Additional Test Review for this weekend:
• p. 288 – 291 1-24. 34-36, 42, 55, 56, 57, 63, 64, 65,
• p. 250 – 251 #1-10, 12, 13, 14, 19, 20
Remember to use your notes to answer questions.
Check your answers with the back of the book.
p. 248 #1-7, 10, 13, 14, 15, 19
2. What is the significance of the bold staircase line on the periodic
table?
The bold staircase separates the metals from the non-metals. Along
the staircase are the metalloids.
3. Dmitri Mendeleev designed the periodic table. Elements were
originally organized according to atomic mass. The modern periodic
table organizes elements in order of increasing atomic number.
4. See above.
5. Explain the difference between the following:
 An element is a pure substance made of one type of atom.
 A compound is a pure substance made of 2 or more different
atoms chemically combined.
 A group is a vertical column in the periodic table.
 A row is a horizontal row in the periodic table.
 A metal is an element that is usually silver, solid at room temp.
conducts heat and electricity, is malleable, ductile and lustrous.
 A non-metal exists in different colours and states, does not
conduct electricity and heat and is not malleable, ductile or
lustrous.
 A proton is a positively charged particle. A neutron is a neutral
particle and has no charge.
They are both found in the nucleus.
 An electron is a negatively charged particle found outside the
nucleus in energy shells.
 The atomic number represents the number of protons in an atom.
 The mass number represents the number of protons and neutrons
in an atom.
6. Explain the similarities and differences between the plum pudding
model and the Bohr model of the atom.
Plum Pudding (Thompson) – believed that the atoms contained
negatively charged electrons found throughout a positively charged
atom.
Bohr found evidence to support that electrons orbited the nucleus of
the atom like planets orbit the sun. Each orbit holds a certain number
of electrons.
7. What did the surprising results of Rutherford’s gold foil experiment
prove?
In Rutherford’s experiment some of the positively charged particles
were deflected from the piece of gold foil. This was surprising because
it proved that a strong positive charge in the gold atoms must be
repelling the positive particles. Rutherford suggested that the atom
must have a strong positive central mass. This was called the nucleus.
9. JJ Thomson’s evidence that the atom contains particles that are
negatively charged:
10.
***11.
13. Elements in the same family (alkaline Earth Metals – silver,
lustrous, reactive)
Elements in the same period have the same number of energy shells.
Elements in the family of noble gases are gases, odourless, colourless
and inert (unreactive).
14. Maximum number of electrons –
a) 2, 8, 8
b)
15. The alkali metals are highly reactive. This is because they have 1
valence electron. In order to become stable they only have to lose 1
valence electron which happens easily making them highly reactive.
Halogens have 7 valence electrons. To become stable Halogens gain 1
electron. This happens easily making them highly reactive.
Noble gases have 2 or 8 valence electrons. Since they have a full set of
electrons they don’t need to gain or lose electrons and are inert
(unreactive).
19. Thinking
The most reactive solid is C (bubbled vigorously).
The least reactive is B (no change).
I think these elements are Metals because they have metallic lustre. I
think these elements belong in group 2, the Alkaline Earth Metals.
Solid B did not react with water or acid. All alkali metals are reactive
with water, therefore these elements cannot belong to Group 1, the
Alkali Metal group. Solid A and C did react with water and/or acid
showing that these elements are reactive. Alkaline Earth Metals are
not as reactive as Alkali Metals.
Reactivity increases as you move down a metallic family. Solid B did
not react at all and is the least reactive. It would be the highest in the
family. Solid A would be next, and Solid C would be at the bottom
because it reacted with water and acid making it the most reactive.
p. 282 #1-7, 9, 10, 11, 13, 14, 15, 20, 22
6. Ozone is a diatomic molecule. (F – has 3 atoms not 2).
7. Nonmetals react with other non-metals to form ionic compounds.
(F)
9. Propane, butane and pentane all belong to the class of organic
compounds called hydrocarbons.
10. All the bonds in methanol are covalent bonds.
11. An ion is formed when an atom loses one or more electrons and
retains the same number of protons.
13. Noble gases are the most stable elements because they have a full
set of valence electrons. They don’t need to gain or lose electrons to
become stable.
14. All molecules are not considered compounds because some
molecules are elements. Many elements exist as molecules such as O2,
H2, Cl2. These are called diatomic molecules because they exist as 2
atoms bonded together.
15. Potassium + Chloride – Ionic Compound (metal and non-metal –
metal loses electron and non-metal gains electron) See your notes to
see how we draw the bohr Rutherford diagram.
b) A chloride ion has 17 protons, how many electrons does it have?
Chlorine is element number 17, therefore it has 17 electrons and
protons. If it is an ion, it has gained an electron and therefore has 18
electrons.
c) A potassium ion has 19 protons, how many electrons does it have?
Potassium is an alkali metal and therefore loses an electron. This
means that it has 18 electrons and a charge of positive 1.
20. Beryllium and Fluorine make an ionic compound. How do we
know?
Beryllium is a metal and Fluorine is a non-metal. To make this
compound you need 1 Beryllium atom and 2 Fluorine atoms.
a) Identify one material that oxygen reacts with rapidly. Iron/steel.
b) Chlorine gas is a molecular compound because it consists of 2
nonmetals.