periodicity 8 Flashcards

1
Q

periodic table

A

order of increasing atomic number

can predict the properties depending on its position

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2
Q

groups

A
  • the vertical column of elements
  • similar chemical properties
  • same number of electrons
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3
Q

reactivity

A

s-block metals = get more reactive going down the group

transition metals = non-reactive

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4
Q

periods

A

-horizontal rows

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5
Q

placing hydrogen

A

-forms a 1+ ion but not chemically similar and is also a gas

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6
Q

placing helium

A

-not a p-block element 1S2

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7
Q

group 1,2,3 elements bonding

A

giant structure
ionic compounds
metallic bonding

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8
Q

group 4 elements bonding

A

four covalent bonds (giant covalent)

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9
Q

group 5,6,7 elements bonding

A

non-metals

covalent bonds

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10
Q

group 0 (8) element bonding

A

noble gas
full outer shell
unreactive

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11
Q

melting and boiling point

A

1 - group 4
2- group 3,2,1
3- group 6,5,7
4-group 8

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12
Q

atomic radii

A

taken to be half the distance between the centres of a pair of atoms

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13
Q

the size of the atom ……. going across a period

A

decrease

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14
Q

radii of the atoms increase down a group

A

going down a group an extra shell of electrons are added, the electron is further away from the nucleus

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15
Q

why does the first ionisation energy increase across a period

A

a number of protons in the nucleus increases but the electrons enter the same shell. so it gets increasing difficult to remove an electron

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16
Q

why does the first ionisation energy decrease going down a group

A

the number of filled inner shells increase down the group, this means that there is an increase in shielding.
the electron is further away from the nucleus so it’s easier to remove

17
Q

why there is a drop in ionisation energy from one period to the next

A

the new main level starts and so there is an increase in atomic radius, the outer electron is further from the nucleus so less strongly attracted to its easier to remove

18
Q

drop in first ionisation energy between group 2 and 3

A

p-electron is already in a higher energy level than the s-electron, so it takes less energy to remove it

19
Q

drop in first ionisation energy between groups 5 and 6

A

an electron in a pair will be easier to remove that one in an orbital on its own because it is already being repealled by the other electron

20
Q

Bonding ( period 3)

A

Metallic - Na, Mg,Al
Giant covalent - Si
Covalent - P,S,Cl,Ar

21
Q

Structure ( period 3)

A

Giant metallic - Na,Mg,Al
Giant covalent - Si
Molecular - P4, S8, Cl2
Noble gas - Ar

22
Q

Atomic radii

A

Tells us the size of the atoms
Half the distance between the centres of a pair of atoms is used
Radius differs depending on what type of bonding
Decreases across a period ( theres a jump when starting the next period)

23
Q

Why the radii of atoms decrease across a period

A

Add a proton ( increase nuclear charge)
Increased charge pulls the electron in closer to the nucleus
No more shielding from next shells

24
Q

First ionisation energies

A

The enrgy required to convert 1 mole of gaseous ions into one mole of +1 gaseous ions

25
Q

first ionisation energy increases across a period

A

because more protons are added to the nucleus however no more shells are adding meaning there is no extra shielding. therefore it is harder to move an electron so the ionisation energy is more

26
Q

first ionisation energy drops as you go down a group

A

there is an increase in atomic radius and the outer electron is further away from the positive nucleus and so is easier to remove

27
Q

periodicity

A

the regular recurrence of the properties of elements when they are arranged in atomic number order as the periodic table

28
Q

classification

A

An element is classi ed as s, p, d or f block according to its position in the Periodic Table, which is determined by its proton number