CHEMISTRY REGENTS REVIEW ALL TOPICS Flashcards
which statement describes the earliest model of the atom
1) an atom is an invisible hard sphere
2) an atom has a small dense nucleus
3) electrons are negative particles in an atom
4) electrons in an atom have wavelike properties
1
in all atoms of bismuth the number of electrons must equal the
number of protons
number of neutrons
sum of the number of neutrons and protons
difference between the number of neutrons and protons
1
an orbital is a region in an atom where there is a high probabitlity of finding
an alpha particle
an electron
a neutron
a positron
2
which electron shell in an atom of calcium in the ground state has an electron with the greatest amount of energy
1
2
3
4
4
as the elements in period 2 are considered in order from lithium to flourine, there is an increase in the
atomic radius
electronegativity
number of electron shells
number of electrons in the fist shell
2
which element is classified as a metalloid
boron
potassium
sulfur
xenon
boron
strontium and barium have similar chemical properties because atoms of these elements have the same number of
protons
neutrons
electron shells
valance electrons
valance electrons
which term represents the fixed proportion of elements in a compound
atomic mass
molar mass
chemical formula
density formula
chemical formula
which two terms represent types of chemical formulas
mechanical and structural
mechanical and thermal
molecular and structural
molecular and thermal
3
which element has metallic bonds at room temp
bromine
cesium
krypton
sulfur
cesium
what is the number of electrons shared between the atoms in a molecule of nitrogen, N2
8
2
3
6
6
given the equation representing a reaction
H + H yeilds H2
what occurs during this reaction?
a bond is broken and energy is absorbed
a bond is broken and energy is released
a bond is formed and energy is absorbed
a bond is formed and energy is released
4
an atom of which element has the strongest attraction for electrons in a chemical bond
chlorine
carbon
phosphorus
sulfur
chlorine
at STP, a 50 gram sample of H2O (l) and a 100 gram sample of H2O (l) have
the same chemical properties
the same volume
diff temperatures
diff empirical formulas
1
what statement describes a mixture of sand and water at room temperature
it is heterogeneous and its components are in the same phase
it is heterogeneous and its componets are in different phases
it is homogenous and its componets are in the same phase
it is homogenous and its components are in different phases
2
distillation is a process used to separate a mixture of liquids based on different
boiling points
densities
freezing points
solubilities
boiling points
according to the kinetic molecular theory, which statement describes the particles in a sample of an ideal gas
the particles are constantly moving in circular patterns
the particles collide decreasing the total energy in the system
the particles have attractive forces between them
the particles are considered to have negligible volume
4
for a chemical system at equilibrium the concentrations of both the reactants and the products must
decrease
increase
be constant
be equal
constant
in terms of disorder and energy, systems in nature have a tendency to undergo changes toward
less disorder and lower energy
less disorder and higher energy
greater disorder and lower energy
greater disorder and higher energy
3
the only two elements in alkenes and alkynes are
carbon and nitrogen
carbon and hydrogen
oxygen and nitrogen
oxygen and hydrogen
2
which functional group contains a nitrogen atom and an oxygen atom
ester
ether
amide
amine
amide
when a sample of Mg (s) reacts completely with O2(g), the Mg(s) loses 5 moles of electrons. How many moles of electrons are gained by the O2(g)
1 mol
2.5 mol
5 mol
10 mol
5 mol
which statement describes the reactions in an electrochemical cell
oxidation occurs at the anode and reduction occurs at the cathode
oxidation occurs at the cathode and reduction occurs at the anode
oxidation and reduction both occur at the cathode
oxidation and reduction both occur at the anode
1
what is the color of bromcresol green indicator in a solution with a pH value of 2
blue
green
red
yellow
4
in which reaction is an atom of one element converted into an atom of another element
combustion
fermentation
oxidation-reduction
transmutation
4
in which type of nuclear reaction do nuclei combine to form a nucleus with a greater mass
alpha decay
beta decay
fusion
fission
fusion
which electron configuration represents the electrons in an atom of sulfur in an excited state
2-8-6
2-7-7
2-8-7
2-7-8
2
which notations represent atoms that have the same number of protons but a different number of neutrons
H-3 and He-3
S-32 and S-32
Cl-35 and Cl-37
Ga-70 and Ge-73
3
what is the molarity of 2 liters of an aqueous solution that contains .5 mole of potassium iodide, KI
1 M
2 M
.25 M
.5 M
.25 M
hydrochloric acid reacts faster with powdered zinc than with an equal mass of zinc strips because the greater surfact are of the powdered zinc
decrease the frequency of particle collisions
decreases the activation energy of the reaction
increases the frequency of particle collisions
increases the activation energy of the reaction
3
which radioisotope requires long term storage as the method of disposal to protect living things from radiation exposure over time
Pu-239
Fr-220
Fe-53
P-32
1
state the number of protons in an atom of N-15
7
state the number of electrons in each shell of an N-14 atom in the ground state
2-5
based on the atomic mass of the element nitrogen on the periodic table compare the relative abundances of the naturally occuring isotopes of nitrogen
the relative abundances of the naturally occuring isotopes of N-14 is more abundant than N-15
which statement describes a concept included in the wave mechanical model of the atom
protons neutrons and electrons are located in the nucleus
electrons orbit the nucleus in shells at fixed distances
atoms are hard invisible spheres
electrons are located in regions called orbitals
4
as an electron in an atom moves from a higher energy state to a lower energy state, the atom
becomes a negative ion
becomes a poisive ion
releases energy
absorbes energy
3
two atoms that are different isotopes of the same element have
the same number of protons and the same number of neutrons
the same number of protons but a different number of neutrons
a different number of protons but the same number of neutrons
a different number of protons and a different number of neutrons
2
the element in group 14 period 3 of the periodic table is classified as a
metal
noble gas
metalloid
nonmetal
3
which conclusion was developed as a result of the gold foil experiment
atoms are mostly empty space
all atoms are hard invisible spheres
atoms have different volumes
all atoms have the same volume
1
which two particles each have a mass approximately equal to one atomic mass unit
positron and proton
positron and electron
neutron and electron
neutron and proton
4
an excited potassium atom emits a specific amount of energy when one of its electrona moves from
the first shell to the fourth shell
the second shell to the fourth shell
the fourth shell to the fifth shell
the fourth shell to the second shell
4
which list of elements includes a metal, a metalloid, and a noble gas?
Rd, Cl, Ne
Rn, Cl, Ne
Sr, Si, Rn
Si, Rb, Sr3
3
which element has the lowest density at 298K and 101.3kPa
argon
fluorine
nitrogen
oxygen
3
which statement describes the changes in bonding and energy that occur when a molecule of iodine forma two separate atoms of iodine
a bond is formed as energy is absorbed
a bond is formed as energy is released
a bond is broken as energy is absorbed
a bond is broken as energy is released
3
the degree of polarity in the bond between a hydrogen atom and an oxygen atom in a molecule of water can be assessed using the difference in
densities
electronegativities
melting points
intermolecular forces
2
which substance can not be broken down by a chemical change
ammonia
krypton
ethanol
water
2
which term is used to express the concentration of an aqueous solution
parts per million
heat of fustion
pressure at 0 degrees C
volume at 0 degrees C
1
which process represents a chemical change
iodine sublimes
water evaporates
an ice cube melts
a candle burns in air
4
systems in nature tend to undergo changes toward
higher energy and higher entropy
higher energy and lower entropy
lower energy and higher entropy
lower energy and lower entropy
3
which statement describes the bonding in an alkyne molecule
there is at least one carbon to carbon double bond
there is at least one carbon to carbon triple bond
there is at least one carbon to oxygen single bond
there is at least one carbon to oxygen double bond
2
which term identifies a type of organic reaction
deposition
distillation
polymerization
vaporization
3
in an electrochemical cell, oxidation occurs at the
anode
cathode
salt bridge
switch
anode
which energy conversion occurs in an operating electrolytic cell
chemical energy to electrical energy
electrical energy to chemical energy
nuclear energy to electrical energy
electrical energy to nuclear energy
2
one acid base theory states that a base is an
H- donor
H- acceptor
H+ donor
H+ acceptor
4
the acidity or alkalinity of a solution can be measured by its
pH value
electronegativity value
boiling point
freexing point
1
which nuclear emission has the greatest mass
positron
gamma ray
beta particle
alpha particle
4
which statement describes the net change that occurs during nuclear fission
electrons are converted to protons
protons are converted to electrons
mass is converted to energy
energy is converted to mass
3
which general trend is observed as the elements in period 2 are considered from left to right
atomic mass decreases
melting point increases
electronegativity increases
first ionization energy decreases
3
one mole of bromine gas, Br2, has a mass of
35 g
70 g
79.9 g
159.8 g
4
which sattement describes the charge and the radius of the magnesium ion formed when a magnesium atom loses two electrons
the Mg ion is postive and has a radius larger than the Mg atom
the Mg ion is negative and has a radius larger than the Mg atom
the Mg ion is positive and has a radius smaller than the Mg atom
the Mg ion is negative and has a radius smaller than the Mg atom
3
the concept that matter is composed of tiny, discrete particles is generally attributed to the
greeks
romans
english
germans
greeks
the first subatomic particle discovered was the
proton
neutron
electron
photon
electron
According to the law of the conservation of mass, if the products of a reaction have a mass of 64 g, then the total mass of the reactants
must be less than 64g
must be equal to 64g
must be more than 64g
is not related to the mass of the products
2
the gold foil experiment led scientists to conclude that an atoms
positive charge is evenly distributed throughout its volume
negative charge is mainly concentrated in its nucleus
mass is evenly distributed throughout its volume
volume is mainly unoccupied
4
the model of the atom that pictured the atom with electrons stuch randomly throughout the mass of the atom was called the
cannonball model
plum pudding model
planetary model
wave mechanical model
2
after bombarding a gold foil sheet with alpha particles scientists concluded that atoms mainly consist of
electrons
empty space
protons
neutrons
empty space
experimental evidence indicates that the nucleus of an atom
contains most of the mass of the atom
contains a small percentage of the mass of the atom
has no charge
has a negative charge
1
daltons atomic theory states that
all atoms of an element are positively charged
different elements can have the same mass
atoms of a given element must be identical
all the atoms in a compound are identical
3
modern theory pictures an electron as
a particle
a wave only
both a particle and a wave
neither a particle nor a wave
3
why did rutherford conclude that the atom was mostly empty space
most alpha particles went through it
the atomic mass of an element is defined as the weighted average mass of that elements
most abundant isotope
least abundant isotope
naturally occuring isotopes
radioactive isotopes
3
element x has two isotopes. if 72% of the element has an isotopic mass of 84.9 amu and 28% has an isotopic mass of 87 amu, the average atomic mass of element X is numerically equal to
(72 + 98.9)(28 + 87)
(72 - 84.9)(28 - 87)
(.720)(84.9) + (.280)(87)
(72)(84.9) + (28)(87)
3
a neutral atom with 6 electrons and 8 neutrons is an isotope of
carbon
silicon
nitrogen
oxygen
1
the major portion of an atoms mass consists of what
neutrons and protons
a neutron has approximately the same mass as
an alpha particle
a beta particle
an electron
a proton
4
what is the nuclear cahrge of an atom with a mass of 23 and an atomic number of 11
11
12
23
34
11
compared to the charge and mass of a proton, an electron has
the same charge and a smaller mass
the same charge and the same mass
an opposite charge and a smaller mass
an opposite charge and the same mass
3
which of the following statements are correct
a proton is positively charged and a neutron is negatively charged
a proton is negatively charged and a neutron is positively charged
a proton is positively charged and an electron is negatively charged
a proton is negatively charged and an electron is positively charged
3
when electrons in an excited state fall to lower energy levels, energy is
absorbed
released
neither absorbed nor released
both absorbed and released
2
the characteristic bright line spectrum of an atom is produced when
nuclei undergo fission
nuclei undergo fusion
electrons move from higher to lower levels
electrons move from lower to higher energy levels
3
when the electrons of an excited atom fall back to lower energy levels, the emission of energy produces
beta particles
alpha particles
spectral lines
gamma radiation
3
which atom in the ground state contains one completely filled p orbital
Ne
O
He
Be
1
hat is the total number of electrons in the second principal energy level of a calcium atom in the ground state
6
2
8
18
8
the atom of which element in the ground state has two unpaired electrons in the 2p sublevel
Fl
N
Be
C
C
what is the toal number of occupied s orbitals in an atom of nickel in ground state
1
2
3
4
4
which atom in hte ground state has only three electrons in the 3p sublevel
phosphorus
potassium
argon
aluminum
1
what is the total number of occupied principal energy levels in a neutral atom of neon in the ground state
1
2
3
4
2
in an atom of lithium in the ground state, what is the total number of orbitals that contain only one electron
1
2
3
4
1
which of the following cannot be decomposed by chemical means
sodium
ethanol
sucrose
water
sodium
a compound differs from an element in that a compound is
homogenous
has difinite composition
has a definite melting point
can be decomposed by a chemical reaction
4
a compound differs from a mixture in that a compound always has a
homogenous composition
maximum of two elements
minimum of three elements
heterogenous composition
1
a pure substance that is composed only of identical atoms is classified as
a compound
en elements
a heterogeneous mixture
a homogenous mixture
2
most elements are
metals
nonmetals
gases
made in a laboratory
1
which is a characteristic of all mixtures
they are homogenous
they are heterogeneous
their compositions are in a definite ratio
their compositions may vary
4
a heterogeneous material may be
an element
a compound
a pure substance
a mixture
4
which of these materials is a mixture
water
air
methane
magnesium
2
each particle contained in hydrogen gas is made up of two identical hydrogen atoms chemically joined together. Hydrogen gas is
a compound
an element
a homogenous mixture
a heterogeneous mixture
an elements
which of the following materials is a pure substance
air
water
fire
earth
2
which statement is an identifying characteristic of a mixture
a mixture can consist of a single element
a mixture can be separated by physical means
a mixture must have a definite composition by weight
a mixture must be homogenous
2
which substance can be decomposed by a chemical change
ammonia
aluminum
magnesium
manganese
ammonia
a model of the atom that pictured the atom with electrons traveling in circular orbit was called the
planetary model
cannonball model
wave mechanical model
plum pudding model
1
compared to the entire atom, the nucleus of the atom is
smaller and contains most of the atoms mass
smaller and contains little of the atoms mass
large and contains most of the atoms mass
large and contains little of the atoms mass
1
neutral atoms must contain equal number of
protons and electrons
protons and neutrons
protons, neutrons, and electrons
neutrons and electrons
1
compared with an electron a proton has
more mass and the same charge
more mass and an opposite charge
equal mass and the same charge
equal mass and an opposite charge
2
the total number of electrons in a neutral atom of any element is always equal to the atoms
mass number
number of neutrons
number of protons
number of nucleons
3
all isotopes of neutral atoms of sodium have
11 protons and 12 neutrons
12 protons and 11 neutrons
11 protons and 11 electrons
12 protons and 12 electrons
3
an atom in the excited state contains
more electrons than an atom in the ground state
more protons than an atom in the ground state
more potential energy than an atom in the ground state
more mass than an atom in the ground state
3
which of the following particles has the smallest mass
neutron
electron
proton
hydrogen atom
2
a chemical formula is an expression used to represent
mixtures only
elements only
compounds only
elements and compounds
4
which formula represents a compound
Ca
Cr
CO
Co
3
What is the total number of atoms in the formula Ca(NO3)2
7
2
3
9
9
pure nitrogen combines directly with an active metal to form a
nitrate
nitride
nitrite
permanganate
2
Ag + Hsub2S yeilds Agsub2S +H sub
what is the sum of the coefficients when teh equation is completely balanced using the smallest whole number coefficients
5
8
10
4
5
pure oxygen reacts with metals to form
oxalates
oxalites
oxides
oxygenates
3
which of the following is the formula of a compound
Fr
Mn
LiH
O3
3
a chemical formula represents
qualitative info only
quantitative info only
both quantitative and qualitative info
neither info
3
