CHEMISTRY 1ST SEMESTER EXAM
REVIEW
1. A measure of the quantity of matter is
MASS
2. List a process that is a physical change.
CUTTING, GRINDING, TEARING
3. List a process that is a chemical change?
BURNING
4. A chemical change occurs when
MOLECULES ARE REARRANGED TO FORM A
NEW COMPOUND
5. A physical change occurs when a
MOLECULES ARE MOVED AROUND, BUT ARE
STILL MADE OF THE SAME COMPONENTS
6. A state of matter in which a material has no definite
shape but has a definite volume is the ____ state.
LIQUID
7. Under ordinary conditions of temperature and
pressure, the particles in a gas are
RANDOMLY SPREAD FAR APART
8. The liquid state of matter can be described as
HAVING A DEFINED VOLUME BUT
NO DEFINED SHAPE
9. A solid substance is
STATE OF MATTER WITH A DEFINED
SHAPE AND DEFINED VOLUME
10. If a mixture is uniform in composition, it is said to
be HOMOGENEOUS
11. If a mixture is not uniform throughout, it is called
HETEROGENEOUS
12. The quantity of matter per unit volume is
DENSITY
13. The relationship/equation between the mass m of
a material, its volume V, and its density D is
D = M/V
14. The density of aluminum is 2.70 g/cm3. What is
the mass of a solid piece of aluminum with
a volume of 1.50 cm3? 4.05 G
15. A sample of gold has a mass of 96.5 g and a
volume of 5.00 cm3. The density of gold is
19.3 G/CM3
16. The density of pure diamond is 3.5 g/cm3. What is
the volume of a diamond with a mass of 0.25 g?
.07 CM3
17. How many significant figures are in 0.202grams?
THREE
18. How many significant figures does 30.00 have?
FOUR
19. The speed of light is 300 000 km/s. Rewrite this in
scientific notation.
3.0 X 105
20. The average distance between the Earth and the moon is
386 000 km. Rewrite this in scientific notation.
3.86 X 105
21. In oxides of nitrogen, such as N2O, NO, NO2, and N2O3,
atoms combine in small whole-number ratios. this evidence
supports the law of
MULTIPLE PROPORTIONS
22. If two or more compounds are composed of the same two
elements, the ratio of the masses of one element that
combines with a fixed mass of the other element is a simple
whole number. This is a statement of the law of
MULTIPLE PROPORTIONS
23. Oxygen can combine with carbon to form two compounds, carbon
monoxide and carbon dioxide. The ratio of the masses of oxygen that
combine with a given mass of carbon is 1:2 This is an example of:
MULTIPLE PROPORTIONS
24. According to the law of definite proportions, any two samples of KCl
have
EQUAL/DEFINED PROPORTIONS OF K TO Cl
25. According to the law of conservation of mass, when sodium,
hydrogen, and oxygen react to form a compound, the mass of the
compound is _____ the sum of the masses of the individual elements.
THE SAME AS
26. An atom is electrically neutral because:
IT HAS EQUAL PROTONS(+) AND ELECTRONS (-)
27. The number of atoms in one mole of carbon is
6.022 x 1023
28. Avogadro’s number represents what amount?
The number of molecules in a mole
29. How many moles are in 15 grams of Lithium?
2.16 moles
30. How many grams are in 3.3 moles of Potassium Sulfide,
K2S?
363.86 grams
31. How many molecules are in 52 grams of CO?
1.12 x 1024
32. What is the mass of 3.01x1023 molecules of Fe2O3?
79.8 grams
33.The statement that an electron occupies the lowest available
energy orbital is what law/principle?
THE AUFBAU PRINCIPLE
34.“Orbitals of equal energy are each occupied by one electron
before any is occupied by a second electron, and all electrons in a
singly occupied orbital must have the same spin” is a statement of
what law/principle?
HUND’S RULE
35.The statement that no two electrons in the same atom can
have the same four quantum numbers is what law/principle?
PAULI’S EXCLUSION PRINCIPLE
36.Which rule requires that each of the P orbitals at a particular
energy level receive one electron before any of them can have two
electrons?
HUND’S RULE
37. The sequence in which energy levels are filled is
specified by what law/principle?
THE AUFBAU PRINCIPLE
38. The Aufbau Principle states that an electron
FILLS UP THE LOWEST ENERGY LEVEL FIRST,
THEN BUILDS UP
39. The Pauli Exclusion Principle states that no two
electrons in the same atom can
HAVE THE SAME SET OF QUANTUM NUMBERS,
& CAN’T BE IN THE SAME PLACE AT SAME TIME
40. What is the correct order of atomic orbitals filled
according to the Aufbau Principle?
1S, 2S, 2P, 3S, 3P, 4S, 3D, 4P
41.The element with electron configuration 1s22s22p63s23p2 is
SILICON, Si
42.The electron configuration for the Carbon atom, C, is
1s22s22p2. The atomic number of Carbon is
6
43.What is the electron configuration for Nitrogen, N atomic
number 7?
1S22S22P3
44.The electron configuration for Aluminum, Al, atomic
number 13 is
1S22S22P63S23P1
45. Write the correct electron configuration for Fluorine:
1s22s22p5
46. Which element has the following electron configuration:
1s22s22p63s23p64s23d8? NICKEL, Ni
47. Which element has the following electron configuration: [Ne]3s1?
SODIUM, Na
48. The higher the frequency of a wave, the ________ the energy of
that wave.
HIGHER
49. The higher the wavelength of a wave, the __________ the energy of
the wave.
LOWER
50. This individual is responsible for the organization of one of the first
periodic tables which was organized based on the atomic mass of the
known elements.
DIMITRI MENDELEEV
51. This individual is responsible for organization of the present day
periodic table which is based on the increasing number of protons in the
nucleus.
HENRY MOSELEY
52.What is the group of radioactive elements called with the
atomic numbers from 90 to 103?
ACTINIDES
53.The elements with atomic numbers from 58 to 71 are
called? LANTHANIDES
54. Argon, Krypton, and Xenon are all examples of what
group of elements?
NOBLE GASES
55. The periodic law states that
THE PHYSICAL AND CHEMICAL PROPERTIES OF THE
ELEMENTS ARE FUNCTIONS OF THEIR ATOMIC NUMBERS
56. Elements in a group or column in the periodic table can
be expected to have similar
PROPERTIES
57. The elements in Group 1 are also known as the
ALKALI METALS
58. The most reactive group of nonmetals are the
HALOGENS
59. The soft, silvery, reactive metals, all of which have
one electron in its s orbital is known as the
ALKALI METALS
60. The most characteristic property of the noble
gases is that they are
UNREACTIVE
61.A measure of the ability of an atom in a chemical compound to
attract electrons from another atom in the compound is called
ELECTRONEGATIVITY
62.When an electron is acquired by a neutral atom, the energy is called
ELECTRON AFFINITY
63.As you move down a group of elements you expect to see the
atomic radii
INCREASE
64. Across a period in the period table, ionic radii
DECREASES
65. Groups 1-2 and 13-18 are known as this
MAIN GROUP ELEMENTS
66.What is the correct block, period and group for the
element with the electron configuration [Kr]5s2 ?
BLOCK: S PERIOD: 5 GROUP: 2
67. What are the 2 main types of bonds that we have learned
about so far? COVALENT AND IONIC
68.During an ionic bond, valence electrons are____
TAKEN OR GIVEN AWAY
69. During a covalent bond, valence electrons are_____
SHARED
70.What periodic trend can be used to determine the type of
bond that elements will form?
ELECTRONEGATIVITY
71. When using the electronegativity difference method,
what amounts correspond to what bonds?
Nonpolar Covalent: 0.0-0.3,
Polar Covalent: 0.3-1.7,
Ionic: 1.7-4.0
72. If Sodium, Na, was to bond with Chlorine, Cl, what type of
bond would they form?
IONIC
73. If Bromine, Br was to bond with Chlorine, Cl, what type of
bond would they form?
NONPOLAR COVALENT
74. If Hydrogen, H was to bond with Oxygen, O, what type of
bond would they form?
POLAR COVALENT
STUDY HARD, AND AS ALWAYS,
MAY THE ODDS BE EVER IN YOUR FAVOR