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WorksheetsChem 2-8 Wednesday
Total questions: 73
Worksheet time: 37mins
the number of protons in the nucleus of an element
atomic number
mass number
atomic mass
which state of matter has a definite volume ad takes the shape of its container
solid
liquid
gas
which state of matter takes both the shape and volume of its container
solid
liquid
gas
which state of matter is characterized by having a definite shape and a definite volume
solid
liquid
gas
which of the following is a physical change
corrosion
explosion
evaporation
rotting of food
which of the following is a heterogeneous mixture
air
salt water
steel
soil
which of the following is a homogeneous mixture
salt water
beef stew
sand and water
soil
what is one difference between a mixture and a compound
a compound consists of more than one phase
a compound can only be separated into its components by chemical means
a mixture can only be separated into its components by chemical means
a mixture must be uniform in composition
the first figure in a properly written chemical symbol always is
boldface
capitalzed
italicized
underlined
which of the following is not a physical change
grating cheese
melting cheese
fermenting of cheese
mixing two cheeses in a bowl
which of the following processes does not involve a change in chemical properties
rusting
fermenting
boiling
burning
what happens to matter during a chemical reaction
matter is neither created nor destroyed
some matter is destroyed
some matter is created
some matter is destroyed and some is created
which of the following is true for all chemical reactions
the total mass of the reactants increases
the total mass of the products is greater than the total mass of reactants
the total mass of the products is less than the total mass of the reactants
the total mass of the reactants equals the total mass of the products
who was the man who lived from 460B.C.-370B.C. and was among the first to suggest the idea of atoms
atomos
dalton
democritus
thomson
the particles that are not found in the nucleus of an atom are
protons and electrons
electrons only
neutrons and electrons
protons and neutrons
all atoms are
positively charged, with the number of protons exceeding the number of electrons
negatively charged, with the number of electrons exceeding the number of protons
neutral, with the number of protons equaling the number of electrons
neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons
the nucleus of an atom
the central core and is composed of protons and neutrons
positively charged and has more protons than neutrons
negatively charged and has a high density
negatively charged and has a low density
an element has an atomic number of 68. the number of protons and electrons in a neutral atom of the element are
136 protons and 68 electrons
68 protons and 68 electron
68 protons and 0 electrons
35 protons and 34 electrons
all atoms of the same element have the same
number of neutrons
number of protons
mass number
mass
How is the number of neutrons in the nucleus of an atom calculated
add the number of electrons and protons together
subtract the number of electrons from the number of protons
subtract the number of protons from the mass number
add the mass number to the number of electrons
In which of the following is the number of neutrons correctly represented
19/9F has 0 neutrons
75/33As has 108 neutrons
24/12Mg has 24 neutrons
238/92 U has 146 neutrons
The atomic mass of an element depends upon
mass of each electron in the element
mass of each isotope of that element
relative abundance of protons in that element
mass and relative abundance of each isotope of that element
In the Bohr model of an atom, an electron in an orbit has a foxed
position
color
energy
size
The principal quantum number indicates what property of an electron
position
speed
energy level
electron cloud shape
How many energy sublevels are in the third principal energy level
1
2
3
4
what is the maximum number of s orbitals in any single energy level in an atom
1
3
5
7
what is the maximum number of d orbitals in a principal energy level
1
2
3
5
what is the maximum number of orbitals in the p sublevel
2
3
4
5
The energy required to remove an electron from an atom
Quantum
Ionization energy
cation
what is the maximum number of electron in the second principal energy level
2
8
18
32
When an electron moves from a lower to a higher energy level, the elcetron
always doubles its energy
absorbs a continuously variable amount of energy
absorbs a quantum of energy
moves closer to the nucleus
the letter "p" in the symbol 4p3 indicates the
spin of an electron
orbital shape
principle energy level
speed of an electron
if the spin of one electron in an orbital is clockwise, what is the spin of the other electron in the orbital?
zero
clockwise
counterclockwise
both counter and clockwise
if three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals
one electrons in each
two electrons in one orbital and one in another and none is the third
three in one orbital and none in the other two
three electrons cannot fill three empty 2p orbitals
what are quanta of light called
charms
protons
orbitals
photon
which scientist developed the quantum mechanical model of the atom
albert einstein
erwin schrodinger
niels bohr
ernest rutherford
who predicted that all matter can behave as waves as well as particles
albert einstein
erwin schrodinger
max planck
louis de broglie
what is another name for representative elements
group a elements
group b elements
group c elements
transition elements
what is another name from transition metals
group a elements
group b elements
noble gases
group c elements
which of the following is in the same group as phosphorus
carbon
magnesium
nitrogen
oxygen
the modern periodic table is arranged by increasing
mass
charge
number
radius
who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements
moseley
lavoisier
Dalton
Mendeleev
elements that are characterized by filling of p orbitals are classified as
groups 13-18
transition metals
inner transition metals
groups 1 and 2
which subatomic particle plays the greatest part in determining the properties of an element
electron
proton
neutron
proton and neutron
how does the atomic radius change from top to bottom in a group on a periodic table
it decreases
it increases
decreases then increases
increases then decreases
how does the atomic radius change from left to right across a period in the periodic table
decreases
increases
increase then decrease
decrease then increase
what element in the second period has the largest atomic radius
carbon
lithium
potassium
neon
metals tend to
gain electrons when they for ions
all form ions with a negative charge
all have ions with a 1+ charge
lose electrons when they form ions
a covalent bond in which the shared electron pair comes from only one of the atoms
single covalent bond
hydrogen bond
coordinate covalent bond
how many valence electrons are in an atom of phosphorus (#15)
2
3
4
5
what is the name given to the electrons in the highest occupied energy level of an atom
orbital electrons
valence electrons
anions
cations
what is the charge of a strontium ion
-2
-1
+1
+2
the octect rule states that in chemical compounds atoms tend to have
the electron configuration of noble gases
more protons that electrons
more electrons that protons
eight electrons in their principle energy level
how many electrons does barium (#56) have to give up to achieve a noble-gas electron configuration
1
2
3
4
What is the formula of an ion formed when potassium achieve noble gas electron configuration
k+2
k+1
k-1
k-2
how many electrons does nitrogen gain in order to achieve a noble gas electron configuration
1
2
3
4
what is the formula of the ion formed when phosphorus achieves noble gas electron configuration
p+3
p+2
p-2
p-3
what is the electron configuration of the calcium ion
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p4 4s2
1s2 2s2 2p6 3s2 3p6 4s1
1s2 2s2 2p6 3s2
the electron configuration of a fluoride ion F-1 is
1s2 2s2 2p5
the same as the neon atom
1s2 2s2 2p6 3s1
the same as that of a potassium ion
what is the electron configuration of the oxide ion (O-2)
1s2 2s2 2p4
1s2 2s2 2p6
1s2 2s2
1s2 2s2 2p2
what is the net charge of any ionic compound
-2
-1
0
+1
what is the formula for sodium nitride
NaN
Na2N
Na3N
NaN3
what is the formula unit of aluminum oxide
AlO
Al3O
AlO3
Al2O3
which of the following pairs of elements is most likely to form an ionic compound
magnesium and fluorine
nitrogen and sulfur
oxygen and chlorine
sodium and aluminum
which of the following particles are free to drift in metals
protons
electrons
neutrons
anions
an ionic bond is a bond between
a metal and a nonmetal
valence electrons and cations
the ions of two different metals
the ions of two different nonmetals
which of these elements does not exist as a diatomic molecule
Ne
F
H
I
which elements can form diatomic molecules held together by triple covalent bonds
hydrogen only
halogens only
halogens and members of the oxygen group only
hydrogen and halogens only
which of the following diatomic molecules is joined by a double covalent bond
O2
Cl2
N2
He2
the side-by-side overlap of p orbitals produces what kind of bond
alpha bond
beta bond
pi bond
sigma bond
according to VESPR theory molecules adjust their shapes to keep which of the following as far apart as possible
pairs of valence electrons
mobile electrons
inner shell electrns
the electrons closest to the nuclei
the shape of the methane (CH4) molecule is called
tetrahedral
square
four-cornered
planar
what causes hydrogen bonding
attraction between ions
motion of electrons
sharing of electron pairs
banding of a covalently bonded hydrogen atom with an unshared electron pair
