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Chemistry > PERIODICTY > Flashcards

PERIODICTY Flashcards

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1
Q

Are noble gases hard to remove electrons and why?

A

Yes, full electron configuration

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2
Q

explain the trend in reactivity of the halogens

A

reactivity decreases down the group, as atomic radius increase (more electron shells), attraction of nucleus on electron decreases (electron affinity decreases)

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3
Q

describe the bonding in metals and explain their malleability

A

electrostatic attraction between a lattice of positive ions/cations and delocalised/sea of electrons

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4
Q

3 characteristic properties of transition elements

A

variable oxidation numbers/valency
if ions they form complex
form coloured COMPOUNDS/IONS
catalytic behaviour

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5
Q

what is the easiest group to remove electrons from?

A

Group 1

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6
Q

what do oxidising agents do?

A

Gain electrons (reduced)

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7
Q

the oxide that metal creates, are they acidic or basic?

A

Basic

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8
Q

what must all ligands contain?

A

a non-bonding pair of electrons

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9
Q

what is “Electron affinity”

A

The energy change when one mole of electrons is added to one mole of gaseous atoms to form one mole of gaseous ions.

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10
Q

ionisation energy (IE)

A

is the amount of energy required to remove one mole of electrons from one mole of atoms of an element in the gaseous state to form one mole of gaseous ions.

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11
Q

draw out the period table relationships
this includes:
atomic radius
ionisation energy
electronegativity
electron affinity

A

on ipad

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12
Q

Properties of non-metals and metals
include:
density, ionisation energy
electronegativity values
cations or anions
reducing and oxidising
what types of bonds with non-metals
basic or acidic oxides

A

metals:
high density
low ionisation energies
low electronegativity values
lose electrons to form positive cations
behave as reducing agents (undergoes oxidation)
form ionic bonds with non-metals
form basic oxides
non-metals:
low density
high ionisation energies
high electronegativity values
gain electrons to form negative ions (anions)
behave as oxidising agents (undergo reduction)
form covalent bonds with other non-metals
form acidic oxides

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13
Q

properties of metalloids

A

moderate density, intermediate ionisation energies, intermediate electrical conductivity, amphoteric or weakly acidic oxides

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14
Q

what is effective nuclear charge

A

is the net positive charge experienced by valence electrons
Z(eff) = Z atomic number - S number of shielding electrons

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15
Q

does Z eff decrease or increase across a period (left to right)

A

increase

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16
Q

what does Z eff do when doing down a group

A

Stays the same

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17
Q

what is electron negativity

A

Electronegativity is the ability of an atom to attract a pair of electrons towards itself in a covalent bond.

18
Q

size of cation, atom and anion compare

A

cation < atom < anion

19
Q

outline 2 reasons why electronegativity increases across period 3 in the periodic table and 1 reason why noble gases are not assigned electronegativity numbers

A
  1. because atomic radius decreases
  2. nuclear charge increases (number of protons)
  3. Nobel gases have full valence electron shell
20
Q

What causes transition metals to have colour?

A

electron transition between d-orbitials

21
Q

the ___ the ligand is in the electrochemical series, the ____ the splitting of the d orbitals

A

the HIGHER the ligand is in the electrochemical series, the GREATER the splitting of the d orbitals

22
Q

Left to right on the periodic table, does it go basic to acidic or acidic to basic?

A

basic to acidic (think of H2SO4 as it is acidic)

23
Q

what is periodicity?

A

repeating patterns of physical and chemical properties

24
Q

describe the structure of a complex ion

A

A complex ion consist of a central metal ion bonded to ligands by coordinate covalent bonds

25
Q

define the term ligands

A

a ligand is a species with a lone pair of electrons that forms an coordinate bond to the central central metal ion. Ligands can be negative
ions (CN-1) or neutral molecules (NH3).

26
Q

how does a coordinate covalent bond differ from a conventional covalent bond

A

In a coordinate covalent bond, both electrons in the bond comes
from one atom. In a conventional covalent bond, each atom
supplies one electron in the bond.

27
Q

explain how ligands are also able to act as a lewis base

A

Ligands have lone pairs of electrons, therefore they can act as
Lewis bases. The central metal ion is classed as the Lewis acid.

28
Q

what is diamagnetic

A

when you have no unpaired electrons in the d orbitals

29
Q

what is paramagnetic

A

when you have unpaired electrons in the d orbitals

30
Q

what is the charge on ligand:
H2O
NH3
CN
Cl
SO4

A

H2O = 0
NH3 = 0
CN = -1
Cl = -1
SO4 = -2

31
Q

4 ligands is…

A

Square planar or tetrahedral

32
Q

can cations be ligands

A

no

33
Q

what is the product of Cl2 + H2O

A

HCl + HOCl

34
Q

the halogen at the ___ of the group _____ the halide ____

A

the halogen at the top of the group displaces the halide below

35
Q

a higher electronegativity correlates with higher… and what does it usually involve?

A

boiling and melting points, intermolecular forces

36
Q

Suggest why the colour of [Fe(NH3)6]3+ is different from the colour of [Fe(H2O)6]3+

A

the only diff is the ligand. NH3+ has a higher charge density than H2O so as it approaches the ion it creates a larger split in the d-orbital electrons and a lower wavelength is absorbed

37
Q

Suggest why the colour of [Fe(NH3)6]2+ is different from the colour of [Fe(H2O)6]3+

A

The oxidation number. a different number of d electrons. Fe 3+ has the higher oxidation number so shorter wavelength is absorbs and a larger energy difference

38
Q

suggest why the colour of [Cr(H2O)6]3+ is different from the colour of [Fe(H2O)6]3+

A

the only diff is the central metal ion thus Fe has a higher nuclear charge than Cr/ Ligands interact more effectively with the d-orbitals of an ion with higher nuclear charge thus a shorter wavelength is absorbed and a larger energy diff between Fe and Cr.

39
Q

Explain why Fe2+(aq) is coloured and can behave as a reducing agent, whereas Zn2+(aq) is not coloured and does not behave as a reducing agent.

A

Zn2+ ion has a full 3d orbital, is not a coloured transition metal. Fe2+ does not have full 3d orbitals.

40
Q

what does charge density influence?

A

spin and creates a larger spilt. The bigger the charge density the bigger the split and spin.

Chemistry (3 decks)

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