Which of the following best explains the difference between physical and chemical properties, and gives one example of each?

Physical properties can be observed without changing the substance, like color; chemical properties involve a change in composition, like flammability.

Physical properties involve a change in composition, like rusting; chemical properties can be observed without changing the substance, like melting point.

Physical properties and chemical properties are the same; both involve changes in composition.

Physical properties are only found in solids; chemical properties are only found in liquids.

Which of the following are two ways mixtures can be separated, along with an example of each method?

Filtration (e.g., separating sand from water) and evaporation (e.g., separating salt from water)

Melting (e.g., melting ice) and freezing (e.g., making ice cream)

Condensation (e.g., forming dew) and sublimation (e.g., dry ice)

Boiling (e.g., boiling water) and dissolving (e.g., sugar in tea)

The three main types of chemical bonds found in compounds are:

Ionic, covalent, and metallic bonds

Hydrogen, peptide, and disulfide bonds

Van der Waals, ionic, and peptide bonds

Covalent, hydrogen, and glycosidic bonds

The difference between physical and chemical properties is:

Physical properties can be observed without changing the substance's identity, while chemical properties involve a change in identity.

Physical properties involve a change in identity, while chemical properties do not.

Both physical and chemical properties involve changes in identity.

Physical properties and chemical properties are the same.

Which of the following lists the three main types of chemical bonds?

Covalent, hydrogen, and van der Waals

Metallic, peptide, and hydrogen

Which of the following correctly explains the difference between intrinsic (intensive) and extrinsic (extensive) properties, and provides two examples of each?

Intrinsic properties do not depend on the amount of matter (e.g., density, boiling point), while extrinsic properties do (e.g., mass, volume).

Intrinsic properties depend on the amount of matter (e.g., mass, volume), while extrinsic properties do not (e.g., density, boiling point).

Both intrinsic and extrinsic properties depend on the amount of matter (e.g., mass, volume).

Neither intrinsic nor extrinsic properties depend on the amount of matter (e.g., color, shape).

The metric system is organized in a certain way and is called a base ten system because:

It is based on multiples of ten, making conversions simple by moving the decimal point.

It uses random units for each measurement, making conversions difficult.

It is based on the imperial system, which uses fractions.

It is organized by alphabetical order of units.

What is meant by a “physical property” of a substance? Give three examples.

A characteristic that can be observed or measured without changing the substance's identity; examples: color, melting point, density.

A property that involves a chemical reaction; examples: flammability, reactivity, acidity.

A property that only appears at high temperatures; examples: boiling, burning, rusting.

A property that describes the ability to conduct electricity; examples: magnetism, solubility, radioactivity.

What is meant by a “chemical property”?

A characteristic that describes a substance's ability to change into different substances.

A property related to the mass and volume of a substance.

A property that can be measured using a ruler.

Which of the following lists describes the five chemical changes?

Color change, temperature change, gas production, formation of a precipitate, change in odor

Melting, freezing, boiling, condensation, sublimation

Cutting, tearing, crushing, bending, stretching

Dissolving, mixing, filtering, evaporating, condensing

Which of the following correctly compares pure substances and mixtures, providing at least two examples of each?

Pure substances have a fixed composition and include water and gold; mixtures have variable composition and include air and salad.

Pure substances have variable composition and include air and salad; mixtures have a fixed composition and include water and gold.

Pure substances and mixtures both have variable composition; examples include water and salad for both.

Pure substances and mixtures both have fixed composition; examples include air and gold for both.

What are homogeneous and heterogeneous mixtures? Give an example of each.

Homogeneous mixtures have a uniform composition throughout, like salt water; heterogeneous mixtures have visibly different parts, like salad.

Homogeneous mixtures have visibly different parts, like salad; heterogeneous mixtures have a uniform composition throughout, like salt water.

Both homogeneous and heterogeneous mixtures have a uniform composition throughout.

Homogeneous mixtures and heterogeneous mixtures are both pure substances.

Distillation separates mixtures by:

Evaporating and condensing liquids based on their boiling points

Using a magnet to separate components

The significance of the Gold Foil Experiment and its contributions to atomic theory can be summarized as:

It showed that atoms have a small, dense, positively charged nucleus.

It proved that atoms are indivisible and solid.

It demonstrated that electrons orbit the nucleus in fixed paths.

It confirmed that atoms are made only of protons and neutrons.

Who was Mendeleev and what was his contribution to science?

He was a Russian chemist who created the periodic table of elements.

He was an Italian physicist who invented the battery.

He was a French biologist who discovered penicillin.

He was a German mathematician who developed calculus.

What determines the atomic number of an element? Why is this important?

The number of protons in the nucleus; it defines the identity of the element.

The number of neutrons in the nucleus; it determines the isotope.

The number of electrons in the outer shell; it determines reactivity.

The atomic mass; it determines the stability of the element.

The difference between atomic number and atomic mass is:

Atomic number is the number of protons; atomic mass is the sum of protons and neutrons.

Atomic number is the sum of protons and neutrons; atomic mass is the number of protons.

Atomic number is the number of neutrons; atomic mass is the number of protons.

Atomic number and atomic mass are the same.

The three main types of chemical bonds are:

Metallic, Hydrogen, Van der Waals

You can determine what type of bond will form between two elements by:

Comparing their electronegativities

Key differences between covalent and ionic compounds include:

Covalent compounds share electrons, while ionic compounds transfer electrons.

Covalent compounds conduct electricity in solution, while ionic compounds do not.

Ionic compounds have low melting points, while covalent compounds have high melting points.

Covalent compounds are always solids, while ionic compounds are always gases.

Transition metals in compounds are named by:

Using Roman numerals to indicate the oxidation state

Using prefixes to indicate the number of atoms

Using Greek letters to indicate the charge

Subscripts in a chemical formula tell you the number of atoms of each element. What do subscripts indicate?

The number of atoms of each element

The Law of Conservation of Energy states that:

Energy can be transformed from one form to another, but cannot be created or destroyed.

Energy can be created and destroyed.

Energy is always lost in every process.

Energy only exists in living things.

Energy shells are ______ and valence electrons are important because ______.

layers around the nucleus; they determine chemical reactivity

types of atoms; they give mass to the atom

protons in the nucleus; they define atomic number

neutrons in the atom; they affect stability

Which of the following correctly compares the properties of metals, non-metals, and metalloids?

Metals are good conductors, non-metals are poor conductors, metalloids have intermediate conductivity.

Metals are brittle, non-metals are malleable, metalloids are ductile.

Metals are dull, non-metals are shiny, metalloids are always gases.

Metals are non-magnetic, non-metals are magnetic, metalloids are always liquids.

Rows on the periodic table are called periods, and columns are called groups because:

Rows represent repeating patterns of properties, and columns group elements with similar properties.

Rows group elements with similar properties, and columns show repeating patterns.

Rows and columns are named randomly.

Rows and columns are named after scientists.

How does the arrangement of the periodic table reflect properties of elements?

It groups elements with similar properties together.

It arranges elements in alphabetical order.

It separates metals and nonmetals randomly.

It lists elements by their discovery date.

Give an example of a compound formed by a covalent bond, and one formed by an ionic bond.

Water (H₂O) and Sodium chloride (NaCl)

Sodium chloride (NaCl) and Oxygen (O₂)

Hydrogen (H₂) and Carbon dioxide (CO₂)

Magnesium oxide (MgO) and Water (H₂O)

What clues in the chemical formula or names help you identify if a compound is ionic, covalent, or metallic?

The presence of metals and nonmetals, prefixes in names, and the type of elements involved

The physical state at room temperature

How would you use oxidation numbers to write a chemical formula from element names?

By balancing the total positive and negative oxidation numbers to zero.

By adding the atomic numbers of the elements.

By arranging the elements alphabetically.

By using only the first letter of each element.

Newton’s First law of motion deals with inertia. State that law.

An object at rest stays at rest and an object in motion stays in motion unless acted upon by an external force.

Force equals mass times acceleration.

For every action, there is an equal and opposite reaction.

Energy cannot be created or destroyed.

Newton’s Third law of motion states that:

Every action has an equal and opposite reaction.

A body remains at rest unless acted upon by a force.

Force equals mass times acceleration.

Energy cannot be created or destroyed.

Physical Science Final Exam Study Guide

9th Grade

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77 Qs

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Physical Science Final Exam Study Guide

Quiz

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Science

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9th Grade

•

Practice Problem

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Medium

•

NGSS

MS-PS1-1, MS-PS1-2, HS-PS1-1

Standards-aligned

Kimberly Martin

Used 5+ times

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77 questions

Show all answers

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The metric system uses prefixes such as kilo-, hecto-, and milli- to represent different _______________ of measurement.

prefixes

colors

shapes

tools

MATCH QUESTION

1 min • 1 pt

Match the metric prefix with its unit.

1/1000

centi-

1/10

milli-

1/100

hecto-

1000x

kilo-

100x

deci-

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Fill in the blank with the correct words. A _______________ property can be observed without changing the substance into something new.

physical

chemical

atomic

magnetic

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Fill in the blank with the correct words. _______________ are pure substances that cannot be broken down into simpler substances by chemical means.

elements

compounds

mixtures

solutions

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Fill in the blank: The number of _______________ in an atom determines its atomic number.

protons

neutrons

electrons

nuclei

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Fill in the blank: In a _______________ bond, electrons are shared between atoms.

covalent

ionic

metallic

hydrogen

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following is an example of a chemical change?

Melting ice

Dissolving sugar in water

Rusting iron

Cutting paper

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Physical Science Final Exam Study Guide

77 questions

The metric system uses prefixes such as kilo-, hecto-, and milli- to represent different _______________ of measurement.

Match the metric prefix with its unit.

Fill in the blank with the correct words. A _______________ property can be observed without changing the substance into something new.

Fill in the blank with the correct words. _______________ are pure substances that cannot be broken down into simpler substances by chemical means.

Fill in the blank: The number of _______________ in an atom determines its atomic number.

Fill in the blank: In a _______________ bond, electrons are shared between atoms.

Which of the following is an example of a chemical change?

Which scientist is known for the "Gold Foil Experiment"?

Which of these is NOT a type of chemical bond?

What does the arrow in a chemical equation represent?

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