Periodicity

Question

Describe the electronegativity and atomic radius trend across a period

Answer 1

The electronegativity decreases across a period The atomic radius decreases across a period

Answer 2

The electronegativity increases across a period The atomic radius decreases across a period

Answer 3

The electronegativity Increases across a period The atomic radius increases across a period

Answer 4

The electronegativity decreases across a period The atomic radius increases across a period

Answer 5

electrical conductivity decreases down a group when they are conductable

Answer 6

electrical conductivity - made possible by ions or electrons that are not free to move

Answer 7

electrical conductivity across a period decreases overall

Answer 8

occurs in covalent bonds

Answer 9

there are higher intermolecular forces between sulphur than phosphorous

Answer 10

there are lower intermolecular forces between sulphur than phosphorous

Answer 11

Ionic radius

Answer 12

Atomic radius

Answer 13

Electronegativity

Answer 14

The atomic radius doesn't affect their nuclear charge

Answer 15

Nuclei distance is difficult to measure

Answer 16

They do not generally bond to other atoms

Answer 17

Cl, Cl-, Cl+

Answer 18

Cl+, Cl, Cl-

Answer 19

Cl-, Cl+, Cl

Answer 20

Cl-. Cl, Cl+

Answer 21

odour, colourless, mono atomic, reactive

Answer 22

odourless, colourless, mono atomic, unreactive

Answer 23

odourless, colour, not mono atomic, unreactive

Answer 24

odour, colour, not mono atomic, reactive

Answer 25

reactivity increases down group, 1 electron in outer shell, form ionic compounds, doesn't conduct electricity, very reactive, low density

Answer 26

reactivity decreases down group, 1 electron in outer shell, form ionic compounds, doesn't conduct electricity, very reactive, low density

Answer 27

reactivity increases down group, 1 electron in outer shell, form ionic compounds, conducts electricity, very reactive, low density

Answer 28

reactivity increases down group, 2 electron in outer shell, doesn't conduct electricity, very reactive, low density

Answer 29

Na, Mg - alkaline

Answer 30

Al - amphoteric

Answer 31

Si, P, S, Cl - alkaline

Answer 32

Si, P, S, Cl - acidic

Answer 33

Na, Mg - acidic

Answer 34

Na -----> Al = steady increase as there is an increase in the availability of electrons in the metallic bonding

Answer 35

Si = massive increase since Si has a giant macromolecular structure

Answer 36

P = slight increase due to as have only van der Waals forces between molecules whereas the others have giant structures; P4 molecule

Answer 37

S = small increase as have only van der Waals forces between molecules whereas the others have giant structures; S8 molecule

Answer 38

P= large decrease as have only van der Waals forces between molecules whereas the others have giant structures; P4 molecule

Answer 39

Cl ---> Ar = decrease as chlorine is a much smaller molecule with weaker van der Waals forces; argon is just a single atom = very weak van der Waals forces

Answer 40

P4O10 (or P4O6)

Answer 41

SO3 (or SO2)

Answer 42

Cl2O7 Cl2O

Answer 43

SO3 (OR SO2)

Answer 44

P4O10 (OR P4O6)

Answer 45

Cl2O7 Cl2O

Answer 46

1st Ionisation Energy = minimum energy required to remove 1 mole of gaseous electrons from 1 mole of gaseous atoms Electronegativity = ability of an atom to attract electrons in a ionic bond

Answer 47

1st Ionisation Energy = minimum energy required to remove 1 mole of gaseous electrons from 1 mole of gaseous atoms Electronegativity = ability of an atom to attract electrons in a covalent bond

Answer 48

Variable oxidation number

Answer 49

complex ion formation

Answer 50

Catalyst properties

Answer 51

Coloured complexes

Answer 52

Sc not transition metal as its common ion Sc³⁺ has no d electrons

Answer 53

Zinc not transition metal as contains full d sub level in all oxidation states

Answer 54

Zinc not transition metal as contains has no full d sub level in all oxidation states

Answer 55

Species that uses a lone pair of electrons to form dative covalent bonds with a non-metal ion.

Answer 56

Species that possesses an incomplete or sub-level in one or more of its oxidation states

Answer 57

Species that uses a lone pair of electrons to form dative covalent bonds with a metal ion.

Answer 58

Species which is the arrangement showing the properties of elements repeat periodically

Answer 59

energy difference between levels corresponds to particular wavelength of light

Answer 60

because they are

Answer 61

colour produced complement to wavelength absorbed when electrons excited.

Answer 62

electron transitions (electron jumps) from one orbital to another

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Periodicity

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Resumen del Recurso

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