Chemistry Unit Review
Game
Chapter 1
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Anything that has mass and volume is
considered to be???
– Matter
An example of this type of change is a change of
state.
– Physical change
What physical property can be measured
numerically?
– Quantitative properites
Qualitative and Quantitative
Properties
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Which of these properties is not a qualitative
property: ductility, malleability, magnetism,
conductivity, colour?
– Conductivity
What quantitative property is the ability to
dissolve in water?
– Solubility
What qualitative property is the ability to be
beaten into sheets?
- Malleability
Dalton’s Atomic Theory – Main
Points
All matter is made of small particles called
atoms.
 Atoms cannot be created, destroyed, or divided
into smaller particles.
 All atoms of the same element are identical in
mass and size, but are different in mass or size
from the other elements.
 Compounds are created when atoms of different
elements link together in definite proportions.
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Who proposed the “raisin bun” model of
the atom?
A – J.J. Thomson
 Who proposed specific energy levels or
shells for electrons to be found?
A – Niels Bohr
 What was the positive particle that
Rutherford used to shoot through the gold
foil?
A – Alpha particle
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The Atom
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A, B, and C are
considered what?
– Subatomic particles
Which letter refers to
the electron of the
atom?
–A
What type of charge
does B have?
-0
B
C
Which two subatomic
particles are nearly
equal in mass?
A – Protons and
neutrons (B and C)
 What subatomic
particle determines
what element you
have?
A - Protons
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B
C
State the Symbol
NO PERIODIC TABLES
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Gold
– Au
Potassium
–K
Strontium
– Sr
Manganese
- Mn
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Silver
– Ag
Mercury
– Hg
Selenium
– Se
Xeon
- Xe
State the Name
NO PERIODIC TABLES
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Ne
– Neon
W
– Tungsten
Kr
– Krypton
Fe
– Iron
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Ti
– Titanium
Cs
– Cesium
Mg
– Magnesium
Be
Beryllium
An element is found to be malleable and
have a shiny luster. It is considered a …
A – metal
 A new element is found and it is solid,
shiny, decent conductor of heat, and
brittle. What type of element can this be
considered?
A - metalloid
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What is meant by the term “ion charge”?
– the number of electrons an atom may gain or
lose from other atoms.
What particle has to be removed from an atom
so that the atom becomes a positive ion?
– electrons
What kind of ions do elements on the right side
of the periodic table form?
- negative
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What periodic family has a common ion charge
of zero?
– Noble gases
What kind of reactivity will these elements have?
– none, stable, non-reactive
Which family will react more with water – Alkali
metals or Alkaline earth metals?
– alkali metals
What is a valence electron?
A – an electron found in a valence shell
which is the outermost shell for atoms.
 Why is H listed in the same column as the
metals Li, Na, and K even though H is a
non-metal?
A – it want to give away one electron;
therefore, it has the same number of
valence electrons as the alkali family.
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Identify the following atoms:
1. 2,8,3
A – Aluminum
2. 2,8,4
A – Silicon
3. 2,7
A – Fluorine
4. 2,8
A – Neon
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Atomic Numbers and Atomic
Masses
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Atomic # = 78
– Platinum
Atomic # = 72
– Hafnium
Atomic mass = 258
– Mendelevium
Atomic mass = 88
- Radium
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# of e- = 31
– Gallium
# of e- = 63
– Europium
Atomic # = 18
– Argon
Atomic mass = 51
- Vanadium
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What is Ca2+? It’s an
…
– Ion
What is Cl? It’s an …
– Atom
What do the red dots
represent?
– Electrons
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Is the picture to the
right a ionic or
covalent bond?
– covalent
How do you know?
– The electrons are
being shared.
What atoms are
represented here?
– Hydrogen
What is the structure on
the right called?
A – A crystal lattice
 What is the most
common crystal lattice
known?
A – NaCl (salt)
 What type of bonding
produces crystal lattices?
A – Ionic bonding
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How are ionic bonds produced?
A – When a metal and non-metal combine. The
metal gives the non-metal electrons, causing it
to become positive. The non-metal becomes
negative and the positive and negative charges
attract.
 What is a chemical formula?
A – The symbols that show the elements in a
compound and their ratios (relative number of
each element in the compound)
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Ionic Bonds – State the Name
Rubidium is mixed with bromine.
A – rubidium bromide
 Sulphur is mixed with calcium.
A – calcium sulphide
 Cesium is mixed with phosphorus.
A – Cesium phosphide
 Oxygen is mixed with strontium.
A – Strontium oxide
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Ionic Bonds – State the Formula
Lithium combines with fluorine.
A – LiF
 Calcium combines with chlorine.
A – CaCl2
 Silver combines with oxygen.
A – Ag2O
 Scandium combines with sulphur.
A – Sc2S3
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Ionic Bonds – State the Formula
Oxygen combines with calcium.
A – CaO
 Tungsten combines with nitrogen.
A – WN2
 Barium combines with sulphur.
A – BaS
 Zinc combines with bromine.
A – ZnBr2
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Multivalent Ions
Give three examples of multivalent ions.
A – Titanium, vanadium, iron, manganese,
cobalt, nickel, copper, gold, mercury, etc.
 What do we need to do when naming
compounds that contain multivalent ions?
A – Use Roman numerals to indicate the ion
charge for the metal
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Multivalent Ions – State the
Formulas
Copper (II) oxide
A – CuO
 Nickel (III) chloride
A – NiCl3
 Cobalt (III) oxide
A – Co2O3
 Manganese (IV) sulphide
A – MnS2
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Multivalent Ions – State the Name
CrCl3
A – Chromium (III) chloride
 PbO
A – Lead (II) oxide
 SnS2
A – Tin (IV) sulphide
 NiF3
A – Nickel (III) fluoride
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Polyatomic Ions
Give three examples of polyatomic ions.
 How are polyatomic ions bonded?
A – By covalent bonds
 Do polyatomic ions have an ion charge?
A – Yes
 Can polyatomic ions be bonded to metals
in an ionic bond?
A - Yes
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Polyatomic Ions – State the
Formula
Potassium permanganate
A – KMnO4
 Lithium dichromate
A – Li2Cr2O7
 Calcium hydroxide
A – Ca(OH)2
 Magnesium phosphate
A – Mg3(PO4)2
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