Periodic Table Flashcards

1
Q

what was Dalton’s theory

A

the atom was a solid sphere that was indestructible and all atoms of the same element were identical

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2
Q

what was JJ Thomson’s theory called

A

the plum pudding model

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3
Q

findings of Rutherford’s gold foil experiment

A

most particles passed straight through showing atom consisted of mainly empty space
few particles were deflected
few bounced back

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4
Q

structure of an atom

A

consists of protons, neutrons and electrons

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5
Q

atomic number

A

number of protons

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6
Q

mass number

A

number of protons and neutrons

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7
Q

what are isotopes

A

different atoms of the same element that have the same number of protons but different number of neutrons in their nuclei

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8
Q

why isotopes have similar chemical properties

A

they have the same number of electrons in their outer shell

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9
Q

2 ways isotopes are similar

A

same number protons in their nuclei

similar chemical properties

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10
Q

2 ways isotopes are different

A

different physical properties

different number of neutrons in their nuclei

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11
Q

what is relative atomic mass

A

average mass of an atom of an element relative ti 1/12th of the mass of an atom of carbon-12

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12
Q

how did Mendeleev arrange his elements

A

in order of increasing relative atomic mass

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13
Q

why did Mendeleev leave gaps

A

he assumed these elements had not been discovered yet and predicted the properties of some missing elements

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14
Q

3 similarities between Mendeleev’s table and modern table

A

elements put into groups
elements put into periods
elements with similar chemical properties put in same groups

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15
Q

what are group 1 metals called

A

the Alkali metals

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16
Q

what are group 7 elements called

A

the halogens

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17
Q

what are group 0 elements called

A

the noble gases

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18
Q

what does the period number show

A

number of occupied electron shells

19
Q

what does group number show

A

number of electrons in the outer shell

20
Q

how are G1 metals stored and why

A

under oil to prevent them from reacting with oxygen in the air

21
Q

metal + water ——–>

A

metal hydroxide + hydrogen

22
Q

properties of G1 metals

A
low densities
very reactive 
white ionic solids 
low melting points 
soft
good conductors of electricity
23
Q

why reactivity increase as you go down group 1

A

as you go down the group, the atom gets bigger because there is one more shell of electrons. The outer electron is further away from the nucleus and is more shielded by the inner shells of electrons. The outer electron is less strongly attracted to the nucleus, so is lost more easily

24
Q

what do you observe when G1 metal is added to water

A

fizzing
metal melts and float on water
lilac flame for K, Rb, Cs

25
Q

test for hydrogen

A

test gas with a lighted splint, there will be a squeaky pop

26
Q

chemical properties of G1 metals

A

react with water to produce alkaline solution
react with water, releasing hydrogen
react with acids

27
Q

why is a lilac flame seen when potassium reacts with water

A

reaction is exothermic and hydrogen is produced. Heat energy given out ignites the hydrogen causing a lilac flame

28
Q

uses of transition metals

A

construction
vehicles
electrical wiring

29
Q

physical properties of transition metals

A
malleable
ductile
good conductors of electricity
high melting points
high densities
shiny when polished
30
Q

chemical properties of transition metals

A

compounds are coloured
more than 1 oxidation state
catalysts

31
Q

why do halogens not conduct electricity

A

there are no free electrons

32
Q

what happens to the boiling points of halogens as you go down group and why

A

increase as larger molecules have larger forces of attraction between them , so intermolecular forces become stronger as you go down the group

33
Q

what happens to reactivity as you go down G7

A

atom get larger as there are more shells of electrons, so force of attraction between positive nucleus and incoming electron decreases. Reactivity decrease because it becomes more difficult for atom to form a negative ion

34
Q

test for chlorine gas

A

test gas with damp blue litmus paper. Litmus first turns red and then bleaches

35
Q

colour of bromine

A

orange

36
Q

colour of iodine

A

brown

37
Q

why are group 0 elements inert

A

they have a full outer shell of electrons so their atoms tend not to gain, share of lose electrons

38
Q

properties of group 0 elements

A

colourless gases at room temp
single atoms
very low MP and BP
poor conductors of heat and electricity

39
Q

uses of helium

A

weather balloons and airships

40
Q

why is helium used in weather balloons

A

have low density and is non - flammable

41
Q

uses of argon

A

added to space above wine barrels
lamps
welding

42
Q

why argon is used in lamps and welding

A

to provide an inert atmosphere and to stop oxygen reacting with metal (oxidation) due to high temp

43
Q

use of neon

A

illuminated signs and lasers