Accounting
Anthropology
Archaeology
Art History
Banking
Biology & Life Science
Business
Business Communication
Business Development
Business Ethics
Business Law
Chemistry
Communication
Computer Science
Counseling
Criminal Law
Curriculum & Instruction
Design
Earth Science
Economic
Education
Engineering
Finance
History & Theory
Humanities
Human Resource
International Business
Investments & Securities
Journalism
Law
Management
Marketing
Medicine
Medicine & Health Science
Nursing
Philosophy
Physic
Psychology
Real Estate
Science
Social Science
Sociology
Special Education
Speech
Visual Arts
Chemistry
Q:
How many protons (p) and neutrons (n) are in an atom of calcium-46?
A) 20 p, 26 n
B) 20 p, 46 n
C) 26 p, 20 n
D) 46 p, 60 n
Q:
How many protons (p) and neutrons (n) are in an atom of ?
A) 38 p, 52 n
B) 38 p, 90 n
C) 52 p, 38 n
D) 90 p, 38 n
Q:
Boron-9 can be represented as
A) .
B) .
C) .
D) .
Q:
The isotope represented by is named
A) carbon-6
B) carbon-7
C) carbon-13
D) carbon-19
Q:
Which of the following represent isotopes?
A: [ ] B: [ ] C: [ ] D: [ ]
A) A and B
B) A and C
C) A and D
D) C and D
Q:
Which are isotopes? An atom that has an atomic number of 34 and a mass number of 76 is an isotope of an atom that has
A) an atomic number of 32 and a mass number of 76.
B) an atomic number of 34 and a mass number of 80.
C) 42 neutrons and 34 protons.
D) 42 protons and 34 neutrons.
Q:
Which of the following two atoms are isotopes?
A) and B) and C) and D) and
Q:
The mass number of an atom is equal to the number of
A) electrons.
B) neutrons.
C) protons.
D) protons plus neutrons.
Q:
The symbol that is usually used to represent atomic number is ________.
A) A
B) N
C) X
D) Z
Q:
A proton is approximately
A) 200 times larger than an electron.
B) 2000 times larger than an electron.
C) 200 times smaller than an electron.
D) 2000 times smaller than an electron.
Q:
Which subatomic particle has the smallest mass?
A) a proton
B) a neutron
C) an electron
D) an alpha particle
Q:
Most of the alpha particles directed at a thin gold foil in Rutherford's experiment
A) bounced directly back from the foil.
B) passed directly through the foil undeflected.
C) passed through the foil but were deflected at an angle.
D) were absorbed by the foil.
Q:
The existence of neutrons in the nucleus of an atom was demonstrated by
A) Millikan's oil drop experiment.
B) Rutherford's gold foil experiment.
C) Thomson's cathode ray tube experiment.
D) None of these
Q:
The current model of the atom in which essentially all of an atom's mass is contained in a very small nucleus, whereas most of an atom's volume is due to the space in which the atom's electrons move was established by
A) Millikan's oil drop experiment.
B) Rutherford's gold foil experiment.
C) Thomson's cathode ray tube experiment.
D) None of these
Q:
The charge-to-mass ratio of an electron was established by
A) Millikan's oil drop experiment.
B) Rutherford's gold foil experiment.
C) Thomson's cathode ray tube experiment.
D) None of these
Q:
The existence of electrons in atoms of all elements was demonstrated by
A) Millikan's oil drop experiment.
B) Rutherford's gold foil experiment.
C) Thomson's cathode ray tube experiment.
D) None of these
Q:
Elements A and Q form two compounds. The ratio (mass Q)/(mass A) for compound one is 0.271 and ratio (mass Q)/(mass A) for compound two is 0.362. If compound one has the chemical formula AQ, what is the chemical formula for compound two?
A) A3Q4
B) A2Q3
C) AQ2
D) AQ3
Q:
Elements A and Q form two compounds, AQ and A2Q. Which of the following must be true?
A) (mass Q)/(mass A) is one for AQ, and 1/2 for A2Q.
B) (mass Q)/(mass A) for AQ must equal (mass Q)/(mass A) for A2Q.
C) (mass Q)/(mass A) for AQ must be 2 times (mass Q)/(mass A) for A2Q.
D) (mass Q)/(mass A) for AQ must be 1/2 (mass Q)/(mass A) for A2Q.
Q:
Elements A and Q form two compounds, AQ and A2Q3. The mass ratio (mass Q)/(mass A) for AQ is 0.574. What is the mass ratio (mass Q)/(mass A) for A2Q3?
A) 0.383
B) 0.861
C) 1.16
D) 2.61
Q:
Which of the following is not explained by Dalton's atomic theory?
A) conservation of mass during a chemical reaction
B) the existence of more than one isotope of an element
C) the law of definite proportions
D) the law of multiple proportions
Q:
Which of the following is a part of Dalton's atomic theory?
A) Atoms are rearranged but not changed during a chemical reaction.
B) Atoms break down during radioactive decay.
C) Atoms contain protons, neutrons, and electrons.
D) Isotopes of the same element have different masses.
Q:
Which of the following statements is not a postulate of Dalton's atomic theory?
A) Each element is characterized by the mass of its atoms.
B) Atoms are composed of protons, neutrons, and electrons.
C) Chemical reactions only rearrange atomic combinations.
D) Elements are composed of atoms.
Q:
The observation that hydrogen and oxygen can react to form two compounds with different chemical and physical properties, one having an O:H mass ratio = 8:1 and the other having an O:H mass ratio = 16:1 is consistent with the law of
A) definite proportions.
B) energy conservation.
C) mass conservation.
D) multiple proportions.
Q:
A sample of pure calcium fluoride with a mass of 15.0 g contains 7.70 g of calcium. How much calcium is contained in 45.0 g of calcium fluoride?
A) 2.56 g
B) 7.70 g
C) 15.0 g
D) 23.1 g
Q:
A sample of pure lithium carbonate contains 18.8% lithium by mass. What is the % lithium by mass in a sample of pure lithium carbonate that has twice the mass of the first sample?
A) 9.40%
B) 18.8%
C) 37.6%
D) 75.2%
Q:
The formula of iron(III) oxide contains ________ iron(III) and ________ oxide ions.
Q:
Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was consumed in the reaction?
A) 4.68 g
B) 5.98 g
C) 10.14 g
D) 10.66 g
Q:
Phosphate ion has the formula ________.
Q:
Methane and oxygen react to form carbon dioxide and water. What mass of water is formed if 3.2 g of methane reacts with 12.8 g of oxygen to produce 8.8 g of carbon dioxide?
A) 7.2 g
B) 8.8 g
C) 14.8 g
D) 16.0 g
Q:
The bonding in MgO is ________, whereas the bonding in CO is ________.
Q:
The observation that 4.0 g of hydrogen reacts with 32.0 g of oxygen to form a product with
O:H mass ratio = 8:1, and 6.0 g of hydrogen reacts with 48.0 g of oxygen to form the same product
with O/H mass ratio = 8:1 is evidence for the law of
A) definite proportions.
B) energy conservation.
C) mass conservation.
D) multiple proportions.
Q:
The number of electrons in the ion C4- is ________.
Q:
The observation that 15.0 g of hydrogen reacts with 120.0 g of oxygen to form 135.0 g of water is evidence for the law of
A) definite proportions.
B) energy conservation.
C) mass conservation.
D) multiple proportions.
Q:
The number of electrons in the ion Ca2+ is ________.
Q:
According to history, the concept that all matter is composed of atoms was first proposed by
A) the Greek philosopher Democritus, but not widely accepted until modern times.
B) Dalton, but not widely accepted until the work of Mendeleev.
C) Dalton, but not widely accepted until the work of Einstein.
D) Dalton, and widely accepted within a few decades.
Q:
10% saline solution (sodium chloride dissolved in water) is an example of a ________ mixture.
Q:
Nuclei that are in the band of stability have a neutron/proton ratio ________ (equal to, greater than, less than) 1:1.
Q:
In an electron capture reaction a proton is converted into a ________.
Q:
undergoes alpha decay producing one alpha particle and a single nuclide. To balance the equation, ________ and ________ must be added to the right side of the equation below. -> ? + ?
Q:
In a nuclear reaction is the symbol for ________.
Q:
In a nuclear reaction, the symbol for a beta particle is ________.
Q:
The missing reactant in the nuclear reaction ? - + is ________.
Q:
The number of protons, neutrons, and total nucleons in are ________, ________, and ________, respectively.
Q:
The number of moles of Li in 34.7 g Li is ________.
Q:
To the nearest whole number, the number of grams of Ba in 3.25 mol of Ba is ________.
Q:
The number of atoms in 23 g of Na is ________ (greater than, less than, the same as) the number of atoms in 12 g of C.
Q:
Chlorine has two common isotopes, chlorine-35 and chlorine-37, and an atomic mass of 35.45 amu. The natural abundance of chlorine-35 is ________ (greater than, less than, the same as) the natural abundance of chlorine-37.
Q:
A neutral atom with atomic number 5 and mass number 11 contains ________ electrons.
Q:
The number of neutrons in a neutral atom of uranium-238 is ________.
Q:
The symbol for technetium-98 is ________.
Q:
The symbol of the isotope having Z = 88 and A = 226 is ________.
Q:
Isotopes have the same number of ________ but different numbers of ________ in their nuclei.
Q:
Atoms of the same element always have the same number of ________ in their nuclei.
Q:
The subatomic particles contained in the nucleus of an atom are ________ and ________.
Q:
The charge to mass ratio of an electron was determined from Rutherford's cathode-ray tube experiment to be 1.759 108 C/g and the charge on a single electron was determined from the Millikan oil drop experiment to be 1.602 10-19 C, so the mass of a single electron is ________.
Q:
According to the law of multiple proportions, if 12 g of carbon combine with 16 g of oxygen to form CO, the number of grams of carbon that combine with 16 g of oxygen in the formation of CO2 is ________.
Q:
In the reaction HBr + NaOH → H2O + NaBr, If 81 g HBr react with 40 g of NaOH to produce 18 g of H2O, the number of grams of NaBr produced is ________.
Q:
The chemical formula for nitrous acid is
A) H3N(aq).
B) H NO2(aq).
C) H NO3(aq).
D) H2N2O6(aq).
Q:
The ion, IO2-, is named
A) iodate ion.
B) iodite ion.
C) iodine dioxide ion.
D) iodine(II) oxide ion.
Q:
The compound, SO3, is named
A) sulfate.
B) sulfite.
C) sulfur trioxide.
D) sulfur ( VI) oxide.
Q:
The compound, Cu( IO3 )2, is named
A) copper iodate(II).
B) copper(I) iodate.
C) copper(I) iodate(II).
D) copper(II) iodate.
Q:
The chemical formula for lithium peroxide is
A) LiOH.
B) LiO2.
C) Li2O.
D) Li2O2.
Q:
An aqueous solution of H2S is named
A) hydrosulfuric acid.
B) hydrosulfurous acid.
C) sulfuric acid.
D) sulfurous acid.
Q:
What is the chemical formula for magnesium hydride?
A) MgH2
B) MgOH
C) MgOH2
D) Mg(OH)2
Q:
What is the chemical formula for calcium hydroxide?
A) CaH2
B) CaOH
C) CaOH2
D) Ca(OH)2
Q:
Rb2S is named
A) rubidium disulfide.
B) rubidium sulfide.
C) rubidium(II) sulfide.
D) rubidium sulfur.
Q:
What is the charge on the Cr ions in Cr2O3?
A) 2-
B) 1+
C) 2+
D) 3+
Q:
What is the chemical formula for iron( III) sulfate?
A) Fe3S
B) Fe3SO4
C) Fe2S3
D) Fe2( SO4)3
Q:
The solid compound, Mg(NO3)2, contains
A) Mg2+, N5+, and O2- ions.
B) Mg2+ ions and (NO32- ions.
C) Mg 2+ and (NO32- ions.
D) Mg(NO3)2 molecules.
Q:
Which of the compounds CH4, SrCl2, Cr(NO3)3, XeF2 are expected to exist as molecules?
A) only CH4
B) CH4 and Xe F2
C) CH4, Cr(NO3)2, and Xe F2
D) SrCl2 and Cr(NO3)2
Q:
Which of the compounds, Li3N, NH3, C3H8, IF3 are ionic compounds?
A) only C3H8
B) only Li3N
C) Li3N and NH3
D) NH3, C3H8, and I F3
Q:
Which of the following is the correct chemical formula for a molecule of astatine?
A) At
B) At-
C) At+
D) At2
Q:
Which one of the following compounds contains ionic bonds?
A) SrO
B) H Br
C) P Br3
D) SiO2
Q:
What type of bonding is found in the compound O F2?
A) covalent bonding
B) hydrogen bonding
C) ionic bonding
D) metallic bonding
Q:
How many electrons are in the ion, PO43-?
A) 26
B) 44
C) 47
D) 50
Q:
In which of the following sets do all species have the same number of protons?
A) F-, Ne, Mg2+
B) Ge, Se2-, Br-
C) K+, Rb+, Cs+
D) Br, Br-, Br+
Q:
In which of the following sets do all species have the same number of electrons?
A) F-, Ne, Mg2+
B) Ge, Se2-, Br-
C) K+, Rb+, Cs+
D) Br, Br-, Br+
Q:
How many electrons are in the ion, Cu2+?
A) 27
B) 29
C) 31
D) 64
Q:
In which set do all elements tend to form cations in binary ionic compounds?
A) K, Ga, O
B) Sr, Ni, Hg
C) N, P, Bi
D) O, Br, I
Q:
Ammonia is an example of
A) a compound.
B) an element.
C) a heterogeneous mixture.
D) a homogeneous mixture.