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Chemistry H Review Multiple Choice

Terms in this set (100)

Chemistry is the study of
matter and changes it undergoes
Matter
has mass and takes up space
Weight is a measure of the amount of matter and the effect of
gravity
Calculate the weight in Newtons of an object with mass equal to 5.0 x 10^5 g and the acceleration due to gravity of 98.0 x 10^-1 m/s^2. Recall Weight [Newtons] = mass [kg] x acceleration [m/s^2]
4,900 Newtons
An example of qualitative data
texture
An example of quantitative data
volume
A tentative explanation of what is observed
hypothesis
In an experiment, the variable the experimenter plans to change
independent variable
An explanation supported by many experiments
theory
Describes a relationship in nature that is supported by many experiments
scientific law
The practical use of scientific information
technology
Which is NOT a base SI unit
A) temperature- degrees kelvin
B) time- seconds
C) length- meters
D) Amount of substance- pounds
D) Amount of substance- pounds
Which is NOT a unit for volume
A) kilometer (km)
B) cubic decimeter (dm^3)
C) liter (L)
D) cubic centimeter [CC] (cm^3)
A) kilometer (km)
1 x 10^-3 kg is equal to
1 g
Find the density in units of (g/cm^3) of a substance with a mass of 250 mg occupying a volume of 250 mm^3
1 g/cm^3
Find the volume in units of m^3 of a cube with dimensions 1 x 10^2 cm on a side.
1 m^3
Chemist found that a complex reaction occurred in three steps. The first step takes 2.5731 x 10^2 s to complete, the second step takes 3.60 x 10^-1 s, and the third step takes 7.482 x 10^1 s. The total amount of time elapsed during the reaction is
3.3249 x 10^2 s
Sodium (Na) reacts with water (H2O) to produce a metallic hydroxide (NaOH) and hydrogen (H2) gas as follows:
2Na (s) + 2H2O (l) --> 2NaOH (aq) + H2 (g)

For the reaction above, 112.2 grams of Sodium (2Na) combine with 87.8 grams of water (2H2O). What is the total Mass of the reactants and the Mass of Hydrogen gas (H2) that forms given the Mass of Sodium Hydroxide (2NaOH) that forms is 195 grams
mass of reactants is 200 grams; mass of H2 gas is 5 grams
The percentage by mass (%) of the elements is as follows:
Sodium (Na) = 57.5%
Oxygen (O) = 40.0%
Hydrogen (H) = 2.5%
The mass of each element is
Na = 57.5 grams, O = 40.0 grams, and H = 2.5 grams
Matter that has uniform and definite composition
A) additive
B) heterogeneous mixture
C) chemical
D) none
D) none
Identify the heterogeneous mixture
A) oil & water
B) air
C) tap water
D) salt and water
A) oil & water
Matter that has uniform and unchanging composition
substance
Example of extensive property
mass
Example of intensive property
density
The ability of a substance to combine with or change into one or more other substances
chemical property
Three states of matter
solid, liquid, gas
Find the percent by mass of sulfur in sulfuric acid, H2SO4, where the atomic mass of hydrogen (H) = 1.008, the atomic mass of sulfur (S) = 32.065, and the atomic mass of Oxygen (O) = 15.999
32.69%
Calculate the mass in kilograms of a gold (Au) bar with the following dimensions: length = 30.5 cm, width 10.15 cm, and height 7.6 cm. The density of gold (Au) is 19,000 kg/m^3
44.7 kg
States that mass is neither created nor destroyed during a chemical reaction
law of conservation of mass
Regardless of the amount, a compound is always composed of the same elements in the same proportion by mass
law of definite proportions
Identify three subatomic particles
protons, electrons, neutrons
The number of protons in an atom is referred to as the element's
atomic number
The atomic number is
equal to the number of electrons = protons
Atoms with the same number of protons but different numbers of neutrons
isotope
Mass number is
equal to atomic number + neutrons
Calculate the weighted average atomic mass for chlorine (Cl), where the first isotope of chlorine has an atomic mass = 34.969 amu and percent abundance = 75.77% and the second isotope of chlorine has an atomic mass = 36.966 amu and percent abundance = 24.23%
35.453 amu
The unstable nuclei isotope Cobalt (Co) - 60 (atomic number = 27) will decay to Nickel (Ni) - 60 (atomic number = 28) by emitting
beta particle
Spontaneous emission of radiation
radioactivity
Reactions that involve an atom of one element changing into an atom of another element
nuclear reaction
The smallest particle of an element that retains the properties of the element
atom
Form of energy that exhibits wavelike behavior as it travels through space
electromagnetic radiation
The laser in a compact disc (CD) player uses light with a wavelength of 780 nm. What is the frequency of this light?
3.8 x 10^14 Hz
What is the energy of a photon of red light having a frequency of 4.48 x 10^14 Hz?
2.97 x 10^-19 J
Calculate the de Broglie wavelength of an object with mass of 257.4102 kg and velocity of 2.574102 x 10^8 m/s.
1 x 10^-44 m
Electrons in the outermost orbital
valence electrons
States that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time
Heisenberg uncertainty principle
The valence band of noble gases satisfy the
octet rule
The trend in atomic radii as you move from left-to-right across a row of elements in the Periodic Table of Elements
generally decreases
Statement that atoms tend to gain, lose, or share electrons to acquire a full set of eight valence electrons
octet rule
The modern Periodic Table of Elements arranges the elements in the following order
increasing atomic number
Most of the elements in groups 6A-8A are classified as
nonmetals
Describes the periodic repetition of the chemical and physical properties of the elements within the Periodic Table of Elements
periodic law
If groups identify the number of valence electrons, periods identify
orbital energy level
Columns in the Periodic Table of Elements
groups
Rows in the Periodic Table of Elements
periods
Group B elements
transition elements
The number of electrons in an octet
8
Elements with similar properties
A) sodium and bromine
B) lithium and sodium
C) carbon and oxygen
D) potassium and helium
B) lithium and sodium
Moving down a column of the Periodic Table of Elements, the first ionization energy
generally decreases
A force that holds two atoms together
chemical bond
Electrostatic force that holds oppositely charged particles together in an ionic compound
ionic bond
The simplest ratio of ions represented in an ionic compound
formula unit
An ionic compound whose aqueous solution conducts an electric current
electrolyte
An ionic compound containing a metal cation and a nonmetal anion
salt
The charge of a monatomic ion
oxidation number
A polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms
oxyanion
Ions made up of more than one atom
polyatomic ions
A one atom ion
monatomic ion
Name the ionic compound NaBr
sodium bromide
Name the ionic compound Ag2CrO4 where the ion [CrO4^2-] is chromate
silver chromate
Name the ionic compound Cu(NO3)2 where the ion [NO3^1-] is nitrate
copper II nitrate
A chemical bond that results from the sharing of electrons
covalent bond
Formed when two or more atoms bond covalently
molecule
Occurs when more energy is released forming new bonds than is required to break bonds in the initial reactants
exothermic reaction
Use electron-dot diagrams to show how electrons are arranged in molecules
Lewis structure
Values assigned by Linus Pauling comparing the abilities of atoms to attract shared electrons with the ability of fluorine to do so
electronegativity
A bond with unequal sharing of electrons
polar covalent bond
The weak forces of attraction between individual molecules
van der Waals forces
Type of bond that will form between H (electronegativity = 2.20) and S (electronegativity = 2.58)
non-polar covalent bond
Type of bond that will form between Na (electronegativity = 0.93) and Cl (electronegativity = 3.16)
ionic bond
Which of the following diatomic gases has the shortest bond length?
A) HI
B) Cl2
C) N2
D) O2
C) N2
Name the binary covalent compund CCl4
carbon tetrachloride
Name the binary covalent compound H2O
dihydrogen monoxide
Name the acid H2SO4 where [SO4^2-] is sulfate
sulfuric acid
Name the acid HCl
hydrochloric acid
Identify the type of reaction: 4C5H9O + 27O2 --> 20 CO2 + 18 H2O
combustion
Identify the type of reaction: 2NH3 + H2SO4 --> (NH4)2SO4
synthesis
Identify the type of reaction: Li3N + 3NH4NO3 --> 3LiNO3 + (NH4)3N
double replacement
Identify the type of reaction: 3Pb + 2H3PO4 --> 3H2 + Pb3(PO4)2
single replacement
Identify the type of reaction: 2NaClO3 --> 2NaCl + 3O2
decomposition
Identify the coefficients that balance the equation:
__ HNO3 (aq) + __ KHCO3 (aq) --> __ H2O (l) + __ CO2 (g) + __ KNO3 (aq)
1, 1, 1, 1, 1
Identify the type of product for the reaction in aqueous solution:
3H2S (aq) + 2FeBr3 (aq) --> 6HBr (aq) + Fe2S3 (s)
precipitate
Identify the coefficients that balance the equation:
__ HI (aq) + __ Li2S (aq) --> __ H2S (g) + __ LiI (aq)
2, 1, 1, 2
Determine the number and type of representative particle in 11.5 mol C (carbon)
6.923 x 10^24 atoms
Determine the number and type of representative particle in 0.15 mol of the ionic compound CaCl2
9.03 x 10^22 formula units
Determine the mass of 2.0 mol of copper (Cu), with = 63.546 amu
127.092 g
Determine the mass in grams of 10,500 mg C12H22O11 (Sucrose)
10.5 g
Find the percent copper contained in CuFeS2, where the amu of Cu, Fe, and S are 63.546, 55.845, and 32.065 respectively
34.626%
Find the percent water contained in the hydrate calcium chloride dihydrate (CaCl2 · 2H2O), where the amu of Ca, Cl, H, and O are 40.078, 35.453, 1.008, and 15.999 respectively
24.51%
Name the hydrate Cu(II)SO4·5H2O
copper (II) sulfate pentahydrate
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