Honors Chemistry Midterm Review
The measurement 0.035550 g rounded off to two significant figures would be *
0.036 g
What group are alkali metals located in?
1
A volume of 1 milliliter is equivalent to *
1 cubic centimeter
How many centigrams are in 104 grams?
10400 cg
Solve for the following [ remember to use the correct significant figures and to include the unit] (120 cm² + 3.5 cm²) - 18 cm² = *
106 cm²
To eject one electron from the valence shell of copper, 1.20 x 10⁻¹⁷ J is needed. What is the wavelength of light required to eject the electron?
16.6 nm
What group are halogens located in?
17
What group are noble gases located in?
18
How many significant figures are in the number 0.085 ?
2
What group are alkaline earth metals located in?
2
Solve for the following [ remember to use the correct significant figures and to include the unit] 12.0 m + 5.28 m + 10.5 m = *
27.8 m
How many significant figures are in the number 0.00860?
3
If 4.0 g of element A combine with 10. g of element B, then 12 g of element A combine with ____ g of element B. *
30
32 grams of pure gold are taken out of a jeweler's heating bath at a temperature of 180 °C. The gold cools to room temperature of 21 °C. The specific heat of gold is 0.129 J/g⋅°C. What is the mass of the equation?
32 g
How many joules of heat are needed to increase the temperature of 19.3 g of lead from 22 °C to 41 °C? (Specific heat of lead = 0.128 J/g⋅°C)
47 J
Which portion of the graph indicates the presence of only a gas? *
5. E
Solve for the following [ remember to use the correct significant figures and to include the unit] 2.7 kg to pounds (lbs.) (1 kg = 2.2 lbs.) *
5.9 lbs.
Convert 486.0 °F to Kelvin.
525.2 K
Perform the following calculation and report your answer with the correct number of significant figures: 97.57 − 38.799 = _____.
58.77
32 grams of pure gold are taken out of a jeweler's heating bath at a temperature of 180 °C. The gold cools to room temperature of 21 °C. How much heat is given up to the surroundings? The specific heat of gold is 0.129 J/g⋅°C.
660 J
Which represents a neutral atom acquiring an electron in a process where energy is released?
A + e- → A- - energy
Which compound would evaporate the fastest under the same atmospheric conditions?
Acetone
What element is this [Ne] 3s² 3p⁶
Argon
Which of the following statements is true according to modern atomic theory? *
Atoms of the same element may have different masses.
What unit is this [Ar] 4s²
Ca
The ionization energies required to remove successive electrons from one mole of calcium atoms are 590 kJ/mol, 1145 kJ/mol, 4912 kJ/mol, and 6474 kJ/mol. The most common ion of calcium is
Ca2+
What element is this [Ne] 3s² 3p⁵
Cl
Which element has the electron configuration of 1s²2s²2p⁵?
Fluorine
What element is this? 1s^2
Helium
What happens to the energy in a substance when it changes state? *
It changes form.
Which of these statements about units of measurement is NOT true? *
Measurements can be compared without knowing their units.
Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?
The number of energy levels increase.
What is the electron configuration of phosphorous?
[Ne] 3s² 3p³
A mixture is *
a physical blend of any two or more kinds of matter.
A compound is *
a substance, made of two or more atoms that are chemically bonded, that can be broken down into simpler, stable substances.
A piece of metal has a mass of 4.09 g and a volume of 17.04 cm³. What is its density?
a) 0.2400 g/cm³
What happens to the temperature as a substance reaches its melting point?
a) The temperature remains constant during the phase change
Whenever a liquid changes to a vapor, it *
absorbs energy from its surroundings.
Which of the following is an example of a homogeneous mixture? *
air
A solid substance is *
always the same shape regardless of its container.
Compared to the alkali metals, the alkaline-earth metals
are less reactive.
One-half the distance between the nuclei of identical atoms that are bonded together is called the
atomic radius.
Because most particles fired at metal foil passed straight through, Rutherford concluded that *
atoms were mostly empty space.
Green light has a wavelength of 532 nm. How much energy does each photon have? (h =6.626 x 10⁻³⁴ J⋅s, c = 2.998 x 10⁸ m/s)
b) 3.73×10⁻¹⁹ J
Which of the following has the largest atomic radius?
bismuth
Which of the following is not a physical change? *
burning
Which of the following temperatures is impossible?
c) -481.0 °C
If a liquid boils at 158 °F. What is the temperature of the boiling liquid in Celsius?
c) 70.0 °C
What do the electron configurations of zinc, cadmium, and mercury have in common?
c) Their valence electrons completely fill the s and d orbitals.
B. rust forming on a car *
chemical
D. digestion of food in the stomach
chemical
Which of the following is an example of a heterogeneous mixture? *
chocolate chip cookie
If two or more compounds are composed of the same two elements, the ratio of the masses of one element that combine with a fixed mass of the other element is a simple whole number. This is a statement of the law of *
conservation of mass.
How many cubic centimeters are in 1250 milliliters?
d) 1250 cm³
The yellow/orange light given off by a street light has a frequency of 4.82 x 10¹⁴ Hz. What is the wavelength of this light? (h =6.626 x 10⁻³⁴ J⋅s, c = 2.998 x 10⁸ m/s)
d) 622 nm
How much liquid is in this 100 mL graduated cylinder?
d) 71.6 mL
What is electron spin?
d) A quantum property that allows two electrons to share an orbital or sub-orbital because they do not have the same quantum state.
What is the SI unit of energy?
d) Joules (J)
Which element would you expect to have similar properties to calcium?
d) strontium.
In a row in the periodic table, as the atomic number increases, the atomic radius generally
decreases
Which of the following do solids share with liquids? *
definite volume
A photon with a frequency of 2.10 × 10¹⁴ Hz has an energy of which of the following?
e) 1.39×10⁻¹⁹ J
Blue light has a frequency of 6.15×10¹⁴ Hz. How much energy does each photon have? (h =6.626 x 10⁻³⁴ J⋅s, c = 2.998 x 10⁸ m/s)
e) 4.07×10⁻¹⁹ J
Experiments with cathode rays led to the discovery of the *
electron
A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called
electron affinity
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. *
equal to
Which term best describes the process by which particles escape from the surface of a non‐boiling liquid and enter the gas state? *
evaporation
The element that has the greatest electronegativity is
fluorine
Which of these SI units is used to measure mass? *
g
As you move left to right in Period 4 from gallium through bromine, atomic radii
generally decrease. .
As you move down Group 14 in the periodic table from carbon through lead, atomic radii
generally increase
How does the energy required to remove an electron from an atom change as you move left to right in Period 4 from potassium through iron?
generally increases.
A physical change occurs when a *
glue gun melts a glue stick.
In the alkaline-earth group, atoms with the smallest radii
have the highest ionization energies.
The liquid state of matter can be described as *
having a definite volume but not a definite shape.
Which of the following causes particles in a liquid to escape into a gas state? *
high kinetic energy
If a mixture is uniform in composition, it is said to be *
homogeneous
If a mixture is uniform throughout, it is called *
homogeneous.
As the atomic number of the metals of Group 1 increases, the ionic radius
increases
For each successive electron removed from an atom, the ionization energy
increases
Within a group of elements, as the atomic number increases, the atomic radius
increases
The energy required to remove an electron from an atom is the atom's
ionization energy
The symbols for units of length in order from largest to smallest are *
km, m, cm, mm.
During the process of freezing, a liquid *
loses kinetic energy.
All of the following are examples of SI units EXCEPT *
mass
Which of the following is not a chemical change? *
melting
In Rutherford's experiments, most of the particles *
passed through the foil.
breaking glass
physical
ice melting
physical
If repeated measurements agree closely with each other but differ widely from the accepted value, the measurements are *
precise, but not accurate.
The following values were recorded as the mass of products when a chemical reaction was carried out three separate times: 8.83 g; 8.84 g; 8.82 g. The mass of products from that reaction is 8.50 g. The recorded values are *
precise, but not accurate.
Elements in a group or column in the periodic table can be expected to have similar
properties
While a substance is boiling, the temperature of the liquid *
remains constant.
A numerical result is said to have good precision if *
repeated measurements agree closely.
Because a few alpha particles bounced back from the foil, Rutherford concluded that they were *
repelled by densely packed regions of positive charge.
What is the process of a substance changing from a solid to a vapor without passing through the liquid phase? *
sublimation
The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates that
the noble gas configuration has been reached.
The periodic law states that
the physical and chemical properties of the elements are functions of their atomic numbers.
When multiplying or dividing numbers, the answer should be rounded so that it has *
the same number of significant figures as the value with the fewest significant figures.
Under ordinary conditions of temperature and pressure, the particles in a gas are *
very far from one another.
