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chemistry > INORGANIC - MOCKS > Flashcards

INORGANIC - MOCKS Flashcards

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1
Q

what is periodicity?

A

regularly repeating pattern of atomic, physical and chemical properties with increasing atomic number

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2
Q

four blocks on the periodic table?

A

S = gp 1 + 2

d = transition

p = rhs

f = bottom

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3
Q

why does the first ionisation energy generally decrease down a group?

A

more shells

more shielding

easier to lose outer electron

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4
Q

why does Si have such a high melting/boiling point?

A

giant covalent structure
all silicon atoms held together with strong covalent bonds
require lots of energy to overcome

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5
Q

definition of first ionisation energy

A

energy required to remove one outer electron from one mole of gaseous atoms to produce one mole of gaseous ions with a 1+ charge

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6
Q

why does the first ionisation energy generally increase across period 3?

A

increasing nuclear charge
same shielding
stronger electrostatic attraction between outer electrons and nucleus so harder to remove the outer electron

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7
Q

why does the 1st ionisation energy in period 3 fall at ALUMINIUM?

A

aluminium outer electron = in 3p rather than 3s

higher energy level
slightly more distant from nucleus
partially screened by 3s electrons too

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8
Q

why does the first ionisation energy in period 3 fall at SULFUR?

A

in sulfur the electron is being removed from a PAIR

repulsion between two electrons in same orbital

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9
Q

why does melting point generally decrease down group 2?

A

more shielding
electrons in sea of delocalised electrons further from nucleus
metallic bond strength decreases

(Mg = lowest but no simple explanation)

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10
Q

how does the reaction with water change down the group?

A

gets more vigorous down the group

eg - M(s) + 2H2O(l) —- M(OH)2(aq) + H2(g)

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11
Q

reaction of magnesium with cold water + with steam

A

Mg and cold water —- very slow reaction

Mg and steam —- very rapid reaction - forms magnesium OXIDE
and hydrogen

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12
Q

trend in solubility of group 2 hydroxides down the group?

A

down group = more soluble

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13
Q

use of Mg(OH)2 (almost insoluble)

A

indigestion tablets

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14
Q

trend in solubility of group 2 sulfates down group 2?

A

become LESS soluble down the group

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15
Q

how can barium sulfate be used in medicine?

A

barium meal to outline the gut in medical x-rays

barium = highly toxic but BaSO4 is v insoluble so is safe

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16
Q

using barium sulfate to test for sulfate ions in solution?

A
  • solution first acidified with nitric / hydrochloric acid
  • barium chloride solution added
  • if a sulfate is present a white precipitate of BaSO4 will form
17
Q

trend in oxidising ability up the halogens?

A

oxidising ability of halogens INCREASES UP THE GROUP

18
Q

reaction between chlorine and bromide ions

A

Cl2 + 2KBr —— Br2 + 2KCl

  • bromine is formed so red-brown solution
  • chlorine = oxidising agent
19
Q

equation for formation of bleach - NaClO

A

2NaOH + Cl2 —— NaClO + NaCl + H2O

20
Q

what type of reaction is the formation of bleach?

A

disproportionation

the OS of Cl increases and decreases as it is both oxidised and reduced

21
Q

trend in halides as reducing agents?

A

reducing ability increases down the group

22
Q

reaction of chloride ions with SULFURIC ACID?

add halide as a salt

A

NaCl + H2SO4 ——- NaHSO4 + HCl

HCl = misty white fumes

NaHSO4 = sodium hydrogen sulfate + made in all these reactions

23
Q

reaction of fluoride ions with sulphuric acid?

A

NaF + H2SO4 —- NaHSO4 + HF

HF = misty white fumes

24
Q

reaction of bromide ions with sulfuric acid

two reactions

A

NaBR + H2SO4 —– NaHSO4 + HBr (misty white fumes)

HBr = better reducing agent so reacts again with H2SO4

2HBr + H2SO4 —— Br2 + SO2 + 2H2O

25
Q

reaction between iodide ions and sulfuric acid

A

NaI + H2SO4 —– NaHSO4 + HI

2HI + H2SO4 —- I2 + SO2 + 2H2O

6HI + SO2 —– H2S + 3I2 + 2H2O

26
Q

describe the test for halides

A

+ nitric acid - HNO3 (to remove unwanted carbonate ions)

+ silver nitrate - AgNO3

27
Q

results when testing for halide ions with

nitric acid + silver nitrate?

A

Cl- white ppt

Br- cream ppt

I- yellow ppt

28
Q

testing further for halide ions after adding HNO3 and AgNO3?

A

add ammonia NH3

AgCl will dissolve in DILUTE NH3

AGBr will dissolve in CONCENTRATED NH3

AgI won’t dissolve in NH3

29
Q

basic trend in oxidising in gp 7

A

a halogen will displace a halide from a solution if it is below it in the periodic table

30
Q

what is meant by the thermal stability of the halides?

A

how easily a hydrogen halide is broken up into its constituent elements when heated

31
Q

why does the thermal stability of the halides decrease down the group?

A

down group, covalent bonds are weaker and can be broken more easily upon heating

chemistry (9 decks)

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