organic chemistry
the study of all chemicals containing carbon
inorganic chemistry
the study of chemicals that do not contain carbon
biochemistry
the study of the processes that take place in organisms
analytical chemistry
the study of the composition of matter
physical chemistry
concerned with the mechanism, rate, and energy transfer that occurs when matter undergoes a change
which of the following was a major contribution to chemistry by Lavoisier
He showed that oxygen is required for material to burn
a theory is
a well tested explanation for a broad set of observations
which step in the scientific method requires you to use your sense to obtain information
making an observation
the step that usually comes last in solving numeric problems is
evaluate
mixture
physical blend of two or more compounds
product
substance formed in a chemical reaction
phase
part of a sample having uniform composition and properties
reactant
starting substance in a chemical reaction
heterogeneous
not uniform in composition
vapor
gaseous state of a substance that is a liquid or solid at room temperature
distillation
process in which a liquid is boiled to produce a vapor that is condensed again into a liquid
mass
amount of matter an object contains
chemical reaction
process in which substances are changed into different substances
compound
composed of two ore more substances chemically combined in a fixed proportion
element
substance that can't be changed into simpler substances by chemical means
homogenous
describes a mixture with a uniform composition
which of the following is not an example of matter
air
an example of an extensive property of matter is
mass
all of the following are physical properties of matter except
ability to rust
which of the following are considered physical properties of a substance
all the above
a vapor is which state of matter
gas
which state of matter takes both the shape and volume
gas
which state of matter is characterized by having definite shape and definite volume
solid
which of the following is a physical change
evaporation
which of the following can't be considered a single phase
heterogeneous mixture
separating a solid from a liquid by evaporation the liquid is called
distilliation
which of the following is true about compounds
they are substances
the chemical symbol for iron is
Fe
Which of the following represents a compound
H2O
in the chemical reaction in which sucrose is heated and decomposes to form carbon dioxide and water, which of the following is a reactant
sucrose
which of the following does not involve a physical change
decomposing
what is the melting point of water in C
0
How many physical states does water commonly exist
3, solid, lliquid, gas
what is the boiling point of water in C
78
How many grams of liquid water are produced when 60 grams of ice melt
60
absolute zero
the lowest point on the Kelvin scale
Kelvin
SI scale for temperature
Celsius
no SI scale for temperature
weight
force of gravity on an object
mass
the quantity of matter an object contains
significant figure
known or estimated in a measurement
precision
narrowness of range of measurements
accuracy
closeness to true value
the diameter of a carbon atoms is 0.000000000154m. What is this number in scientific notation
1.54 x 10^-10
what is the result of multiplying 2.5 x 10^10 by 3.5 x 10^-7
8.75 x 10^3
the closeness of a measurement to its true value is its
accuracy
which of the following measurements is the most accurate
3.000000 g
which of the following measurements is expressed to 3 sig figs
7.30 x 10^-7
how many sig figs are in the measurement 0.0034 kg
2
how many sig figs are in the measurement 40500
3
express the sum of 111 and 222 using the correct number of sig figs
1333
express the product of 2.2 and 5.00 using sig figs
11
what is 111.099 rounded to 4 sig figs
111.0
what quantity is represented by the metric system prefix deci
.1
what is the metic system prefix for 0.000001
micro
which of the following units is the largest
1 dg
Chlorine boils at 239 K. What is the boiling point in C
-34
a cubic meter is about the same as the volume occupied by a
washing machine
what is the density of an object having a mass of 8.0 grams and a volume of 25 cm^3
.32 g/cm^3
what is the volume of 45.6 g of silver if the density of silver is 10.5 g/cm^3
4.34 mL
if the temperature of a piece of steel decreases, what happens to its density
density increases
round 0.0030955 to 3 sig fig
.00309
what is the sum of 2.7 and 2.47
5.2
what is the sum of 6.210 and 3
9
what is the product of the number 1000 and the measurement .00357
3.57
what is .05 grams in kilograms
5 x 10^-5
what is .06 liters in cubic meters
6 x 10^5
what is the volume of an object with a density of 7.73 and a mass of 5.40 x 10^2
69.9
proton
positively charge subatomic particle
nucleus
central part of an atom, containing protons
atom
smallest particle of an element that retains the properties of that element
electron
negatively charged subatmic particle
neutron
subatomic particle with no charge
mass number
total number of protons and neutrons in the nucleus of an atom
atomic mass unit
1/12 the mass of a carbon atom having six protons and six neutrons
atomic number
number of protons in the nucleus of an element
atomic mass
weighted average of the masses of the isotopes of an element
isotop
atoms with the same number of protons, but different numbers of neutrons in the nucleus of an atom
who was the man to first suggest the idea of atoms
Democritus
smallest particle of an element that retains the properties of that element is an
atom
which of the following is not a part of dalton's atomic theory
atoms are always in motion
who conducted experiments to determine the quantity of charge carried by an electron
Millikan
what is the relative mass of an electron
1/1840 the mass of a hydrogen atom
which of the following is correct concerning subatomic particles
the neutron was discovered by Chadwick
as a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true
electrons are distributed around the nucleus and occupy almost all the volume of the atom
the nucleus of an atom is
the central core and is composed of protons and neutrons
the atomic number of an element is the total number of which particles in the nucleus
protons
an element has an atomic number of 76. the number of protons and electrons in a neutral atoms of the element are
76 protons, 76 electrons
all atoms of the same element have the same
number of protons
in which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly
In, 49 and 49
what is the number of neutrons in isotope 16O
8
if E is the symbol for an element, which two of the following symbols represent isotopes of the same element
1 and 4
select the correct symbol for an atom of tritium
3/1 H
in which of the following is the number of neutrons correctly represented
238/92 U has 146 neutrons
which of the following isotopes has the same number of neutrons as phosphorus-31
32/16 S
What unit is used to measure weighted average atomic mass
amu
which of the following statements is NOT true
the nucleus of an atom is positively charge
the atomic mass of an element is the
weighted average of the masses of the isotopes of the element
list the number of proton, neutrons, and electrons in 13/6 C
p - 6
n - 7
e - 6
chlorine has 2 naturally occurring isotops Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant
Cl-35
Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is 45.0% abundant. What is the average atomic mass for
19.9
A fictitious element X is composed of 10 percent of the isotope 55X, 20 percent of the isotope 56X and 70 percent of the isotope 57X. Estimate the atomic mass of element X
56.6
the element chromium has four naturally occurring isotopes. Use the relative abundance of each to calculate the average atomic mass of chromium.
50Cr= 4.34%, 52Cr= 83.79%, 53Cr= 9.50%, 54Cr= 2.37%
52.06
What is the charge carried by an electron
-1
what is the charge of a proton
+1
about how many more times massive is a proton than an electron
one
determine the number of electrons in a neutral atom of Li
3
determine the number of protons in an atom of Ba
56
how many protons are present in an atom of Be-9
4
what is the total number of subatomic particles in the nucleus of an atom of 209/83 Bi
209
determine the number of electrons in an atom of Iridium
77
what is the atomic number for an element with 41 neutrons and a mass number of 80
39
how may electrons are in an atom of gold
79
what is the mass number for an oxygen atom that has 10 neutrons in its nucleus
18
how many protons are present in the nuclei of the 3 known isotopes of hydrogen
one
determine the number of neutrons in N-14
7
how many neutrons are present in an atom of the isotope 235/92 U
143
calculate the number of neutrons in 210Pb
128
atomic orbital
region of high probability of finding an electron
aufbau principle
tendency of electrons to enter orbitals of lowest energy first
electron configuration
arrangement of electrons around atomic nucleus
ground state
lowest energy level
Pauli exclusion principle
each orbital has at most two electrons
Heisenberg uncertainty principle
states the impossibility of knowing both velocity and position of a moving particle at the same time
n Bohr's model of the atom, where are the electrons and protons located?
the electrons move around the protons, which are at the center of the atom
How does the energy of an electron change when the electron moves closer to the nucleus?
decreases
the principle quantum number indicates what property of an electron
energy level
how many energy sublevels are in the second principle energy level
2
what is the maximum number of f orbitals in any single energy level in an atom
7
what is the maximum number of electrons in the second principal energy level
8
when an electron moves from a lower to high energy level, the electron
absorbs a quantum of energy
What types of atomic orbitals are in the third prinicipal energy level
s,p,d
according to the aufbau principle
electrons enter orbitals of highest energy first
what is the electron config of potassium
1s22s22p23s23p24s1
how many unpaired electrons are in a sulfur atom
2
stable electron config are likely to contain
filled energy sublevels
which of the following electron configs of outer sublevels is the most stable
4d55s1
which of the following electromagnetic waves have the highest frequencies
gamma rays
how are the frequency and wavelength of light related
they are inversely proportional to each other
what is the wavelength of an electromagnetic wave that travels at 3x10^8 and has a frequency of 60 MHZ
300,000,000 / 60,000,000
emission of light from an atom occurs when an electron
drops from a higher to a lower energy level
What is the approximate frequency of a photon having an energy 5x10^-24
8 x 10^9
which variable is directly proportional to frequency
energy
what are quanta of light called
photons
electronegativity
ability of an atom to attract electrons when the atom is in a compound
ionization energy
energy required to remove an electron from an atom
atomic radius
1/2 the distance between the nuclei of two atoms when the atoms are joined
metal
type of element that is a good conductor of heat and electric current
transition metal
type of element characterized by the presence of electrons in the d orbital
periodic law
a repetition of properties occurs when elements are arranged in order of increasing atomic number
cation
type of ion formed by Group 2A elements
period
horizontal row in the periodic table
groups
vertial column in the periodic table
electrons
subatomic particles that are transferred to form positive and negative ions
which of the following elements ins in the same period as phosphorus
magnesium
each period in the periodic table corresponds to
a principal energy level
the modern periodic talbe is arranged in order of increasing atomic
number
who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements
Dmitri Mendeleev
of the elements Pt, V, Li, and Kr, which is a nonmetal
Kr
what element has the electron config of 1s22s22p63s23p2
silicon
which subatomic particle plays the greatest part in determining the properties of an element
electron
Which is a representative element Fe, Hg, U, and Te
Te
how does atomic radius change from left to right across a period in the periodic table
decrease
what causes the shielding effect to remain constant across a period
electrons are added to the same principle energy level
what element in the second period has the largest atomic radius
Li
Which element has the smallest atomic radius
chlorine
what is the charge of a cation
positive
which of the following statements is NOT true about ions
when a cation forms, more electrons are transferred to it
why is the second ionization energy greater than the first
it is more difficult to remove a second electron from an atom
in which of the following groups of ions are the charges shown correctly
Ca+2, Al+3, Br-
what is the element with the highest electronegativity value
fluorine
what is the energy required to remove an electron from an atom in the gaseous state called
ionization energy
from Group 2A metals, which electron is the most difficult to remove
the third
which of the following elements has the smallest first ionization energy
potassium
compared with the electronegatives of the elements on the left side of a period, the electronegativites of the elements on the right side of the same period tend to be
higher
which of the following decreases with increasing atomic number in Group 2A
ionization energy
of the following elements, which one has the smallest first ionization energy
Al
halide ion
an anion of chlorine or other halogen
octet rule
atoms react so as to acquire the stable electron structure of a noble gas
ionic bond
force of attraction biding oppositely charged ions together
electron dot structure
depiction of valence electrons around the symbol of an element
valence electron
an electron in the highest occupied energy level of an atom
coordination number
number of ions of opposite charges surrounding each ion in a crystal
metallic bond
the attraction of valence electrons for metal ions
how many valence electrons are in P
5
how many valence electrons are in Si
4
What is the maximum charge an ion is likely to have
3
what is the charge on the Sr ion
+2
the octet rules states that in chemical compounds atoms tend to have
the electron config of a noble gas
how many electrons does silver have to give up in order to achieve a pseudo-noble gas electron config
1
what is the formula of the ion formed when potassium achieves noble gas electron configuration
K+
which of the following elements does NOT form an ion with a charge of +1
fluorine
how does oxygen obey the octet rule when reacting to form compounds
gains electrons
what is the charge on the action in the ionic compound sodium sulfide
+1
which of the following occurs in an ionic bond
oppositely charge ions attract
what is the net charge of the ionic compound CaF
0
which of the following is true about an ionic compound
all the above
Chemical symbol for sodium nitride
Na3N