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Thermo CHEM

Total questions: 69

Worksheet time: 2hrs 0mins

Name
Class
Date
1.

What is the definition of specific heat?

a)

The temperature at which a substance freezes

b)

Amount of heat required to raise the temperature of one gram of a substance by one degree Celsius

c)

The amount of energy released during a chemical reaction

d)

Amount of heat required to boil water

2.

What is the difference between endothermic and exothermic reactions?

a)

Endothermic reactions and exothermic reactions both release heat into the surroundings.

b)

Endothermic reactions and exothermic reactions both absorb heat from the surroundings.

c)

Endothermic reactions release heat into the surroundings, while exothermic reactions absorb heat from the surroundings.

d)

Endothermic reactions absorb heat from the surroundings, while exothermic reactions release heat into the surroundings.

3.

Explain the concept of calorimetry and its application in chemistry.

a)

Calorimetry is used in chemistry to measure the heat of chemical reactions or physical changes.

b)

Calorimetry is used in chemistry to measure the pressure of chemical reactions

c)

Calorimetry is used in chemistry to measure the color changes in chemical reactions

d)

Calorimetry is used in chemistry to measure the volume of chemical reactions

4.

Which best describes enthalpy change?.

a)

Enthalpy is the measure of acidity in a chemical reaction.

b)

Enthalpy is the change of energy that is available as heat during a chemical reaction.

c)

Enthalpy is the amount of matter present in a chemical reaction.

d)

Enthalpy is the measure of heat.

5.

Sweating is an __________________ process because heat is released.

a)

endothermic

b)

exothermic

6.
What is the symbol for heat?
a)
q
b)
H
c)
J
d)
∘C
7.

What is the study of heat changes that accompany chemical reactions and phase changes?

a)

energy

b)

chemistry

c)

work

d)

thermochemistry

8.

What is the formula for calculating heat?

a)

q = mcΔT

b)

H = ΔH x moles

c)

H = ΔH x grams

d)

products - reactants

9.

How much heat does an aluminum block absorb if 10.00 grams is heated from 25.0oC to 50.0oC? *Specific heat of aluminum is 0.900 J/goC

a)

450 J

b)

-450 J

c)

225 J

d)

-225 J

10.

When a hot object and a cold object come together, heat will move from the warmer one to the colder one until they are the same temperature. What is this called?


a)

Equal

b)

Equality

c)

Equilibrium

11.

When ammonium chloride dissolves in water the temperature falls. The type of energy change is described as ____

a)

exothermic    

b)

 activated  

c)

decomposition

d)

endothermic

12.

_____ reactions usually feel hot!

a)

endothermic

b)

exothermic

13.

How can you find the change in temperature?

a)


Tfinal + TinitalT_{final}\ +\ T_{inital}

b)

Tfinal − TinitialT_{final}\ -\ T_{initial}

c)

Tinitial​ − Tfinal​

14.

The amount of heat energy required to change the temperature of 12 g of gold from 45°C to 15°C is -47 J. What is the specific heat capacity of gold?

a)

0.13 J/(g°C)

b)

17,000 J/(g°C)

c)

1600 J/(g°C)

d)

0.065 J/(g°C)

15.
What is a device used to measure the heat absorbed or released during a chemical or physical change?
a)
joule
b)
enthalpy
c)
calorimeter
d)
specific heat?
16.

What is a substance undergoing a chemical or physical change?

a)

Substance

b)

System

c)

Calorimeter

d)

Specific heat

17.
The specific heat of mercury is 0.140 J/g⋅K.  How many joules of energy are needed to warm 4.52 g of mercury from 24.6 oC to 27.1 oC?
a)
0.632 J
b)
13.8 J
c)
3.96 J
d)
1.58 J
18.
Energy is measured in units of
a)
kelvin
b)
grams
c)
pounds
d)
joules
19.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

20.

What does q stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

21.

What does c stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

22.

Calculate ΔT\Delta T  when a substance goes from 10*C to 75*C

a)

-65*C

b)

75*C

c)

10*C

d)

65*C

23.

For an exothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

24.

For an endothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

25.

The specific heat of platinum is 0.133 J/g°C. How much heat is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

26.

What is the specific heat capacity of Water?

a)

4.184 J/g*C

b)

50.184 K/g*F

27.

What is the SI unit of heat and energy?

a)

calorie

b)

celsius

c)

joule

28.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

29.

According to Dalton's atomic theory, all matter is made of ________.

a)

Molecules

b)

Protons, neutrons, and electrons

c)

Atoms

d)

Subatomic particles

30.

Dalton proposed that all atoms of a given element are ________ in mass and properties.

a)

Different

b)

Similar

c)

Identical

d)

Varied

31.

Which part of Dalton's atomic theory had to be modified based on the discovery of subatomic particles and isotopes?

a)

All matter is made of atoms

b)

All atoms of a given element are identical in mass and properties

c)

Compounds are combinations of two or more different types of atoms

d)

A chemical reaction is a rearrangement of atoms

32.

Which scientist discovered the electron?

a)

Bohr

b)

Thomson

c)

Rutherford

d)

Dalton

33.

Whose model of the atom is pictured?

a)

Rutherford

b)

Thomson

c)

Dalton

d)

Bohr

34.

What did Rutheford discover about atoms?

a)

An atom is mostly empty space, but has a dense positively charged center (nucleus)

b)

An atom is always negatively charged

c)

An atom is always positively charged

d)

All particles will pass straight through gold foil with no change in path

35.

Who came up with the first atomic theory?

a)

Thomson

b)

Rutherford

c)

Dalton

d)

Schrodinger

36.

Rutherford did experiments to show -

a)

Neutrons are located in the nucleus

b)

Atoms are mostly empty space

c)

Atoms contain negative particles, now known as electrons

d)

Matter cannot be lost or gained

37.

The scientist credited for discovering the nucleus is -

a)

Dalton

b)

Chadwick

c)

Bohr

d)

Rutherford

38.

Which scientist used the Cathode Ray to discover the negatively charged particles in an atom?

a)

Bohr

b)

Rutherford

c)

Dalton

d)

Thomson

39.
What did Thomson discover?
a)
electron
b)
proton
c)
neutron
d)
electron cloud
40.
The Gold Foil experiment was done by __________.
a)
Chadwick
b)
Bohr
c)
Rutherford
d)
Thomson
41.

Positively charged atoms with electrons. "Plum pudding"

a)

Democritus

b)

Bohr

c)

Thomson

d)

Dalton

42.

Uncertainty principle - you can not determine an electron's speed and position at the same time.

a)

Ernest Rutherford

b)

Niels Bohr

c)

Werner Heisenberg

d)

Erwin Schrodinger

43.
Rutherford's gold foil experiment provided evidence that...
a)
Negative and positive charges are spread evenly throughout the atom.
b)
Alpha particles have a positive charge.
c)
Gold is not a dense as previously thought.
d)
There is a dense positively charged nucleus at the center of an atom.
44.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
45.
Ernst Rutherford discovered which part of the atom through the use of gold foil?
a)

Nucleus

b)
Neutron
c)
Electron
d)
Orbitals
46.

Who used the Cathode Ray Tube?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Erwin Schrodinger

d)

Niels Bohr

47.

Who created this model?

Plum Pudding Model

a)

JJ Thomson

b)

Ernest Rutherford

c)

John Dalton

d)

James Chadwick

48.

What did Rutherford discover in his experiment?

a)

nucleus

b)

electrons

c)

neutrons

d)

protons

49.

Which of the following statements best describes the Heisenberg Uncertainty Principle?

a)

It is impossible to know the exact position and momentum of an electron simultaneously.

b)

Electrons can only exist in certain discrete energy levels.

c)

Electrons orbit the nucleus in fixed paths.

d)

The energy of an electron is always uncertain.

50.

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

51.

The ability to attract an electron in a chemical bond

a)

electronegativity

b)

electron affinity

c)

metallic character

d)

ionization energy

52.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
53.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
54.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
55.
Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?
a)
Aluminum (Al)
b)
Chlorine (Cl)
56.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
57.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

58.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

59.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

60.

When you have Si-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

61.

When you have F-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

62.
The most electronegative atom in the periodic table is:
a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
63.
Which has the greater EN: 
H or F?
a)
H
b)
F
64.

A covalent bond usually forms between:

a)

a metal and a nonmetal

b)

either metals or nonmetals

c)

two metals

d)

two nonmetals

65.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
66.

(select 2) Atomic Radius increases as you move

a)

Down a Group

b)

Up a Group

c)

Left to Right across a Period

d)

Right to Left across a Period

67.

(select 2) Electronegativity energy increases as you move

a)

Down a Group

b)

Up a Group

c)

Left to Right across a Period

d)

Right to Left across a Period

68.

an ion with a positive charge

a)

anion

b)

cation

c)

nonmetals

d)

halogens

69.

an ion with a negative charge

a)

cation

b)

anion

c)

metals

d)

nonmetals

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