Egyptian American International School
Science Department
Grade 10 Chemistry
2015 – 2016
The exam includes the following:
PART A: 20 Multiple Choice questions (1 point each)
PART B: 5 COMPLETE (1 point each)
PART C: 10 MATCHING (1 point each)
PART D: 5 TRUE OR FALSE (1 point each)
PART E: 5 SHORT ESSAY (2 points each)
PART F: BONUS (2.5 points)
The exam includes:
Chapter 2: Matter
2.1 The Nature of Matter
VOCAB
Matter
Molecule
Liquid
Atoms
Elements
Gas
Compounds
Solid
Main Idea
 Matter has mass and occupies space. It is composed of tiny particles called atoms.
 Matter exists in three states:
Solid—is a rigid substance with a definite shape
Liquid—has a definite volume but takes the shape of its container
Gas—takes the shape and volume of its container
 Elements contain only one kind of atom—elemental copper contains only copper atoms, and elemental gold contains only
gold atoms.
 Compounds are substances that contain two or more kinds of atoms.
 Compounds often contain discrete molecules.
 A molecule contains atoms bound together in a particular way—an example is, the water molecule, which is written H2O
2.2 Properties of Matter
VOCAB
Physical properties
Physical change
Chemical properties
Chemical change
Main Ideas
 Matter has both physical and chemical properties.
 Chemical properties describe a substance’s ability to change to a different substance.
 Physical properties are the characteristics of a substance that do not involve changing to another substance. Examples are
shape, size, and color.
 Matter undergoes physical and chemical changes.
• A physical change involves a change in one or more physical properties but no change in composition.
• A chemical change transforms a substance into one or more new substances.
2.3 Classifying Matter
VOCAB
Mixture
Homogeneous mixture
Distillation
Alloys
Solution
Filtration
Pure substance
Heterogeneous mixture
Main Idea
 Matter can be classified as a mixture or a pure substance.
 A mixture has variable composition.
 A homogeneous mixture has the same properties throughout.
 A heterogeneous mixture has different properties in different parts of the mixture.
 A pure substance always has the same composition.
 Mixtures can be separated into pure substances by various means including distillation and filtration.
 Pure substances are of two types:
• Elements, which cannot be broken down chemically into simpler substances
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•
Compounds, which can be broken down chemically into elements
Make sure you check all the resources and worksheets in your binder:
Chapter 2 class notes
Chapter 2 team learning worksheet
Chapter 2 basic review worksheets
All solved section reviews and chapter assessment
Chapter 3: Chemical foundations
3.1 The Elements
VOCAB
Element symbols
Main Idea
 All of the materials in the universe can be chemically broken down into about 100 different elements.
 Nine elements account for about 98% of earth’s crust, oceans, and atmosphere.
 In the human body, oxygen, carbon, hydrogen, and nitrogen are the most abundant elements.
 Each element has a name and a symbol.
• The symbol usually consists of the first one or two letters of the element’s name.
• Sometimes the symbol is taken from the element’s original Latin or Greek name.
3.2 Atoms and Compounds
VOCAB
Law of constant composition
Atoms
Chemical formula
Dalton’s atomic theory
Compound
Main Idea
 The Law of constant composition states that a given compound always contains the same proportion by mass of the
elements of which it is composed.
 Dalton’s atomic theory states:
• All elements are composed of atoms.
• All atoms of a given element are identical.
• Atoms of different elements are different.
• Compounds consist of the atoms of different elements.
• Atoms are not created or destroyed in a chemical reaction.
 A compound is represented by a chemical formula in which the number and type of atoms present are shown by using the
element symbols and subscripts.
3.3 Atomic Structure
VOCAB
Electrons
Proton
Atomic number
Nuclear atom
Neutron
Mass number
Nucleus
Isotopes
Main Idea
 Experiments by J. J. Thomson and Ernest Rutherford showed that atoms have internal structure.
• The nucleus, which is at the center of the atom, contains protons (positively charged) and neutrons (uncharged).
• Electrons move around the nucleus.
 Electrons have a small mass (1/1836 of the proton mass).
 Electrons have a negative charge equal and opposite to that of the proton.
 Isotopes are atoms with the same number of protons but a different number of neutrons.
 A particular isotope is represented by the symbol X, in which Z represents the number of protons (atomic number) and A
represents the total number of protons and neutrons (mass number) in the nucleus.
3.4 Using the Periodic Table
GR 10 CHEMISTRY MID YEAR EXAM STUDY GUIDE - Page 2 of 4
VOCAB
Periodic table
Halogens
Nonmetals
Groups
Noble gases
Metalloids (semimetals)
Alkali metals
Transition metals
Diatomic molecules
Alkaline earth metals
Metals
Main Idea
 The periodic table shows all of the known elements in order of increasing atomic number; the table is organized to group
elements with similar properties in vertical columns.
 Most elements have metallic properties (the metals) and appear on the left side of the periodic table.
 Nonmetals appear on the right side of the periodic table.
 Metalloids are elements that have some metallic and some nonmetallic properties.
3.5 Ions and Their Compounds
VOCAB
Ion
Anion
Cation
Ionic compounds
Main Idea
 Atoms can form ions (species with a charge) by gaining or losing electrons.
• Metals tend to lose one or more electrons to form positive ions called cations; these are generally named by using
the name of the parent atom.
• Nonmetals tend to gain one or more electrons to form negative ions called anions; these are named by using the
root of the atom name followed by the suffix -ide.
 The ion that a particular atom will form can be predicted from the atom’s position on the periodic table.
• Elements in Group 1 and 2 form +1 and +2 ions, respectively.
• Group 17 atoms form anions with -1 charge.
• Group 16 atoms form anions with -2 charges.
• Group 15 atoms form anions with -3 charges.
 Ions combine to form compounds. Compounds are electrically neutral, so the sum of the charges on the anions and cations
in the compound must equal zero.
Make sure you check all the resources and worksheets in your binder:
Chapter 3 class notes
Chapter 3 team learning worksheet
Chapter 3 basic review worksheets
All solved section reviews and chapter assessment
Chapter 4: Nomenclature
4.1 Naming Binary Compounds
VOCAB
Binary compounds
Binary ionic compound
Main Ideas
Binary compounds are named by following a set of rules.
• For compounds containing both a metal and a nonmetal, the metal is always named first. The nonmetal is named
from the root element name.
• If the metal ion can have more than one charge (Type II), a Roman numeral is used to specify the charge.
• For binary compounds containing only nonmetals (Type III), prefixes are used to specify the numbers of atoms
present.
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4.2 Naming and Writing Formulas for More Complex Compounds
VOCAB
Polyatomic ions
Oxyanions
Acids
Main Ideas
 Polyatomic ions are charged entities composed of several atoms bound together. They have special names and must be
memorized.
 Naming ionic compounds containing polyatomic ions follows rules similar to those for naming binary compounds.
 The names of acids (molecules with one or more H ions attached to an anion) depend on whether the acid contains oxygen.
Make sure you check all the resources and worksheets in your binder:
Chapter 4 class notes
Chapter 4 team learning worksheet
Chapter 4 basic review worksheets
All solved section reviews and chapter assessment
GR 10 CHEMISTRY MID YEAR EXAM STUDY GUIDE - Page 4 of 4