Chemistry Honors Final 2012

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