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Adv. Chemistry Semester 1 Review, Part 1

Total questions: 50

Worksheet time: 1hrs 3mins

Name
Class
Date
1.

Which of the numbered pieces of lab equipment is used to light a Bunsen burner?

a)

1

b)

13

c)

17

d)

31

2.

Which of the numbered pieces of lab equipment is used to mix, heat, or hold small quantities of chemicals?

a)

8

b)

14

c)

16

d)

27

3.

Which of the numbered pieces of equipment is used to distribute heat evenly and support glassware over a Bunsen burner?

a)

4

b)

13

c)

22

d)

30

4.

What is the volume shown in this graduated cyclinder?

a)

56 mL

b)

60 mL

c)

57.0 mL

d)

56.0 mL

5.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
6.

Which state of matter is characterized by ionized particles, no definite shape or volume, and good electrical conductivity?

a)

gas

b)

liquid

c)

plasma

d)

solid

7.

What is the SI base unit for temperature?

a)

Fahrenheit

b)

degrees

c)

Celsius

d)

Kelvin

8.

What is the SI base unit for time?

a)

hour

b)

minutes

c)

seconds

d)

days

9.

What is the SI base unit for length?

a)

meter (m)

b)

kilometer (km)

c)

centimeter (cm)

d)

millimeter (mm)

10.

Which of the following answer choices shows metric prefixes in order from largest to smallest?

a)

micro-, milli-, centi-, kilo-

b)

kilo-, centi-, milli-, micro-

c)

deci-, centi-, milli-, nano-

d)

mega-, milli-, kilo-, centi-

11.

The human esophagus us about 250. mm log. How long is that in inches? 1 in = 2.54 cm

a)

10.6 inches

b)

9.84 inches

c)

11.4 inches

d)

8.84 inches

12.

How many sig figs are there in the following measurement?

0.0000080 L

a)

1

b)

2

c)

6

d)

7

13.
Multiply:
(9.4 x 106)(3.2 x 105)
a)
30.08 x 1011
b)
3.8 x 101
c)
3.008 x 1012
d)
2.9375 x 101
14.

Which of the following is a measure of the amount of matter in an object? Please select the best answer.

a)

mass

b)

weight

c)

volume

d)

density

15.

A bar of copper has a mass of 216g and a volume of 24 cm3. What is the density of copper?

a)

.11 g/cm3

b)

9.0 g/cm3

c)

5184g/cm3

d)

322 mL

16.

Which of these are extensive properties of matter?

a)

Mass

b)

Volume

c)

Density

d)

Freezing Point

e)

Size

17.

A, B, and C in the diagram refer to which states of matter?

a)

A = gas, B = liquid, C = solid

b)

A = liquid, B = gas, C = solid

c)

A = solid, B = gas, C = liquid

d)

A = solid, B = liquid, C = gas

18.
Anything that has mass and takes up space
a)
isotope
b)
matter
c)
ion
d)
atomic number
19.

Which state of matter is characterized by ionized particles, no definite shape or volume, and good electrical conductivity?

a)

gas

b)

liquid

c)

plasma

d)

solid

20.

This is the smallest particle into which an element can be divided and still be the same substance.

a)

Mixture

b)

Compound

c)

Element

d)

Atom

21.

What kind of substance is composed of two or more elements that are chemically combined in fixed ratios?

a)

element

b)

mixture

c)

solution

d)

compound

22.

A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called a(n)...

a)

nuclide

b)

neutron

c)

electron

d)

isotope

23.
What is a photon?
a)
When radiation burst through electric waves
b)
The emission of electrons from a metal caused by light striking the metal
c)
The rate at which a waves energy flows through a given unit of area.
d)
packets of electromagnetic energy
24.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

25.

Classify the following as either a physical or chemical change: Ripping up a piece of paper

a)

Physical

b)

Chemical

c)

Both

d)

Neither

26.

Classify the following as either a physical or chemical change: Burning a marshmallow.

a)

Physical

b)

Chemical

c)

Both

d)

Neither

27.

What does the Law of Conservation of Mass imply about the mass of reactants and products in a chemical reaction?

a)

Mass of reactants is always greater.

b)

Mass of products is always greater.

c)

Mass of reactants equals mass of products.

d)

Mass of reactants is always less.

28.

What defines an isotope of an element?

a)

Atoms with the same number of protons but different numbers of electrons

b)

Atoms with the same number of neutrons but different numbers of protons

c)

Atoms with the same number of protons but different numbers of neutrons

d)

Atoms with the same number of electrons but different numbers of protons

29.

Which of the following is a heterogeneous mixture?

a)

Brass

b)

Sand

c)

Kool-aid

d)

Air

30.

Which of the following statements is NOT a part of Dalton's Atomic Theory?

a)

Atoms of different elements can combine in simple whole-number ratios to form compounds.

b)

Atoms are indivisible and indestructible.

c)

Atoms consist of protons, neutrons, and electrons

d)

Chemical reactions involve the rearrangement of atoms.

e)

Atoms of a given element are identical but differ from the atoms of other elements

31.

What experiment did JJ Thomson use to study the negatively charged particles with very small masses that came to be known as electrons?

a)

gold foil experiment

b)

cathode ray tube experiment

c)

oil drop experiment

32.

After Rutherford discovered the nucleus, which model is believed to be true?

a)

protons, neutrons, and electrons are evenly distributed

b)

the nucleus is made of protons, neutrons, and electrons

c)

the nucleus is made of protons and electrons

d)

the model is mostly empty space with a central nucleus

33.

Whose series of experiments identified the nucleus of the atom?

a)

Rutherford

b)

Dalton

c)

Thompson

d)

Bohr

34.

Determine the number of protons, neutrons, and electrons in the element cobalt.

a)

27, 59, 27

b)

27, 32, 27

c)

59, 27, 59

d)

27, 59, 32

35.

An aluminum isotope consists of 13 protons, 13 electrons and 14 neutrons. Its mass number is

a)

13

b)

14

c)

27

d)

40

36.

What information is necessary to determine the average atomic mass of chromium?

a)

The mass of each naturally occurring isotope of chromium.

b)

The relative abundance of each naturally occurring isotope of chromium.

c)

The atomic number of each naturally occurring isotope of chromium.

d)

The mass and the relative abundance of each naturally occurring isotope of chromium.

37.

What does each individual line in an atomic emission spectrum represent?

a)

The light absorbed by an electron as it moves from a lower energy level (ground state) to a higher energy level (excited state).

b)

The concentration of an element in a solution.

c)

The presence of an electron, hence the whole spectrum can be used to determine the number of electrons in an element.

d)

The light emitted by an electron as it relaxes from a higher energy level (excited state) to a lower energy level (ground state).

38.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
39.

Calculate the energy of a photon with a frequency of 5×1014 Hz5 \times 10^{14} \, \text{Hz} . Use h=6.63×10−34 Jsh = 6.63 \times 10^{-34} \, \text{Js} .

a)

3.32×10−19 J3.32 \times 10^{-19} \, \text{J}

b)

3.32×10−20 J3.32 \times 10^{-20} \, \text{J}

c)

3.32×10−21 J3.32 \times 10^{-21} \, \text{J}

d)

3.32×10−22 J3.32 \times 10^{-22} \, \text{J}

40.

Developed the “uncertainty principle” that states that it is impossible to determine simultaneously both the position and the velocity of an electron.

a)

Werner Heisenberg

b)

James Chadwick

c)

Henry Moseley

d)

Erwin Schrödinger

41.

Describes mathematically the wave properties of electrons

a)

Quantum Theory

b)

Werner Heisenberg

c)

Ernest Rutherford

42.

The volume of an atom is made up mostly of

a)

protons.

b)

the nucleus.

c)

the electron cloud.

d)

neutrons.

43.

Which of the following statements about "s" orbitals is correct?

a)

They are found in all principal energy levels.

b)

They can hold up to two electrons.

c)

They can hold up to two electrons.They are spherical in shape.

d)

All of the other answers are correct.

44.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
45.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
46.

Who is credited with being the first to create a periodic table with elements grouped by increasing atomic mass and similarities among their chemical properties? He also correctly predicted the existence of new elements.

a)

Henry Moseley

b)

Antoine Lavoisier

c)

John Newlands

d)

Dmitri Mendeleev

47.

In the periodic table, elements are arranged by ____________.

a)

alphabetical order.

b)

atomic number.

c)

atomic mass.

d)

their number of neutrons.

48.

The atomic number of an element is the total number of which subatomic particle found in the nucleus?

a)

Electron

b)

Neutron

c)

Proton

d)

Neutrons + Protons

49.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
50.
Name group 1 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
noble gases
d)
halogens

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