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Chemistry > C1 - Atomic Structure and The Periodic Table > Flashcards

C1 - Atomic Structure and The Periodic Table Flashcards

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1
Q

what is the smallest part of an element

A

atom

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2
Q

how many different elements are there

A

100

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3
Q

how are compounds formed

A

chemical reactions

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4
Q

what do chemical reactions always involve

A

the formation of one or more new substances, detectable energy change

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5
Q

what do compounds contain

A

two or more elements chemically combined in fixed proportions

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6
Q

how can compounds be split into elements

A

chemical reactions

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7
Q

what does a mixture consist of?

A

2 or more elements or compounds that are not chemically combined together

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8
Q

how can mixtures be seperated

A

physical processes:
crystallisation
simple distillation
fractional distilation
chromotography

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9
Q

what may lead to a change or replacement to a sceintific model

A

new experimental evidence

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10
Q

before the discovery of the electron, what were atoms thought to be

A

tiny spheres that could not be divided

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11
Q

what did the discovery of the electron lead to

A

the plum pudding model of the atom

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12
Q

what did the plum pudding model suggest

A

the atom is a ball of positive charge with negative electrons embedded in it

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13
Q

what was the conclusion from the results of the alpha particle scattering experiment

A

the mass of an atom was concentrated at the centre/ nucleus
the nucleus was charged

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14
Q

how did bohr adapt the nucleur model

A

suggesting that electrons orbit the nucleus at specific distances

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15
Q

after bohr adapted the nucler model, what did further experiments lead to?

A

the idea the positive charge of any nucleus could be subvided into a whole number of smaller particles, each particle having the same amount of positive charge. these were called protons

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16
Q

what did chadwicks work provide evidence for

A

the existance of neutrons within the nucleus

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17
Q

why did new evidence from the scattering experiment lead to a change in atomic model?

A

as most alpha particles passed through the gold foil so most of the atom is empty space. some alpha particles were deflected back so the atom has a positively charged nucleus

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18
Q

relative charges of the particles in the atom

A

proton - +1
neutron - 0’
electron - -1

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19
Q

what is the number of electrons equal to

A

number of protons in the nucleus

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20
Q

what is mass number

A

the number of protons and neutrons there are

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21
Q

what is the number of protons in an atom equal to

A

the atomic number

22
Q

what is the radius of an atom

A

0.1nm (1 x 10-⁸)

23
Q

what is the radius of the nucleus

A

1 x 10-¹⁴

24
Q

releative masses of protons neutrons electrons

A

proton - 1
neutron - 1
electron - very small

25
Q

what are isotopes

A

the same element but different number of neutrons

26
Q

what are elements in the periodic table arranged in order of

A

atomic number
so elements with similar properties were in the same group

27
Q

why is it called a periodic table

A

as elements w similar chemical properties occur periodically

28
Q

before the discovery of protons, neutrons and electrons, what was the periodc tabble arranged by

A

order of atomic weights

29
Q

how did mendeleev overcome some of the problems in the periodic table

A

by leaving gaps for elements he thought had not been discovered

30
Q

why did mendeleevs periodic table become more accepted

A

as he left gaps for elements he predicted were not discovered. later, these undiscovered elements were discovered and their properties matched his predictions

31
Q

what are group 0 called

A

noble gasses

32
Q

properties of noble gases

A

unreactive
dont easily form molecules
boiling point increases going down the group

33
Q

why are group 0 elements unreactive

A

they have a stable arrangement of electrons, 8 on the outershell

34
Q

what are group 1 elements known as

A

alkali metals

35
Q

general word equation for group 1 metal w water

A

metal + water —> metal hydroxide + hydrogen

36
Q

how do group 1 metals react w water

A

vigourosly to make hydrogen gas.
more reactive as you go down
potassium has enough energy to ignite the hydrogen

37
Q

how do group 1 metals react w chlorine

A

vigorously and produce white chloride salts
more vigorous as you go down

38
Q

how do group 1 metals react w oxygen

A

lithium reacts to form lithium oxide
sodium reacts to form sodium oxide and sodium peroxide
potassium makes potassium peroxide and potassium superoxide

39
Q

what are the chlorides formed when group 1 reacts w chlorine at room temp

A

white solids

40
Q

how does lithium react with water

A

fizzes steadily and slowly becomes smaller till it disapeares

41
Q

how does sodium react w water

A

fizzes rapidly and forms a ball

42
Q

how does potassium react w water

A

burns violently with sparks and a lilac flame. melts to form a ball and disappears quickly w a small explosion

43
Q

what are group 7 elements known as

A

halogens

44
Q

what do group 7 elements exist as

A

molecules made of pairs of atoms

45
Q

what can a more reactive halogen do to a less reactive one in an aqueous solution of salt

A

displacement

46
Q

how does the melting point of transition metals compare to group 1

A

higher melting points

47
Q

how do the densities of transition metals compare to group 1

A

higher densities

48
Q

how does strength and hardness of transition metlas compare to group 1

A

much harder and stronger

49
Q

how does the reactivity of transition metals with water, oxygen and halogens compare to group 1

A

they have a lower reactivity

50
Q

unique properties of transition metals

A

ions w different charges
form coloured compounds
useful for catalysts

51
Q

how do lithium, sodium and potassium react with water.

A

lithium - fizzes steadily and slowly becomes smaller until it disappears
sodium - fizzes rapidly, melts to form a ball and quickly becomes smaller until it disappears
potassium - burns violently with sparks and a lilac flame. melts quickly to forma. ball and disappears rapidly with a small explosion.

52
Q

how do group 7 react with non metals

A

floruine - burns and produces white iron (iii) florid
chlorine -

Chemistry (5 decks)

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