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Chemistry: First Semester Final

Total questions: 67

Worksheet time: 1hrs 11mins

Name
Class
Date
1.
1. The scientific method is...
a)
gathering information through observation and using it to form theories.
b)
the rules science follows to gain information and understanding.
c)
what is used in high school labs.
d)
important but seldom actually used in modern science.
2.
2. Chemistry is...
a)
the study of matter, its composition, properties, and reactions.
b)
the study of matter and energy and how they interact.
c)
the study of Earth's composition, history, and structure.
d)
the study of forces and the changes they produce.
3.
3. The SI system is based on the _?_ system.
a)
French
b)
English
c)
SAE
d)
metric
4.
4. Matter is...
a)
the amount of mass a body has.
b)
the ratio of mass to volume.
c)
anything with mass and volume.
d)
anything capable of producing change, heat, or doing work.
5.
5. In a chemical change...
a)
the appearance changes but the identity of the material remains the same.
b)
new substances are created.
c)
the mass after the change is greater than the mass before the change.
d)
heat is given off.
6.
6. An electron is...
a)
a subatomic particle with a mass of 1 amu and a positive charge.
b)
a subatomic particle with a mass of 1 amu and no charge.
c)
a subatomic particle with almost no mass and a negative charge.
d)
none of these.
7.
7. Carbon-12 & carbon-14 are two different _?_ of carbon.
a)
ions
b)
states
c)
isotopes
d)
carbides
8.
8. 1s^2 2s^2 2p^3 is the neutral electron configuration of...
a)
neon
b)
phosphorus
c)
nitrogen
d)
not enough information is given.
9.
9. "When the elements are arranged by atomic number they show a period trend in their properties."
a)
Law of Conservation of Energy
b)
Law of Definite Proportions
c)
Dalton's Atomic Theory
d)
Periodic Law
10.
10. The s-block elements are...
a)
also called the transition metals.
b)
the two rows at the bottom of the periodic table.
c)
columns 1 & 2.
d)
another name for the halogens.
11.
11. A(n) _?_ bond is held together by the attractive force between a cation and anion.
a)
ionic
b)
covalent
c)
metallic
d)
hydrogen
12.
12. Energy is...
a)
measured in newtons (N).
b)
the study of forces and the changes they produce.
c)
measured in Kelvin (K).
d)
the ability to cause change, produce heat, or do work.
13.
13. In the SI, heat is measured in...
a)
Kelvin
b)
Celsius
c)
Joules
d)
calories
14.
14. A combination of non-bonded pure substances which cannot be separated by simple mechanical means is a(n)...
a)
ionic compound
b)
molecular compound
c)
homogeneous mixture
d)
heterogeneous mixture
15.
15. A change in the number of electrons in an atom produces a(n)...
a)
isotope
b)
different element
c)
ion
d)
radioactive substance
16.
16. What is the difference between uranium-235 and uranium-238?
a)
3 neutrons
b)
3 protons
c)
uranium-235 is radioactive -238 is stable
d)
Uranium-238 is radioactive -235 is stable.
17.
17. A single s-orbital can hold _?_ electron(s).
a)
1
b)
2
c)
3
d)
4
18.
18. The periodic table has _?_ periods.
a)
18
b)
7
c)
32
d)
9
19.
19. In the IUPAC periodic table, the halogens are located in group...
a)
1
b)
VII A
c)
17
d)
VII B
20.
20. In a single covalent bond, how many electrons are shared?
a)
Only 1
b)
2
c)
4
d)
Electrons aren't shared in covalent bonds.
21.
21. A bond in a molecule like O2 will be...
a)
ionic
b)
polyatomic ions
c)
polar covalent.
d)
nonpolar covalent
22.
22. Element X is explosive in oxygen and so is element Y. Element X & Y are most likely:
a)
in the same column
b)
in the same row
c)
radioactive
d)
noble gases.
23.
23. The _?_ orbitals are shaped like clover leaves.
a)
s
b)
p
c)
d
d)
f
24.
24. An isotope is...
a)
an atom of an element with a different number of neutrons.
b)
an atom with an overall charge.
c)
a radioactive element.
d)
another name for the metalloids.
25.
25. Which particle(s) are located in the nucleus of the atom?
a)
protons & electrons
b)
protons & neutrons
c)
electrons and neutrons
d)
only portons
26.
26. If you change the number of protons in an atom then...
a)
you change isotopes
b)
you change ions
c)
you make the atom unstable.
d)
you change elements.
27.
27. An object is heated until it becomes liquid. This is an example of a...
a)
physical change.
b)
chemical change.
c)
chemical reaction.
d)
none of the above
28.
28. The SI system measures temperature in...
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
Roentgen
29.
29. Even though it is not an SI unit, _?_ is commonly used world-wide.
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
All of these are SI units.
30.
30. A blend of two or more substances where each substance retains its identity.
a)
molecular substance
b)
ionic substance
c)
mixture
d)
polyatomic ion
31.
31. Who is given credit for the discovery of the electron?
a)
Thomson
b)
Bohr
c)
Rutherford
d)
Dalton
32.
32. Who is given credit for the discovery of the nucleus?
a)
Thomson
b)
Bohr
c)
Rutherford
d)
Dalton
33.
33. Who used the orbital model of the hydrogen atom to explain emission spectra?
a)
Thomson
b)
Bohr
c)
Rutherford
d)
Dalton
34.
34. Which of the following is not true about fluorine (F)?
a)
It is a halogen
b)
It is a nonmetal
c)
It is the most electronegative element
d)
It is chemically inert.
35.
35. The elements of group IA are called the...
a)
Alkali metals.
b)
Alkaline Earth Metals.
c)
Halogens
d)
Noble Gases
36.
36. If an element of column 1 is paired with an element of column 17 the result is most likely...
a)
a molecular substance.
b)
a polar covalent bond
c)
an ionic compound
d)
a polyatomic ion.
37.
37. Which scientist showed that mass is always conserved in chemical reactions?
a)
Galileo
b)
Joule
c)
Lavoisier
d)
Kelvin
38.
38. A positively charged ion is called a(n)...
a)
anion
b)
cation
c)
monatomic ion.
d)
polyatomic ion.
39.
39. A compound that can absorb water molecules into its solid structure is called a(n)...
a)
ionic compound
b)
molecule
c)
hydrate
d)
polar molecule
40.
40. As you move from left to right across a row on the periodic table, the electronegativity generally...
a)
increases
b)
decreases
c)
stays the same
d)
has no predictable pattern.
41.
41. The region around an atom where an electron is likely found is called a(n)...
a)
orbital
b)
quantum energy level
c)
sublevel
d)
Bohr radius
42.
42. In the SI, energy is measure in...
a)
calories
b)
joules
c)
Kelvin
d)
Celsius
43.
43. Calcium is a member of...
a)
the alkali metals
b)
the alkaline Earth metals
c)
the halogens
d)
the noble gases
44.
44. The 4th quantum energy level can hold _?_ electrons.
a)
2
b)
18
c)
4
d)
32
45.
45. The _?_ orbitals are dumbbell shaped.
a)
s
b)
p
c)
d
d)
f
46.
46. Uranium is in the section of the periodic table where the f-orbital of the _?_ quantum energy level is being filled.
a)
4th
b)
5th
c)
6th
d)
7th
47.
47. Because of the Pauli Exclusion Principle, one orbital can hold a maximum of _?_ electrons.
a)
one
b)
two
c)
eight
d)
it depends on if it is an s, p, d, or f orbital.
48.
48. In the third quantum energy level, there are _?_ d-orbitals.
a)
two
b)
three
c)
four
d)
five
49.

This will be an essay question on the final. You will need to be able to answer this in the RACE format.

The Rutherford and Bohr models of the atom are commonly how people imagine the atom. Explain each model. Explain why each person made their changes.

4 lines
50.

If an object has a density of 5.25 g/ml and a volume of 38 ml, what is its mass? Express your answer with the proper number of significant digits.

a)

2.0E2 grams

b)

200 grams

c)

199.5 grams

d)

199.50 grams

51.

6429Cu1+ has ? protons, ? neutrons, and ? electrons.

(a)  

52.

199F1- has ? protons, ? neutrons, and ? electrons.

(a)  

53.

21084Po undergoes alpha decay. Select the correct decay formula.

a)

21084Po --> 42He + 20682Pb

b)

21084Po + 42He --> + 21486Rn

c)

21084Po --> 0-1 e + 21085At

d)

21084Po + 0-1 e --> 21083Bi

54.

Write out the electron configuration of nickel. (put a space between each suborbital and the number of the exponent. You don't need to enter them as exponents on here, but you will on the exam)

(a)  

55.

Write out the electron configuration of bromine. (put a space between each suborbital and the number of the exponent. You don't need to enter them as exponents on here, but you will on the exam)

(a)  

56.

Write out the abbreviated electron configuration of bismuth. (put a space between each suborbital and the number of the exponent. You don't need to enter them as exponents on here, but you will on the exam)

(a)  

57.

What is the name of the ionic compound NaHCO₃?

(a)  

58.

What is the name of the ionic compound Cu₂O? (use capital i's for roman numerals)

(a)  

59.

What is the formula for Iron (III) oxide? (Type the numbers for subscripts on here. Just remember that they need to be subscripts on the exam.)

(a)  

60.

What is the formula for tin (IV) sulfate? (Type the numbers for subscripts on here. Just remember that they need to be subscripts on the exam.)

(a)  

61.

What is the formula for carbon disulfide? (Type the numbers for subscripts on here. Just remember that they need to be subscripts on the exam.)

(a)  

62.

What is the formula for diphosphorus tetroxide? (Type the numbers for subscripts on here. Just remember that they need to be subscripts on the exam.)

(a)  

63.

What is the name of the covalent compound CO₂?

(a)  

64.

What is the name of the covalent compound N₂O₄?

(a)  

65.

What is the name of the acid H₂SO₄?

(a)  

66.

What is the name of MgCl₂•6H₂O?

(a)  

67.

There will be a paragraph response on the final.
The Rutherford and Bohr models of the atom are commonly how people imagine the atom. Explain each model. Explain why each person made their changes.

4 lines

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7th Grade - University