Chemistry Quarter 1 Exam
In Group 2 elements, the valence electrons are in sublevel a. d. b. p. c. s. d. f.
c
Just be able to identify periods bc there are a lot of questions i didn't copy over about that
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Which part of the illustration below shows the particles in a heterogeneous mixture? (Image)
Image shows squares and circles. The squares and circles are separated into multiple clumps.
A positively charged particle with mass 1.673 x 10^-24 g is a(n) a. proton. b. neutron. c. electron. d. positron.
a
A prospector finds 39.39 g of pure gold (atomic mass 196.9665 amu). She has a. 1.204 x 10^23 atoms of Au. b. 2.308 x 10^23 atoms of Au. c. 4.306 x 10^23 atoms of Au. d. 6.022 x 10^23 atoms of Au.
a
A state of matter in which a material has no definite shape but has a definite volume is the ____ state. a. gas b. liquid c. plasma d. solid
a
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. a. equal to b. greater than c. less than d. either greater than or less than
a
Across a period in the periodic table, atomic radii a. gradually decrease. b. gradually decrease, then sharply increase. c. gradually increase. d. gradually increase, then sharply decrease.
a
Across a period, ionization energies of d-block elements generally a. increase. b. decrease. c. remain constant. d. drop to zero.
a
An atom is a. the smallest unit of matter that maintains its chemical identity. b. the smallest unit of a compound. c. always made of carbon. d. smaller than an electron.
a
As you move down Group 14 in the periodic table from carbon through lead, atomic radii a. generally increase. b. generally decrease. c. do not change. d. vary unpredictably.
a
Because any element used in the cathode produced electrons, scientists concluded that a. all atoms contained electrons. b. only metals contained electrons. c. atoms were indivisible. d. atoms carried a negative charge.
a
Because most particles fired at metal foil passed straight through, Rutherford concluded that a. atoms were mostly empty space. b. atoms contained no charged particles. c. electrons formed the nucleus. d. atoms were indivisible.
a
Dalton incorporated the law of conservation of mass into his atomic theory by asserting that a. atoms are indivisible. b. atoms of different elements have different properties. c. matter is composed of atoms. d. atoms can be destroyed in chemical reactions.
a
Elements in which the d-sublevel is being filled have the properties of a. metals. b. nonmetals. c. metalloids. d. gases.
a
For elements in groups 1, 2, and 18, the increase in atomic number for successive elements follows the pattern 8, 8, 18, ?, 32. What number completes the pattern? a. 18 b. 20 c. 24 d. 26
a
If a mixture is uniform in composition, it is said to be a. homogenous b. chemically bonded c. heterogeneous d. a compound
a
In a glass tube attached to a voltage source, electric current passes from the negative electrode, called the ____, to the other electrode. a. cathode b. anode c. electron d. millikan
a
One-half the distance between the nuclei of identical atoms that are bonded together is called the a. atomic radius. b. atomic diameter. c. atomic volume. d. electron cloud.
a
Protons within a nucleus are attracted to each other by a. the nuclear force. b. opposite charges. c. their energy levels. d. electron repulsion.
a
The atomic mass of an element listed in the periodic table is the a. average atomic mass. b. relative atomic mass of the most abundant isotope. c. relative atomic mass of the most abundant radioactive isotope. d. mass number of the least abundant isotope.
a
The average atomic mass of an element is the average of the atomic masses of its a. naturally occurring isotopes. b. two most abundant isotopes. c. radioactive isotopes. d. artificial isotopes.
a
The force of attraction by Group 1 metals for their valence electrons is a. weak. b. zero. c. strong. d. greater than that for inner shell electrons.
a
The most common form of hydrogen has a. no neutrons. b. one neutron. c. two neutrons. d. three neutrons.
a
The number of valence electrons in Group 1 elements is a. 1. b. 2. c. 8. d. equal to the period number.
a
The number of valence electrons in Group 17 elements is a. 7. b. 8. c. 17. d. equal to the period number.
a
The periodic table a. permits the properties of an element to be predicted before the element is discovered. b. will be completed with element 118. c. has been of little use to chemists since the early 1900s. d. was completed with the discovery of the noble gases.
a
The relative atomic mass of an atom can be found by comparing the mass of the atom to the mass of a. one atom of carbon-12. b. one atom of hydrogen-1. c. a proton. d. uranium-235.
a
What are the elements with atomic numbers from 58 to 71 called? a. the lanthanides b. the noble gases c. the actinides d. the alkali metals
a
Which groups in the main group have lower electronegativity than d-block elements? a. groups 1 and 2 b. groups 13 through 18 c. groups 17 and 18 d. groups 13 through 17
a
Which of the following is an example of a homogeneous mixture? a. air b. orange juice c. raw milk d. marble
a
Whose series of experiments identified the nucleus of the atom? a. Rutherford b. Dalton c. Chadwick d. Bohr
a
Within a group of elements, as the atomic number increases, the atomic radius a. increases. b. remains approximately constant. c. decreases regularly. d. varies unpredictably.
a
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. a. equal to b. greater than c. less than d. either greater than or less than
a.
A compound is a. a pure substance that cannot be broken down into simpler, stable substances. b. a substance, made of two or more atoms that are chemically bonded, that can be broken down into simpler, stable substances. c. the smallest unit of matter that maintains its chemical identity. d. any substance, whether it is chemically bonded or not.
b
A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called a(n) a. nuclide. b. neutron. c. electron. d. isotope.
b
A theory is best described as a a. series of experimental observations. b. generalization that explains a body of known facts or phenomena. c. scientifically proven fact. d. testable statement.
b
After measuring the ratio of the charge of a cathode-ray particle to its mass, Thomson concluded that the particles a. had no mass. b. had a very small mass. c. had a very large mass. d. carried a positive charge.
b
All known chemical elements are organized into groups based on similar chemical properties in the a. chemical chart. b. periodic chart. c. element table. d. None of the above
b
Among the d-block elements, as atomic radii decrease, electronegativity values a. remain constant. b. increase. c. decrease. d. drop to zero.
b
As the atomic number increases, the number of electrons in a neutral atom a. decreases. b. increases. c. remains the same. d. is undetermined.
b
As you move left to right in Period 4 from gallium through bromine, atomic radii a. generally increase. b. generally decrease. c. do not change. d. vary unpredictably.
b
Atoms of the same element can differ in a. chemical properties. b. mass number. c. atomic number. d. number of protons and electrons.
b
Evidence gathered since Mendeleev's time indicates that a better arrangement than atomic mass for elements in the periodic table is an arrangement by a. mass number. b. atomic number. c. group number. d. series number.
b
If 63.5 g of copper (Cu) combine with 16 g of oxygen (O) to form the compound CuO, how many grams of oxygen will be needed to combine with the same amount of copper to form the compound CuO2? a. 16 g b. 32 g c. 64 g d. 127 g
b
If a mixture is not uniform throughout, it is called a. homogeneous. b. heterogeneous. c. chemically bonded d. a solution
b
If each atom of element D has 3 mass units and each atom of element E has 5 mass units, a molecule composed of one atom each of D and E has a. 2 mass units. b. 8 mass units. c. 15 mass units. d. 35 mass units.
b
In Rutherford's experiments, most of the particles a. bounced back. b. passed through the foil. c. were absorbed by the foil. d. combined with the foil.
b
In groups 13 through 18, valence electrons may be in sublevels a. s and d. b. s and p. c. d and f. d. p and d.
b
Isotopes are atoms of the same element that have different a. principal chemical properties. b. masses. c. numbers of protons. d. numbers of electrons.
b
Matter includes all of the following except a. air. b. light. c. smoke d. water vapor
b
Nuclear forces exists because the particles in the nucleus are a. oppositely charged. b. close together. c. highly energized. d. moving very fast.
b
Plasma is the fourth state of matter. In the plasma state a. atoms gain electrons. b. atoms lose electrons. c. atoms form molecules. d. atomic nuclei break down.
b
The average atomic mass of an element a. is the mass of the most abundant isotope. b. may not equal the mass of any of its isotopes. c. cannot be calculated. d. always adds up to 100.
b
The deflection of cathode rays in Thomson's experiments was evidence of the ____ nature of electrons. a. wave b. charged c. particle d. spinning
b
The electrons available to be lost, gained, or shared when atoms form compounds are called a. ions. b. valence electrons. c. d electrons. d. electron clouds.
b
The nucleus of deuterium contains one proton and a. two neutrons. b. one neutron. c. no neutrons. d. two electrons.
b
The number of atoms in a mole of any pure substance is called a. its atomic number. b. Avogadro's constant. c. its mass number. d. its gram-atomic number.
b
The periodic law states that a. no two electrons with the same spin can be found in the same place in an atom. b. the physical and chemical properties of the elements are functions of their atomic numbers. c. electrons exhibit properties of both particles and waves. d. the chemical properties of elements can be grouped according to periodicity but physical properties cannot.
b
The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic a. masses. b. numbers. c. radii. d. charges.
b
The principle that states that the physical and chemical properties of the elements are periodic functions of their atomic numbers is a. the periodic table. b. the periodic law. c. the law of properties. d. Mendeleev's law.
b
The two most important properties of all matter are a. the ability to carry an electric current well and to hold electric charge. b. taking up space and having mass. c. being brittle and hard. d. being malleable and ductile.
b
Under ordinary conditions of temperature and pressure, the particles in a gas are a. closely packed. b. very far from one another. c. held in fixed positions. d. unevenly distributed.
b
When an electrical current passed through a glass tube, it caused the surface of the tube directly across from the cathode to glow. Scientists concluded that a. a magnetic field was produced. b. the particles of the beam were negatively charged. c. there was gas in the tube. d. atoms were indivisible.
b
When determining the size of an atom by measuring the distance between bonded, identical, adjacent nuclei, the radius of an atom is a. equal to the distance between nuclei. b. one-half the distance between nuclei. c. twice the distance between nuclei. d. one-fourth the distance between nuclei.
b
Which part of an atom has a mass approximately equal to 1/2000 of the mass of a common hydrogen atom? a. nucleus b. electron c. proton d. neutron
b
A homogeneous mixture is also called a. chemically bonded. b. a compound. c. a solution d. a solute
c
A mixture is a. a combination of pure substances bonded chemically. b. any substance with a uniform composition. c. a blend of any two or more kinds of matter, as long as each maintains its own unique properties. d. any group of elements that are chemically bonded to one another.
c
A solid substance is a. always frozen regardless of its container. b. always a crystal regardless of its container. c. always the same shape regardless of its container. d. always losing particles regardless of its container.
c
A student recorded the following while completing an experiment. Color of substance: yellow, shiny powder Effect of magnet: yellow, shiny powder was attracted The student should classify the substance as a(n) a. element. b. compound. c. mixture. d. plasma.
c
All of the following are steps in the scientific method except a. observing and recording data. b. forming a hypothesis. c. discarding data inconsistent with the hypothesis. d. developing a model based on experimental results.
c
An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is a. 13. b. 14. c. 27. d. 40.
c
An atom is electrically neutral because a. neutrons balance the protons and electrons. b. nuclear forces stabilize the charges. c. the numbers of protons and electrons are equal. d. the numbers of protons and neutrons are equal.
c
Barium, atomic number 56, is the fifth element in Group 2. What is the atomic number of radium, the next element in Group 2? a. 64 b. 74 c. 88 d. 103
c
If 6.0 g of element K combine with 17 g of element L, how many grams of element K combine with 85 g of element L? a. 17 g b. 23 g c. 30. g d. 91 g
c
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 a. conservation of mass. b. mass action. c. multiple proportions. d. definite composition.
c
Molar mass a. is the mass in grams of one mole of a substance. b. is numerically equal to the average atomic mass of the element. c. Both (a) and (b) d. Neither (a) nor (b)
c
Most of the volume of an atom is occupied by the a. nucleus. b. nuclides. c. electrons. d. protons.
c
The first member of the noble gas family, whose highest energy level consists of an octet of electrons, is a. helium. b. argon. c. neon. d. krypton.
c
The most reactive group of the nonmetals is the a. lanthanides. b. transition elements. c. halogens. d. noble gases.
c
The total number of protons and neutrons in the nucleus of an atom is its a. atomic number. b. Avogadro number. c. mass number. d. average atomic mass.
c
Valence electrons are those s and p electrons a. closest to the nucleus. b. in the lowest energy level. c. in the highest energy level. d. combined with protons.
c
What happens to the energy in a substance when it changes state? a. It is destroyed. b. It is changed into matter. c. It changes form, but is neither destroyed nor increased. d. The energy remains unchanged.
c
When an electron is added to a neutral atom, a certain amount of energy is a. always absorbed. b. always released. c. either released or absorbed. d. transferred to the more electronegative element.
c
Which of the following is an example of a heterogeneous mixture? a. a gold ring b. seawater c. granite d. sucrose
c
Which of the following is an extensive property of matter? a. melting point b. boiling point c. volume d. density
c
Which of the following is not a chemical change? a. rusting b. igniting c. melting d. burning
c
A measure of the quantity of matter is a. density. b. weight. c. volume. d. mass.
d
A physical change occurs when a a. peach spoils. b. silver bowl tarnishes. c. bracelet turns your wrist green. d. glue gun melts a glue stick.
d
A statement that can be tested experimentally is a a. variable. b. model. c. generalization. d. hypothesis.
d
A true statement about mass is that a. mass if often measured with a spring scale. b. mass is expressed in pounds. c. as the force of Earth's gravity on an object increases, the object's mass increases. d. mass is determined by comparing the mass of an object with a set of standard masses that are part of a balance.
d
Elements in a group or column in the periodic table can be expected to have similar a. atomic masses. b. atomic numbers. c. numbers of neutrons. d. properties.
d
Experiments with cathode rays led to the discovery of the a. proton. b. nucleus. c. neutron. d. electron.
d
For groups 13 through 18, the number of valence electrons is equal to the group number a. plus 1. b. plus the period number. c. minus the period number. d. minus 10.
d
In Rutherford's experiments, alpha particles a. passed through a tube containing gas. b. were used to bombard a cathode plate. c. collided with electrons. d. were used to bombard thin metal foil.
d
In early experiments on electricity and matter, an electrical current was passed through a glass tube containing a. water b. gas under high pressure. c. liquid oxygen. d. gas under low pressure.
d
In the alkaline-earth group, atoms with the smallest radii a. are the most reactive. b. have the largest volume. c. are all gases. d. have the highest ionization energies.
d
It is easy to determine whether a substance is a metal if the substance is a. easy to break down into its components. b. very hard. c. very brittle. d. a good electrical and heat conductor.
d
Nitrogen monoxide and oxygen, both colorless gases, form a red-brown gas when mixed. Nitrogen monoxide and oxygen are called the a. products. b. equilibria. c. synthetics. d. reactants.
d
The elements whose electron configurations end with s2 p5 in the highest occupied energy level belong to Group a. 3. b. 7. c. 10. d. 17.
d
The energy required to remove an electron from an atom is the atom's a. electron affinity. b. electron energy. c. electronegativity. d. ionization energy.
d
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 a. sodium has four or five electrons. b. the atomic radius has increased. c. a d electron has been removed. d. the noble gas configuration has been reached.
d
The liquid state of matter can be described as a. having definite shape and definite volume. b. having neither a definite shape nor a definite volume. c. having lost electrons owing to energy content. d. having a definite volume but not a definite shape.
d
The mass of a sample containing 3.5 mol of silicon atoms (atomic mass 28.0855 amu) is approximately a. 28 g. b. 35 g. c. 72 g. d. 98 g.
d
The most characteristic property of the noble gases is that they a. have low boiling points. b. are radioactive. c. are gases at ordinary temperatures. d. are largely unreactive.
d
The nucleus of an atom has all of the following characteristics except that it a. is positively charged. b. is very dense. c. contains nearly all of the atom's mass. d. contains nearly all of the atom's volume.
d
The smallest unit of an element that can exist either same or different elements is the a. electron. b. proton. c. neutron. d. atom.
d
Which of the following is not a physical change? a. grinding b. cutting c. boiling d. burning
d
Within the p-block elements, the elements at the top of the table, compared with those at the bottom, a. have larger radii. . b. are more metallic. c. have lower ionization energies d. are less metallic.
d
