Day 5 - Chemical Compounds and Bonding

Think about how much of the course you have covered. Well done to all students for completing week one. On Monday there is a quiz for Chapter 3.

Today's work: Chapter 3 - Compounds

Reading Check Pg 83 # 1 - 9

We practiced naming and writing some of the formulae on pages 86 - 91

Pg 95 # 1, 2abc, 3abcgh, 5abgh, 6abgh

Pg 97-99 (read only, just skim it).

Pg 106-107 Chapter 3 Review # 1 - 20 (#14 - 20 only do a +b for each question)

This weekend it is really important to study all your quizes and daily assignments as I am planning to give a Unit Test on Chapters #1-3 on Tuesday.

This is a good resource on different kinds of bonding and Van Der Waal Forces.

Chapter 2 Quiz Answers
1. C
2. B
3. C
4. B
5. C
6. D
7. C
8. A
9. D
10. A
11. F
12. G
13. B
14. H
15. D
16. A

PG 83 # 1 - 9

Checking Concepts

1. A chemical bond is a link between two atoms

that holds the atoms together.

2. Covalent and ionic

3. In a covalent bond, atoms are connected by

sharing a pair of electrons.

4. In an ionic compound, positive ions and nega-

tive ions are attracted to each other through

their opposite electric charges.

5. When a sodium atom loses an electron, it

becomes positively charged. When a chlorine

atom gains an electron, it becomes negatively

charged. All the negative charges repel each

other but attract the positive charges.

This results in an alternating arrangement

inside a crystal lattice.

6. (a) Lithium forms a positive ion, whereas fluo-

rine forms a negative ion.

(b) Li+and F–

7. (a) Two

(b) One

8. (a) Carbonate, CO

32–

(b) Phosphate, PO

43–

(c) Ammonium, (NH

4+) and nitrate, (NO3–)

9. (a) Covalent

(b) Four

(c) Polyatomic ion

PG 95 Checking Concepts

1. (a) Two

(b) The first part names the positive ion, while

the second part names the negative ion.

2. (a) Lithium, positive ion

(b) Nitrate, negative ion, polyatomic ion

(c) Iron(III), positive ion, multivalent metal

(d) Acetate, negative ion, polyatomic ion

(e) Chromium(II), positive ion, multivalent

metal

(f) Chloride, negative ion

(g) Perchlorate, negative ion, polyatomic ion

(h) Ammonium, negative ion, polyatomic ion

3. (a) Chromate, 1 chromium atom, 4 oxygen

atoms, 5 atoms in total, charge of 2–

(b) Dichromate, 2 chromium atoms, 7 oxygen

atoms, 9 atoms in total, charge of 2–

(c) Ammonium, 1 nitrogen atom, 4 hydrogen

atoms, 5 atoms in total, charge of 1+

(d) Acetate, 2 carbon atoms, 3 hydrogen

atoms, 2 oxygen atoms, 7 atoms in total,

charge of 1–

(e) Hydrogen sulphate, 1 hydrogen atom, 1

sulphur atom, 4 oxygen atoms, 6 atoms in

total, charge of 1–

(f) Sulphate, 1 sulphur atom, 4 oxygen atoms,

5 atoms in total, charge of 2–

(g) Sulphite, 1 sulphur atom, 3 oxygen atoms,

4 atoms in total, charge of 2–

(h) Sulphide, 1 sulphur atom, 1 atom in total,

charge of 2– (f) Mn

3P2

(g) Chromium(II) fluoride

(h) Copper(I) iodide

(i) Manganese(II) sulphide

(j) Lead(IV) oxide

(k) Tin(IV) oxide

(l) Chromium(II) nitride

6. (a) Magnesium hydroxide

(b) Potassium sulphate

(c) Aluminum hydrogen carbonate

(d) Copper(I) carbonate

(e) Iron(II) permanganate

(f) Ammonium sulphate

(g) Na 2SO4

(h) Ca 3(PO4)2

(i) Al(NO 3)3

(j) NH 4HSO4

(k) Pb(ClO3)4

(l) Fe2(CO3)3

PG 106 - 107

1. In an element, only one type of atom is pres-

ent. In a compound, atoms or ions from two

or more different elements are chemically

combined.

2. (a) Ionic and covalent

(b) In ionic compounds, one or more electrons

transfers between atoms, producing posi-

tive and negative ions. These ions are

attracted together because of their opposite

charges. In covalent compounds, two

atoms share the same pair of electrons, and

this sharing acts as a bond to hold them

together.

3. (a) Students’ drawings may vary but could

include either of the following:

Checking Concepts

1. In an element, only one type of atom is pres-

ent. In a compound, atoms or ions from two

or more different elements are chemically

combined.

2. (a) Ionic and covalent

(b) In ionic compounds, one or more electrons

transfers between atoms, producing posi-

tive and negative ions. These ions are

attracted together because of their opposite

charges. In covalent compounds, two

atoms share the same pair of electrons, and

this sharing acts as a bond to hold them

together.

3. (a) Students’ drawings may vary but could

include either of the following:

(b) The covalent bond is represented by the

“sticks” connecting the balls together or

the shared pair of electrons.

4. It is possible to keep dividing water by separat-

ing molecules until there is only one left. If a

molecule is broken up, this is a chemical

change and produces new substances with new

properties. This makes a single water molecule

the smallest possible sample of water.

5. Two neighbouring water molecules are not

covalently bonded. The covalent bonds exist

only between atoms of the same molecule.

6. All positive ions in an ionic lattice are

attracted to all other negative ions anywhere

in the lattice. However, the attraction

decreases with distance, and most of the

attraction is to the nearest negative ions.

7. (a) 2 chromium atoms and 7 oxygen atoms

(b) 2–

8. (a) Ionic

(b) Ionic

(c) Covalent

(d) Covalent

(e) Ionic

9. If the same chemical name applied to more

than one compound, this would lead to confu-

sion about which chemical is being referred to.

10. (a) International Union of Pure and Applied

Chemistry

(b) One important responsibility is to develop

rules for naming compounds.

11. (a) A reactant is a starting material in a chemi-

cal reaction. The reactant gets used up

during the reaction.

(b) A product is a material that is made during

a chemical reaction. The reactants turn

into products.

12. In an exothermic change, there is an overall

release of energy from the system. Often, this

means the reaction system warms up. In an

endothermic change, there is an overall

absorption of energy by the system as energy

flows into it.

Understanding Key Ideas

13. The carbonate ion CO

32–is like a molecule

because the carbon and three oxygen atoms

are covalently bonded to each other. It is like

an ion because the group of atoms carries an

electric charge of 2–.

14. (a) Sodium iodide

(b) Magnesium nitride

(c) Zinc oxide

(d) Aluminum fluoride

15. (a) Potassium nitride

(b) Calcium sulphide

(c) Silver sulphide

(d) Aluminum phosphide

(e) Strontium nitride

(f) Cesium oxide

16. (a) KBr

(b) K2O

(c) CaO

(d) Al2O3

(e) AlCl3

(f) Al2S

17. (a) Chromium(III) chloride

(b) Chromium(II) chloride

(c) Iron(II) chloride

(d) Iron(III) oxide

(e) Gold(I) oxide

(f) Gold(III) oxide

18. (a) FeF2

(b) FeF3

(c) CuF

(d) Cu2O

(e) CuO

(f) SnO2

19. (a) Ammonium phosphide

(b) Ammonium phosphite

(c) Ammonium phosphate

(d) Sodium phosphate

(e) Magnesium phosphate

(f) Iron(II) carbonate

20. (a) Na 2SO4

(b) Ca(NO3)2

(c) Al(OH)3

(d) Sr(HSO 4)2

(e) NH 4HSO4

(f) Ni(ClO )ionic compound

Day 3 - Elements

Today we wrote a quiz, #1-16 and all marks count.

Homework today is:

1.) Read pgs 43 - 47 and complete #1-5 on page 47

2.) Checking concepts Pg 51 #1-4, #6-13

3.) Read pages 52 - 57, 60 -61 and do questions #1-21 on page 63


A good reference to review what you have learned about elements can be found here.

Answers:


Reading Check Answers, p. 47
1. Unlike iron, sodium melts at a low temperature,
is soft, and is highly reactive in water.
2. Iron is strong and can be made stronger by
adding carbon.
3. Mercury is the only metal that is liquid at
room temperature.
4. Chlorine is added to water to kill bacteria.
Chlorine also combines with sodium to make
table salt.
5. Silver can be polished and moulded and is
both malleable and ductile, making it useful
for jewellery. Its conductivity makes it useful
in electronics.

PG 51


1. (a) An element is a substance made up of only
one type of atom. More precisely, all atoms
of the same element have the same number
of protons.
(b) There are about 92 naturally occurring
elements (about 115–120 elements in
total).
2. Chemical symbols allow scientists to communicate
about elements in a way that is understood
by scientists all over the world.
3. (a) Hydrogen, nitrogen, oxygen, fluorine
(b) Bromine, mercury
(c) Answers may vary. Sample answer: potassium,
carbon, phosphorus, sulphur, iodine.
(d) Answers may vary. Sample answer: lithium,
sodium, rubidium, cesium.
4. Any two of strontium, magnesium, copper
6. Hydrogen
7. Silver
8. Iron and carbon make steel. Other metals are
usually added in as well.
9. The atmosphere is about 21% oxygen.
10. Oxygen in our atmosphere was produced by
plants over the past 3 billion years.
11. Sodium metal reacts violently with water,
making it unsuitable for use in drinking
glasses.
12. Chlorine in swimming pools is effective at
killing bacteria and other pathogens in the
water.
13. Hydrogen makes up more than 90% of the
atoms in the universe.
14. Silicon combines with oxygen to make sand.



Checking Concepts Pg. 63

1. The periodic table is a chart that organizes the
elements according to their physical and
chemical properties.
2. Atomic number = number of protons in each
atom of the element
3. Atomic number
4. (a) 2
(b) 8
(c) 26
(d) 79
(e) 92
(f) 101
5. An atom of potassium
6. Atomic mass is the mass of an atom of an element.
7. Atomic mass units
8. Atomic mass generally increases from left to
right and from top to bottom through the
table.
9. (a) 6.9 amu
(b) 28.1 amu
(c) 55.8 amu
(d) 63.5 amu
(e) 200.6 amu
10. Lead
11. Ion charge is an electric charge that forms on
an atom when it gains or loses electrons.
12. An electron
13. (a) Positive
(b) Negative
14. These elements do not form ions.
15. The element is capable of forming an ion in
more than one way.
16. (a) 2+, 3+, and 4+
(b) 2+
17. Metals, non-metals, and metalloids
18. (a) Alkali metals, alkaline earth metals, halogens,
and noble gases
(b) Alkali metals and alkaline earth metals
(c) Halogens and noble gases
19. Any five of boron, silicon, germanium, arsenic,
antimony, tellurium, polonium, and astatine
20. Periods
21. Families or groups