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WorksheetsChemestry Semester Exam - Review
Total questions: 44
Worksheet time: 11hrs 0mins
Which of the following is an example of chemical change?
Melting ice
Cutting paper
Rusting of iron
Dissolving sugar in water
What is the law of conservation of mass?
Mass is created in a chemical reaction.
Mass is destroyed in a chemical reaction.
Mass is unchanged in a chemical reaction.
Mass is inversely proportional to volume.
What is the primary difference between an element and a compound?
Elements are made up of compounds.
Compounds are made up of elements.
Elements are mixtures.
Compounds are mixtures.
Physical changes alter the composition of matter.
True
False
Precision refers to how close a measurement is to the true or accepted value.
True
False
Sublimation is a phase change from gas to liquid.
True
False
In scientific notation, the number is written as the product of a coefficient and 10 raised to a power.
True
False
The mass number of an atom is the sum of its protons and neutrons.
True
False
Electrons are located in the neucleus of an atom.
True
False
Elements in the same period have the same number of valence electrons.
True
False
The atomic radius generally decreases across a period from left to right.
True
False
The smallest unit of an element that retains its chemical properties is called an _.
(a)
The process of a gas changing directly into a solid is called _.
(a)
A substance composed of two or more elements chemically combined in fixed proportions.
Homogeneous mixture
Heterogeneous mixture
Element
Compound
A combination of substances where individual components are visibly distinguishable.
Homogeneous mixture
Heterogeneous mixture
Element
Compound
A mixture that has uniform composition throughout.
Homogeneous mixture
Heterogeneous mixture
Element
Compound
What is the SI unit for mass?
Gram
Kilogram
Milligram
Microgram
How many significant figures are in the measurement 0.00560 g?
2
3
4
5
If a rectangular prism has dimensions of 4 cm x 3 cm x 6 cm, what is its volume?
72 cm3
54 cm3
24 cm3
18 cm3
The matric prefix "kilo-" represents a factor of _.
(a)
The density of an object is calculated by dividing its mass by its _.
(a)
Temperature
Liter
Kelvin
Meter
Second
Volume
Liter
Kelvin
Meter
Second
Time
Liter
Kelvin
Meter
Second
Length
Liter
Kelvin
Meter
Second
What subatomic particle has a positive charge?
Proton
Neutron
Electron
Nucleus
The atomic number of an element is equal to the number of _ in an atom.
Protons
Neutrons
Electrons
Nucleons
Isotopes of an element have the same number of _ but a different number of _.
Protons, Electrons
Electrons, Neutrons
Neutrons, Protons
Nucleons, Electrons
The region around the nucleus where electrons are likely to be found is called the _.
(a)
The electron configuration of oxygen is 1s2 2s2 _.
(a)
The energy required to remove an electron from an atom.
Atomic mass
Atomic radius
Ionization energy
Electron affinity
The size of an atom, usually represented as the distance from the nucleus to the outermost electron.
Atomic mass
Atomic radius
Ionization energy
Electron affinity
The mass of an atom, expressed in atomic mass units (u).
Atomic mass
Atomic radius
Ionization energy
Electron affinity
The energy change that occurs when an electron is added to a neutral atom to form a negative ion.
Atomic mass
Atomic radius
Ionization energy
Electron affinity
According to the periodic law, the properties of elements are a periodic function of their _.
Atomic mass
Atomic number
Number of electrons
Number of protons
Which of the following groups on the eriodic table is known as the "noble gases"?
Group 1
Group 2
Group 17
Group 18
Elements in the same _ have similar chemical properties.
Period
Group
Block
Row
The periodic tablle is organized into _ and _.
(a)
The element with the highest electronegativity is _.
(a)
The energy required to remove an electron from an atom.
Ionization energy
Electronegativity
Atomic radius
Valence electrons
The ability of an atom to attract electrons in a chemical bond.
Ionization energy
Electronegativity
Atomic radius
Valence electrons
The size of an atom, usually represented as the distance from the nucleus to the outermost electron.
Ionization energy
Electronegativity
Atomic radius
Valence electrons
The size of an atom, usually represented as the distance from the nucleus to the outermost electron.
Ionization energy
Electronegativity
Atomic radius
Valence electrons
Electrons in the outermost energy level of an atom.
Ionization energy
Electronegativity
Atomic radius
Valence electrons
