Study Guide 1 Section 2.1 Units and Measurements Key Concepts SI measurement units allow scientists to report data to other scientists. Adding prefixes

Study Guide 1

Section 2.1 Units and Measurements

Key Concepts

• SI measurement units allow scientists to report data to other scientists.

• Adding prefixes to SI units extends the range of possible measurements.

• To convert to Kelvin temperature, add 273 to the Celsius temperature. K = °C + 273

• Volume and density have derived units. Density, which is a ratio of mass to volume, can be used to identify an unknown sample of matter.

Study Guide 2

Section 2.2 Scientific Notation and Dimensional Analysis

Key Concepts

• A number expressed in scientific notation is written as a coefficient between 1 and 10 multiplied by 10 raised to a power.

• To add or subtract numbers in scientific notation, the numbers must have the same exponent.

• To multiply or divide numbers in scientific notation, multiply or divide the coefficients and then add or subtract the exponents, respectively.

• Dimensional analysis uses conversion factors to solve problems.

Study Guide 3

Section 2.3 Uncertainty in Data

Key Concepts

• An accurate measurement is close to the accepted value. A set of precise measurements shows little variation.

• The measurement device determines the degree of precision possible.

• Error is the difference between the measured value and the accepted value. Percent error gives the percent deviation from the accepted value.

error = experimental value – accepted value

Study Guide 3

Section 2.3 Uncertainty in Data (cont.)

Key Concepts

• The number of significant figures reflects the precision of reported data.

• Calculations should be rounded to the correct number of significant figures.

Study Guide 4

Section 2.4 Representing Data

Key Concepts

• Circle graphs show parts of a whole. Bar graphs show how a factor varies with time, location, or temperature.

• Independent (x-axis) variables and dependent (y-axis) variables can be related in a linear or a nonlinear manner. The slope of a straight line is defined as rise/run, or ∆y/∆x.

• Because line graph data are considered continuous, you can interpolate between data points or extrapolate beyond them.

A. A

B. B

C. C

D. D

Chapter Assessment 1

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Which of the following is the SI derived unit of volume?

A. gallon

B. quart

C. m3

D. kilogram

A. A

B. B

C. C

D. D


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Which prefix means 1/10th?

A. deci-

B. hemi-

C. kilo-

D. centi-

A. A

B. B

C. C

D. D


0% 0%0%0%

Divide 6.0 109 by 1.5 103.

A. 4.0 106

B. 4.5 103

C. 4.0 103

D. 4.5 106

A. A

B. B

C. C

D. D


0% 0%0%0%

Round the following to 3 significant figures 2.3450.

A. 2.35

B. 2.345

C. 2.34

D. 2.40

A. A

B. B

C. C

D. D


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The rise divided by the run on a line graph is the ____.

A. x-axis

B. slope

C. y-axis

D. y-intercept

A. A

B. B

C. C

D. D

STP 1

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Which is NOT an SI base unit?

A. meter

B. second

C. liter

D. kelvin

A. A

B. B

C. C

D. D

STP 2

0% 0%0%0%

Which value is NOT equivalent to the others?

A. 800 m

B. 0.8 km

C. 80 dm

D. 8.0 x 105 cm

A. A

B. B

C. C

D. D

STP 3

0% 0%0%0%

Find the solution with the correct number of significant figures:25 0.25

A. 6.25

B. 6.2

C. 6.3

D. 6.250

A. A

B. B

C. C

D. D

STP 4

0% 0%0%0%

How many significant figures are there in 0.0000245010 meters?

A. 4

B. 5

C. 6

D. 11

A. A

B. B

C. C

D. D

STP 5

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Which is NOT a quantitative measurement of a liquid?

A. color

B. volume

C. mass

D. density

Study Guide 1

Section 3.1 Properties of Matter

Key Concepts

• The three common states of matter are solid, liquid, and gas.

• Physical properties can be observed without altering a substance’s composition.

• Chemical properties describe a substance’s ability to combine with or change into one or more new substances.

• External conditions can affect both physical and chemical properties.

Study Guide 2

Section 3.2 Changes in Matter

Key Concepts

• A physical change alters the physical properties of a substance without changing its composition.

• A chemical change, also known as a chemical reaction, involves a change in a substance’s composition.

• In a chemical reaction, reactants form products.

• The law of conservation of mass states that mass is neither created nor destroyed during a chemical reaction; it is conserved.

massreactants = massproducts

Study Guide 3

Section 3.3 Mixtures of Matter

Key Concepts

• A mixture is a physical blend of two or more pure substances in any proportion.

• Solutions are homogeneous mixtures.

• Mixtures can be separated by physical means. Common separation techniques include filtration, distillation, crystallization, sublimation, and chromatography.

Study Guide 4

Section 3.4 Elements and Compounds

Key Concepts

• Elements cannot be broken down into simpler substances.

• Elements are organized in the periodic table of the elements.

• Compounds are chemical combinations of two or more elements and their properties differ from the properties of their component elements.

A. A

B. B

C. C

D. D


A B C D

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Which of the following is NOT a physical property of water?

A. Ice melts at 0°C.

B. Water boils at 100.

C. Water reacts violently with pure sodium.

D. Water is a liquid at room temperature.

A. A

B. B

C. C

D. D


A B C D

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28.0 grams of nitrogen gas reacts completely with 6.0 grams of hydrogen to form 34.0 grams of ammonia. What does this demonstrate?

A. the law of conservation of energy

B. sublimation

C. distillation

D. the law of conservation of mass

A. A

B. B

C. C

D. D


A B C D

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What is the best way to separate salt dissolved in water?

A. sublimation

B. crystallization

C. freezing

D. filtration

A. A

B. B

C. C

D. D


A B C D

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Two or more elements chemically joined form what?

A. substance

B. heterogeneous mixture

C. homogenous solution

D. compound

A. A

B. B

C. C

D. D

STP 1

A B C D

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Which is NOT a chemical reaction?

A. a car rusting

B. dissolving sugar in water

C. wood burning

D. a banana ripening

A. A

B. B

C. C

D. D

STP 3

A B C D

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Elements in the same period are likely to have similar ____.

A. physical properties

B. densities

C. chemical properties

D. melting points

A. A

B. B

C. C

D. D

STP 4

A B C D

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Filtration is an easy way to separate what?

A. heterogeneous mixture

B. homogeneous mixture

C. compounds

D. solutions

A. A

B. B

C. C

D. D

STP 5

A B C D

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Compounds can be broken into their component elements by which of the following?

A. crystallization

B. distillation

C. filtration

D. chemical reaction

Study Guide 1

Section 4.1 Early Ideas About Matter

Key Concepts

• Democritus was the first person to propose the existence of atoms.

• According to Democritus, atoms are solid, homogeneous, and indivisible.

• Aristotle did not believe in the existence of atoms.

• John Dalton’s atomic theory is based on numerous scientific experiments.

Study Guide 2

Section 4.2 Defining the Atom

Key Concepts

• An atom is the smallest particle of an element that maintains the properties of that element.

• Electrons have a 1– charge, protons have a 1+ charge, and neutrons have no charge.

• An atom consists mostly of empty space surrounding the nucleus.

Study Guide 3

Section 4.3 How Atoms Differ

Key Concepts

• The atomic number of an atom is given by its number of protons. The mass number of an atom is the sum of its neutrons and protons.

atomic number = number of protons = number of electrons

mass number = atomic number + number of neutrons

• Atoms of the same element with different numbers of neutrons are called isotopes.

• The atomic mass of an element is a weighted average of the masses of all of its naturally occurring isotopes.

Study Guide 4

Section 4.4 Unstable Nuclei and Radioactive Decay

Key Concepts

• Chemical reactions involve changes in the electrons surrounding an atom. Nuclear reactions involve changes in the nucleus of an atom.

• There are three types of radiation: alpha (charge of 2+), beta (charge of 1–), and gamma (no charge).

• The neutron-to-proton ratio of an atom’s nucleus determines its stability.

A. A

B. B

C. C

D. D


A B C D

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Whose work led to the modern atomic theory?

A. Dalton

B. Rutherford

C. Einstein

D. Aristotle

A. A

B. B

C. C

D. D


A B C D

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Which particle is not found in the nucleus of an atom?

A. neutron

B. proton

C. gamma ray

D. electron

A. A

B. B

C. C

D. D


A B C D

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Two isotopes of an unknown element have the same number of:

A. protons

B. neutrons

C. electrons

D. both A and C

A. A

B. B

C. C

D. D


A B C D

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Lithium has an atomic mass of 6.941 and two isotopes, one with 6 neutrons and one with 7 neutrons. Which isotope is more abundant?

A. 6Li

B. 7Li

C. Both isotopes occur equally.

D. unable to determine

A. A

B. B

C. C

D. D


A B C D

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What happens when an element emits radioactive particles?

A. It gains energy.

B. It gains neutrons.

C. It loses stability.

D. It loses energy.

A. A

B. B

C. C

D. D

STP 1

A B C D

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What is the smallest particle of an element that still retains the properties of that element?

A. proton

B. atom

C. electron

D. neutron

A. A

B. B

C. C

D. D

STP 2

A B C D

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How many neutrons, protons, and electrons does 124

54Xe have?

A. 124 neutrons, 54 protons, 54 electrons

B. 70 neutrons, 54 protons, 54 electrons

C. 124 neutrons, 70 protons, 54 electrons

D. 70 neutrons, 70 protons, 54 electrons

A. A

B. B

C. C

D. D

STP 3

A B C D

0% 0%0%0%

The primary factor in determining an atom's stability is its ratio of neutrons to ____.

A. protons

B. electrons

C. alpha particles

D. isotopes

A. A

B. B

C. C

D. D

STP 4

A B C D

0% 0%0%0%

What is the densest region of an atom?

A. electron cloud

B. nucleus

C. isotopes

D. atomic mass

A. A

B. B

C. C

D. D

STP 5

A B C D

0% 0%0%0%

Why are electrons attracted to the cathode in a cathode ray tube?

A. The cathode is more stable.

B. The cathode has a positive charge.

C. The cathode has a negative charge.

D. The cathode has no charge.

IB 1

Study Guide 1

Section 5.1 Light and Quantized Energy

Key Concepts

• All waves are defined by their wavelengths, frequencies, amplitudes, and speeds. c = λν

• In a vacuum, all electromagnetic waves travel at the speed of light.

• All electromagnetic waves have both wave and particle properties.

• Matter emits and absorbs energy in quanta.Equantum = hν

Study Guide 2

Section 5.2 Quantum Theory and the Atom

Key Concepts

• Bohr’s atomic model attributes hydrogen’s emission spectrum to electrons dropping from higher-energy to lower-energy orbits.

∆E = E higher-energy orbit - E lower-energy orbit = E photon = hν

• The de Broglie equation relates a particle’s wavelength to its mass, its velocity, and Planck’s constant. λ = h / mν

• The quantum mechanical model of the atom assumes that electrons have wave properties.

• Electrons occupy three-dimensional regions of space called atomic orbitals.

Study Guide 3

Section 5.3 Electron Configuration

Key Concepts

• The arrangement of electrons in an atom is called the atom’s electron configuration.

• Electron configurations are defined by the aufbau principle, the Pauli exclusion principle, and Hund’s rule.

• An element’s valence electrons determine the chemical properties of the element.

• Electron configurations can be represented using orbital diagrams, electron configuration notation, and electron-dot structures.

A. A

B. B

C. C

D. D


A B C D

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The shortest distance from equivalent points on a continuous wave is the:

A. frequency

B. wavelength

C. amplitude

D. crest

A. A

B. B

C. C

D. D


A B C D

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The energy of a wave increases as ____.

A. frequency decreases

B. wavelength decreases

C. wavelength increases

D. distance increases

A. A

B. B

C. C

D. D


A B C D

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Atom’s move in circular orbits in which atomic model?

A. quantum mechanical model

B. Rutherford’s model

C. Bohr’s model

D. plum-pudding model

A. A

B. B

C. C

D. D


A B C D

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It is impossible to know precisely both the location and velocity of an electron at the same time because:

A. the Pauli exclusion principle

B. the dual nature of light

C. electrons travel in waves

D. the Heisenberg uncertainty principle

A. A

B. B

C. C

D. D


A B C D

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How many valence electrons does neon have?

A. 0

B. 1

C. 2

D. 3

A. A

B. B

C. C

D. D

STP 1

A B C D

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Spherical orbitals belong to which sublevel?

A. s

B. p

C. d

D. f

A. A

B. B

C. C

D. D

STP 2

A B C D

0% 0%0%0%

What is the maximum number of electrons the 1s orbital can hold?

A. 10

B. 2

C. 8

D. 1

A. A

B. B

C. C

D. D

STP 3

A B C D

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In order for two electrons to occupy the same orbital, they must:

A. have opposite charges

B. have opposite spins

C. have the same spin

D. have the same spin and charge

A. A

B. B

C. C

D. D

STP 4

A B C D

0% 0%0%0%

How many valence electrons does boron contain?

A. 1

B. 2

C. 3

D. 5

A. A

B. B

C. C

D. D

STP 5

A B C D

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What is a quantum?

A. another name for an atom

B. the smallest amount of energy that can be gained or lost by an atom

C. the ground state of an atom

D. the excited state of an atom

Study Guide 1

Section 6.1 Development of the Modern Periodic Table (contd.)

Key Concepts

Elements are classified as either metals, nonmetals, or metalloids.

Study Guide 2

Section 6.2 Classification of the Elements

Key Concepts

The periodic table has four blocks (s, p, d, f).

Elements within a group have similar chemical properties.

The group number for elements in groups 1 and 2 equals the element’s number of valence electrons.

The energy level of an atom’s valence electrons equals its period number.

Study Guide 3

Section 6.3 Periodic Trends

Key Concepts

Atomic and ionic radii decrease from left to right across a period, and increase as you move down a group.

Ionization energies generally increase from left to right across a period, and decrease as you move down a group.

The octet rule states that atoms gain, lose, or share electrons to acquire a full set of eight valence electrons.

Electronegativity generally increases from left to right across a period, and decreases as you move down a group.

A. A

B. B

C. C

D. D


A B C D

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The actinide series is part of the

A. s-block elements.

B. inner transition metals.

C. non-metals.

D. alkali metals.

A. A

B. B

C. C

D. D


A B C D

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In their elemental state, which group has a complete octet of valence electrons?

A. alkali metals

B. alkaline earth metals

C. halogens

D. noble gases

A. A

B. B

C. C

D. D


A B C D

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Which block contains the transition metals?

A. s-block

B. p-block

C. d-block

D. f-block

A. A

B. B

C. C

D. D


A B C D

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An element with a full octet has how many valence electrons?

A. two

B. six

C. eight

D. ten

A. A

B. B

C. C

D. D


A B C D

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How many groups of elements are there?

A. 8

B. 16

C. 18

D. 4

A. A

B. B

C. C

D. D

STP 1

A B C D

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Which group of elements are the least reactive?

A. alkali metals

B. inner transition metals

C. halogens

D. noble gases

A. A

B. B

C. C

D. D

STP 2

A B C D

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On the modern periodic table, alkaline earth metals are found only in ____.

A. group 1

B. s-block

C. p-block

D. groups 13–18

A. A

B. B

C. C

D. D

STP 3

A B C D

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Unreactive gases are mostly found where on the periodic table?

A. halogens

B. group 1 and 2

C. group 18

D. f-block

A. A

B. B

C. C

D. D

STP 4

A B C D

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Bromine is a member of the

A. noble gases.

B. inner transition metals.

C. earth metals.

D. halogens.

Study Guide 1

Section 7.1 Ion Formation

Key Concepts

• A chemical bond is the force that holds two atoms together.

• Some atoms form ions to gain stability. This stable configuration involves a complete outer energy level, usually consisting of eight valence electrons.

• Ions are formed by the loss or gain of valence electrons.

• The number of protons remains unchanged during ion formation.

Study Guide 2

Section 7.2 Ionic Bonds and Ionic Compounds

Key Concepts

• Ionic compounds contain ionic bonds formed by the attraction of oppositely charged ions.

• Ions in an ionic compound are arranged in a repeating pattern known as a crystal lattice.

• Ionic compound properties are related to ionic bond strength.

• Ionic compounds are electrolytes; they conduct an electric current in the liquid phase and in aqueous solution.

Study Guide 2

Section 7.2 Ionic Bonds and Ionic Compounds (cont.)

Key Concepts

• Lattice energy is the energy needed to remove 1 mol of ions from its crystal lattice.

Study Guide 3

Section 7.3 Names and Formulas for Ionic Compounds

Key Concepts

• A formula unit gives the ratio of cations to anions in the ionic compound.

• A monatomic ion is formed from one atom. The charge of a monatomic ion is its oxidation number.

• Roman numerals indicate the oxidation number of cations having multiple possible oxidation states.

• Polyatomic ions consist of more than one atom and act as a single unit.

A. A

B. B

C. C

D. D


A B C D

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Cations form when atoms _______ electrons.

A. gain

B. lose

C. charge

D. delocalize

A. A

B. B

C. C

D. D


A B C D

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What is the repeating pattern of atoms in an ionic solid called?

A. crystal lattice

B. ionic lattice

C. energy lattice

D. ionic bonding

A. A

B. B

C. C

D. D


A B C D

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Give the name of the following: NaClO4

A. sodium hypochlorite

B. sodium chlorite

C. sodium chlorate

D. sodium perchlorate

A. A

B. B

C. C

D. D


A B C D

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As the distance between ions in an ionic bond is shortened,

A. the energy to break the bond decreases.

B. the electrostatic attraction decreases.

C. the electrostatic attraction increases.

D. the ionic bond changes to a metallic bond.

A. A

B. B

C. C

D. D


A B C D

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An alloy is what type of substance?

A. heterogeneous mixture

B. compound

C. mixture of elements

D. element

A. A

B. B

C. C

D. D

STP 1

A B C D

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Which is NOT true about metallic solids?

A. Metals are shiny.

B. Metals are good conductors of heat and electricity.

C. Metals are ductile.

D. Metals have relatively low boiling points.

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Documents

Study Guide 1 Section 2.1 Units and Measurements Key Concepts SI measurement units allow scientists to report data to other scientists. Adding prefixes