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Chemistry S1 - study questions

Total questions: 79

Worksheet time: 3hrs 1mins

Name
Class
Date
1.

An electron is

a)

positively charged

b)

neutral

c)

negatively charged

2.

atomic number is

a)

the number of protons

b)

the number of electrons

c)

the number of neutrons

d)

the location of an atom on the periodic table

3.

Conservation of mass means

a)

all the atoms present before a chemical reaction are not present after

b)

atoms present before chemical reactions are present after

c)

new substances and new elements are formed in a chemical reaction

4.
Can energy be destroyed
a)
no
b)
yes
5.
Frank has an eraser. It has a mass of 4g, and a volume of 2cm3. What is its density?
a)
8 g/cm3
b)
2 g/cm3
c)
1/2 g/cm3
d)
24 g/cm3
6.
Particles of a liquid
a)
are tightly packed together and stay in a fixed position.
b)
have no viscosity.
c)
decrease in volume with increasing temperature.
d)
are free to move around one another but still touch.
7.
Particles (molecules) in a ______________________ have more energy than the other states of matter.
a)
gas
b)
solid
c)
liquid
8.
Molecules are closest together in a 
a)
Solid
b)
Liquid
c)
Gas
9.
Atoms of the same element with a different number of neutrons
a)
Ion
b)
Gluons
c)
Isotope
d)
Quarks
10.
A charged atom
a)
Ion
b)
Isotope
c)
Electron Cloud
d)
Quark
11.
Calculation used to find the number of neutrons in an atom
a)
Atomic Mass - Atomic Number
b)
Atomic Number - Atomic Mass
c)
Atomic Mass - Electrons
d)
none of these
12.

What is the atomic number?

a)

35

b)

18

c)

17

d)

52

13.

How many protons and electrons does this element have?

a)

35

b)

18

c)

17

d)

52

14.

How many neutrons does Chlorine have?

a)

18

b)

17

c)

35

d)

52

15.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
16.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
17.

How many valence electrons are found in atoms of group 4?

a)

4

b)

3

c)

14

d)

16

18.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
19.

All atoms are most stable with (or would "prefer") how many electrons in their valence shell?

a)

1

b)

2

c)

8

d)

18

20.

What groups are the most reactive metals?

a)

2

b)

7A

c)

1

d)

17

21.

Why are halogens so reactive?

a)

They want to get rid of their only valance electron

b)

They only need one more electron

c)

They are non reactive, they have a full shell

22.

How do electrons of an element determine that element's reactivity?

a)

If the valence shell has missing electrons it is very reactive to attract or lose more electrons.

b)

If the valence shell has a full ring of electrons it is very reactive because it needs more.

c)

If the valence shell has a full shell of electrons it is very reactive because it is already full.

d)

If the valence shell has missing electrons it is not reactive because it is missing electrons.

23.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
24.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
25.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
26.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
27.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
28.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
29.
6.  Expressed in scientific notation, 0.0930 m is ___.
a)
      93 x 103 m.
b)
       9.3 x 10-3m.
c)
     9.30 x 10-2 m.
d)
     9.30 x 104 m.
30.
The atom with the largest ionization energy.
a)
Francium
b)
Fluorine
c)
Argon
d)
Radon
31.
Noble gases don't react with anything else because...
a)
they are too large
b)
they are gases
c)
they have 8 valence electrons
d)
they need to gain 1 valence electron
32.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
33.
More than two-thirds of the elements are classified as
a)
a. nonmetals
b)
b. metals
c)
c. metalloids
d)
d. noble gases
34.
The arrangement of the elements in the present Periodic Table is based on atomic
a)
a. mass
b)
b. number
c)
c. radius
d)
d. density
35.
Which two substances can not be broken down by chemical change?
a)
a. C & CuO
b)
b. C and Cu
c)
c. CO2 & CuO
d)
d. CO2 & Cu
36.
An element in an atom moves from the ground state to an excited state, the potential energy of the electron
a)
a. decreases
b)
b. increases
c)
c. remains the same
37.
What is represented by the dots in a Lewis electron-dot diagram of an atom of an element in Period 2 of the Periodic Table?
a)
a. the number of neutrons in the atom
b)
b. the number of protons in the atom
c)
c. the number of valence electrons in the atom
d)
d. the total number of electrons in the atom
38.
What causes the emission of radiant energy that produces the characteristic spectral lines?
a)
a. neutron absorption by the nucleus
b)
b. gamma ray emission from the nucleus
c)
c. movement of electrons to higher energy levels
d)
return of electrons to lower energy levels
39.
The atomic mass of an element is defined as the weighted average mass of that element's 
a)
a. most abundant isotope
b)
b. least abundant isotope
c)
c. naturally occurring isotopes
d)
d. radioactive isotopes
40.
Different isotopes of the same element must have a different 
a)
a. mass number
b)
b. atomic number
c)
c. number of protons
d)
d. number of electrons
41.

Properties you can observe without changing the identity of the substance are called _____________ properties.

a)

chemical

b)

physical

c)

transient

d)

malleable

42.
Is wood burning a physical or chemical change?
a)
Physical 
b)
Chemical
43.
Is making orange juice a physical or chemical change?
a)
Physical 
b)
Chemical
44.

What kind of matter is this?

a)

Element

b)

Compound

c)

Mixture

45.

What kind of matter is this?

a)

Element

b)

Compound

c)

Mixture

46.
The closeness of a measurement to its true (actual) value is a measure of its
a)
accuracy.
b)
precision.
c)
reproducibility.
d)
usefulness.
47.
Which type of radiation has the greatest penetrating power?
a)
Alpha
b)
Beta
c)
Gamma 
d)
Microwaves
48.
What happens to the atomic number during alpha decay?
a)
The atomic number decreases by 4
b)
The atomic number increases by 1
c)
The atomic number decreases by 2.
d)
The atomic number stays the same.
49.

In the symbol 167N what the 7 stand for?

a)

Mass number

b)

Atomic number

c)

Atomic mass

d)

Number of neutrons

50.
Two or more nuclei combine to form one larger nucleus in the process of nuclear _____.
a)
Fusion
b)
Fission
c)
Tracing
d)
Decay
51.
Which produces more energy--nuclear fission or nuclear fusion?
a)
Fusion
b)
Fission
c)
They produce the same amount
d)
It depends on the elements used
52.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Combustion
53.

Under what conditions provide a stable nucleus?

a)

Having more than 83 protons

b)

Having more protons than neutrons

c)

Having way fewer protons than neutrons

d)

Having protons that are about equal too or fewer than the number of neutrons

e)

Having a very large nucleus

54.

Where is the band of stability closest to a 1:1 ratio of Neutrons : Protons in the nucleus?

a)

Isotopes larger than atomic number 83

b)

Isotopes larger than atomic number 20

c)

Isotopes smaller than atomic number 20

d)

Isotopes smaller than atomic number 83

e)

Isotopes that are radioactive

55.

What is radioactivity?

a)

an unstable nuclei releasing particles and rays (energy) to regain stability

b)

a stable nuclei gaining particles and rays to create high energy

c)

an unstable nuclei gaining particles and rays (energy) to regain stability

d)

a stable nuclei releasing particles and rays to create high energy

56.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
Beta
c)
Gamma 
d)
none
57.
During fission, some of the nuclear mass is converted into
a)
energy
b)
heavier nuclei
c)
critical mass
d)
protons
58.
The half life of Thorium-234 is 24 days. What fraction of the element remains after 96 days
a)
1/2
b)
1/4
c)
1/8
d)
1/16
59.

What did Mendeleev use to organize the periodic table?

a)

Atomic number

b)

atomic mass

c)

# of protons

d)

# of electrons

60.
What Periodic Table family is represented by the Lewis dot diagram?
a)
Halogens
b)
Alkali Metals
c)
Transition Metals
d)
Noble Gases
61.

What are the electrons in the outermost energy level called?

a)

valence electrons

b)

octet electrons

c)

energy levels

62.
These are found on the Periodic Table.
a)
Compounds
b)
Elements
c)
Mixtures
63.

______________ refers to the way a metal can be hammered or rolled into thin sheets.

a)

Luster

b)

Malleable

c)

Metalloids

d)

Solid

64.

This group of elements have properties that are opposite those of metals. ______________________

a)

luster

b)

nonmetals

c)

metalloids

d)

metals

65.

What is the area surrounding the nucleus of an atom where electron are likely to be?

a)

electron cloud

b)

nucleus

66.

What is the region in the electron cloud around the nucleus of an atom where electrons are most likely to be?

a)

iCloud

b)

orbital

c)

protons

67.

What particles would you find in the nucleus of an atom?

a)

Protons only

b)

Protons and Neutrons

c)

Neutrons and Electrons

d)

Protons and Electrons

68.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
69.

Properties that DO depend on the amount of matter present.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

70.

Properties that depend on the identity of substance.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

71.

When something is too small or too large to see, we use _______________ to help us understand.

a)

models

b)

patterns

c)

structure and function

d)

energy and matter

72.

A system as a whole is made up of a collection of components, parts and sub-systems. all working together to achive an outcome or function. systems are described in terms of their:

a)

Outcomes

b)

Input, Process, Output

c)

Inputs

d)

Process

73.

What is the First Step of the Engineering Design Process

a)

Testing Solutions

b)

Designing Solutions

c)

Identifying the Problem

d)

Planning Solutions

74.
Which word best describes a constraint?
a)
option
b)
opportunity
c)
limitation
d)
goal
75.

You begin to create a prototype of your design only to find that your solution isn't working at all. What should you do?

a)

Add more tape

b)

Go back to an earlier stage and choose another solution

c)

Blame your partner

d)

Keep going and hope it will be ok

76.
What would a limited amount of time to complete a project be considered?
a)
Criteria
b)
Constraint
c)
Cost
d)
All of the above
77.

When designers make compromises during the Engineering Design Process, this is called __________.

a)

additional criteria.

b)

more constraints

c)

increased efficiency

d)

a trade-off

78.
Open systems like the oven allows energy to enter and leave
a)
True
b)
False
79.

What is a closed system?

a)

Mass can be transferred.

b)

Only energy can be transferred, never mass.

c)

Neither mass nor energy can be transferred.

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