Structure 1. Models of the particulate nature of matter

1.1 Introduction to the particulate nature of matter

1.2 The nuclear atom

1.3 Electron configurations

1.4 The mole

1.5 Ideal gases

Structure 2. Models of bonding and structure

2.1 The ionic model

2.2 The covalent model

2.3 The metallic model

2.4 From models to materials

Structure 3. Classification of matter

3.1 The periodic table

3.2 Functional groups: Organic compounds

Reactivity 1. What drives chemical reactions?

1.1 Measuring enthalpy changes

1.2 Energy cycles

1.3 Energy from fuels

Reactivity 2. How much, how fast and how far?

2.1 Amount of chemical change

2.2 Rate of chemical change

2.3 Extent of chemical change

Reactivity 3. What are the mechanisms of chemical change?

3.1 Proton transfer reactions

3.2 Electron transfer reactions

3.3 Electron sharing reactions (Radicals)

3.4 Electron-pair sharing reactions

IB Chemistry HL 2.1 The ionic model Question Bank

[Maximum number: 2]

There are many oxides of silver with the formula $\mathrm{Ag}_{x} \mathrm{O}_{y^{.}}$ All of them decompose into their elements when heated strongly.

(a)

(i)

Explain the electrical conductivity of molten $\mathrm{Na}_{2} \mathrm{O}$ and $\mathrm{P}_{4} \mathrm{O}_{10}$ .

[ 2 ]

[Maximum number: 2]

A powder has the following percentage composition by mass:
30.0 % sucrose, $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$
45.0 % citric acid, $\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}$
25.0 \% sodium hydrogencarbonate, $\mathrm{NaHCO}_{3}$

In the presence of water, the powder effervesces as the citric acid reacts with the sodium hydrogencarbonate:

$3 \mathrm{NaHCO}_{3}(\mathrm{~s})+\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}(\mathrm{aq}) \rightarrow \mathrm{Na}_{3}\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)(\mathrm{aq})+3 \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$

(a)

Describe the bonding in solid sodium citrate.

[ 2 ]

[Maximum number: 1]

Two groups of students (Group A and Group B) carried out a project* on the chemistry of some group 7 elements (the halogens) and their compounds.

(a)

Group B heated the yellow solid, $\mathrm{CsICl}_{2}(\mathrm{~s})$ , which turned white and released a brown gas which condensed into a brown liquid.

Group B identified the white solid as CsCl(s). Suggest the identity of the brown liquid.

[ 1 ]

[Maximum number: 1]

Iron(II) sulfide can be produced by heating powdered iron and sulfur together.

(a)

Contrast one physical property of iron and iron(II) sulfide.

[ 1 ]

[Maximum number: 2]

Iron may be extracted from iron (II) sulfide, FeS.

(a)

Iron (II) sulfide, FeS, is ionically bonded.

[ 2 ]

(i)

Describe the bonding in this type of solid.

[ 2 ]

[Maximum number: 1]

Titanium and vanadium are consecutive elements in the first transition metal series.

(a)

(i)

State the type of bonding in potassium chloride which melts at 1043 K .

[ 1 ]

[Maximum number: 1]

Nitric acid, $\mathrm{HNO}_{3}$ , is a strong acid.

(a)

(i)

Write the formula of nickel(II) nitrate.

[ 1 ]

[Maximum number: 1]

In which of the following compounds does ionic bonding predominate?

HCl

NaF

$\mathrm{NH}_{4} \mathrm{Br}$

NaOH

[Maximum number: 1]

Which combination would create the strongest ionic bond?

lonic radius

Charges on ions

large

high

large

low

small

high

small

low

[Maximum number: 1]

Which is an ionic compound?

$\mathrm{Mg}_{3} \mathrm{~N}_{2}$

$\mathrm{Al}_{2} \mathrm{Cl}_{6}$

$\mathrm{SiO}_{2}$

$\mathrm{SF}_{6}$

0 selected

Question 1

Question 1(c)

Question 1(c)(ii)

Question 1

Question 1(d)

Question 1

Question 1(d)

Question 1

Question 1(c)

Question 1

Question 1(d)

Question 1(d)(i)

Question 2

Question 2(g)

Question 2(g)(i)

Question 2

Question 2(b)

Question 2(b)(ii)

Question 9

Question 9

Question 9