c1 - atomic structure and the periodic table Flashcards

1
Q

size of atom

A

1x10 -10m

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2
Q

radius of a nucleus

A

1 x 10 -14m

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3
Q

why do atoms have no overall charge

A

the relative charge for an electron is -
and proton is +
number of electrons = number of protons

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4
Q

what is mass number

A

total number of neutrons and protons

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5
Q

avogados constant

A

6.02 x 10^23

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6
Q

what is atomic number

A

number of protons

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7
Q

electron shell limits

A

2,8,8,2

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8
Q

what is an isotope

A

Atoms of the same element can have different numbers of neutrons

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9
Q

abundance equ

A

(isotopic mass number x abundance) + (isotopic mass number x abundance) divided by 100

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10
Q

jj thomson plum pudding model

A

A ball of positive charge with electrons embedded inside.

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11
Q

how did rutherford prove the plum pudding model was wrong

A

Alpha particle scattering experiment.

Fired positive alpha particles at gold foil.

Most particles passed straight through = mainly empty space.

Only a few were deflected back = small positively charged centre where mass is

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12
Q

what did bohr do to the nuclear model

A

electrons orbit the nucleus
at specific distances from the nucleus

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13
Q

what is an element

A

made of only 1 type of atom. Found in the periodic table

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14
Q

what is a compound

A

2 or more elements chemically joined together in a fixed ratio.

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15
Q

what is a mixture

A

2 or more elements or compounds, not chemically joined.

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16
Q

How would you extract salt from a sand and salt solution?

A

Filter to remove the sand.
Evaporate to remove the water.

17
Q

Separating mixtures

A

Filtration

Chromatography

Distillation

18
Q

newlands development of the periodic table

A

Ordered by atomic weight
Elements were therefore in wrong groups
Metals were in groups with non metals

19
Q

mendeleev development of the periodic table

A

Ordered in atomic weight but changed it so elements are in groups with similar properties

Left gaps for undiscovered elements

When elements were discovered, they had properties which matched Mendeleev’s predictions

20
Q

why did mendeleevs periodic table become more widely accepted

A

predicted properties of missing elements
elements were discovered
they matched his predictions

21
Q

properties of alkali metals

A

Soft
Low density
Low melting and boiling points
Very reactive
Form white compounds

22
Q

alkali metals reactions with water

A

produce hydrogen and a metal hydroxide solution.

23
Q

alkali metals reactions with oxygen

24
Q

alkali metals reactions with chlorine

25
group halogens
less reactive as you go down less volality less solubility melting and boiling decrease
26
Group 7 Halogens reactions:
The chlorine displaces the bromide as it is more reactive than bromine
27
why is there a higher boiling point
relative formula mass increases so intermolecular forces increase in strength more energy is needed to overcome
28
why do elements in the same group react in a similar way
same number of electrons in the outer shell
29
group 0 chemical properties
Inert (unreactive due to full outer shell). Non-flammable Colourless gases at room temperature. Boiling point increases
30
properties of transition metals
Form ions with different charges Different coloured compounds Used as catalysts Unreactive Strong High density High melting points Hard Good conductors of electricity Good thermal conductors
31