elecricty.
high boiling and melting points.

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12
Q

physical properties of non metals

A

dull
brittle
lower bp and mp
lower density

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13
Q

what are the alkali metals and what are their properties

A

group 1: lithium, sodium, potassium, rubidium, caesium and francium

they are silvery solids that have to be kept in oil.
one elecron in their outer shells. low density and get more reactive down the group

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14
Q

why do alkali metels get more reactive down the group

A

elecron is further away from force of attraction of the nucleus

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15
Q

what happens to the boiling point going down group 1 elements

A

decreases down the group

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16
Q

what do the alkali metals make when they react with non metals

A

ionic compounds with a positive 1 charge.

the compounds are usually white solids that dissolve in water to form colourless solutions.

17
Q

what is the equation for the reaction of alkali metals with water

A

alkali metal + water = metal hydroxide + hydrogen

18
Q

why are the group 1 metals called alkali metals

A

the hydroxides formed when will dissolve in water to create alkali solutions

19
Q

what is the equation for the reaction of alkali metals with chlorine

A

metal chlorine

its white

20
Q

what is formed when alkali metals react with oxygen

A

metal oxide

21
Q

what elements are the halogens

A

Florine , chlorine, bromine, iodine and astatine

22
Q

how do the halogens exist in their natural state

A

in pairs

23
Q

halogens are metals that have what coloured vapours

A

fluorine - poisonous yellow gas
chlorine - poisonous dense green gas
bromine - poisonous dense red brown volatile liquid or orange vapour
iodine - poisonous dark grey crystalline solid or purple vapour

24
Q

what are the reactivity trends in the halogens

A

less reactive going down the group
because they react by gaining an electron
the outer shell is further away from the nucleus moving down the group so there is a smaller force of attraction from the nucleus

25
Q

what is the boiling point trend for the halogens

A

increase down the group

26
Q

what and how do halogens react with other non metals

A

other non metals
covalent bonds
the compounds formed have simple molecule structures

27
Q

what are formed when a halogen reacts with a metal

A

halide ions

28
Q

what do halogens do in displacement reactions

A

a more reactive halogen will displace a less reactive halogen from an aqueous solution of its salt

29
Q

name 3 noble gasses

A

helium, neon, argon

30
Q

why are the noble gasses inert

A

full outer shell of electrons

31
Q

what do noble gasses look like

A

colourless monatomic gases (single atoms not bonded)

32
Q

why does the boiling point of noble gasses increase going down the group

A

going down the group atomic number increases so there are more electrons which causes the intermolecular forces between the atoms to increase

33
Q

what are some properties of transition metals

A

good conductors of heat and electricity, dense, strong, shiny

34
Q

compare transition metals with alkali metals

A

tm are less reactive
tm are denser, stronger and harder
tm have much higher melting points

35
Q

why do transition metals form coloured compounds

A

due to the tm ion they contain.
e.g potassium chromate is yellow
potassium manganate is purple

36
Q

do transition metals make good catalyst

A

yes