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203
Chemistry
11th Grade
12/16/2012

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Term
Define Chemistry
Definition
Chemistry is the study of the composition, structure, and properties of matter, the processes that matter undergoes, and the energy changes that accompany these processes.
Term
If you were studying properties of diamonds (diamonds are made of carbon), you would be studying ______ chemistry.
Definition
organic
Term
If you were studying how the intake of potassium affects the production of ATP, you would be studying ______ chemistry.
Definition
biochemistry
Term
If you were studying the energy given off by a combustion reaction, you would be studying _____ chemistry.
Definition
physical
Term
If you were studying how oxygen binds to hemoglobin (contains iron), you would be studying __________ chemistry.
Definition
inorganic
Term
If you were studying the composition of wool to determine how to make clothes softer, you would be studying _______ chemistry.
Definition
analytical
Term
If you used computers to put together a model that showed the destruction of the ozone layer, you would be studying _________ chemistry.
Definition
theoretical
Term
Use the definitions of basic research and applied research to distinguish the two terms.
Definition
Basic research is carried out for the sake of increasing knowledge, such as how or why a specific reaction occurs and what the properties of a substance are. On the other hand, applied research is generally carried out to solve a problem.
Term
What is the benefit of technological development? Name one example of technological development in our society.
Definition
The benefit is that it improves the quality of our lives. EX: biodegradable materials, computers, air conditioning
Term
Define matter. Define mass.
Definition
Matter- anything that has mass and takes up space.
Mass- a measure of the amount of matter.
Term
What are the four basic building blocks of matter?
Definition
atom, element, compound, molecule
Term
Define element.
Definition
element- a pure substance that cannot be broken down into simpler, stable substances and is made of one type of atom.
Term
Define atom
Definition
the smallest unit of an element that maintains the chemical properties of that element.
Term
What are extensive properties? Give one example
Definition
Extensive properties depend on the amount of matter present.
EX: volume, mass, amount of energy in a substance
Term
What are intensive properties? Give an example.
Definition
Intensive properties do not depend on the amount of matter present.
EX: melting point, boiling point, density, color, texture, hardness
Term
Four physical properties of a classroom desk.
Definition
1) three feet off the ground
2) tan colored
3) solid
4) flat surface
Term
What are three physical changes involved in cooking?
Definition
1) cutting
2) melting
3) boiling
Term
List two changes of state. Are changes of state classified as physical or chemical changes?
Definition
1) melting
2) boiling
Changes of state are classified as physical changes.
Term
Solids have a _________ volume and __________ shape.
Definition
Solids have a definite volume and a definite shape.
Term
Liquids have a ______ volume and _________ shape.
Definition
Liquids have a definite volume and an indefinite shape.
Term
Gases have a ______ volume and _______ shape.
Definition
Gasses have an indefinite volume and an indefinite shape.
Term
What is the main difference between a physical property and a chemical property?
Definition
A physical property is a characteristic that can be observed or measured without changing the identity of the substance, whereas a chemical property relates to a substances ability to undergo changes that transform it into different substances. Physical properties can be observed without changing the identity of the substance, chemical properties can not.
Term
List three chemical changes involved in cooking
Definition
baking chicken, grilling hamburgers, frying shrimp
Term
Chemical changes involve reactants and products. What is the difference between these two terms.
Definition
Chemical changes begin with reactants which turn into products
Term
The law of conservation of mass states that the mass of the _______ must equal the mass of the _______.
Definition
The law of conservation of mass states that the mass of the reactants must equal the mass of the products.
Term
Matter can be divided into two categories. What are they?
Definition
1) pure substances
2) mixtures
Term
What is the difference between a homogeneous mixture and a heterogeneous mixture? Give an example of each.
Definition
homogeneous is consistent throughout (sweet tea)
heterogeneous is not consistent throughout (salsa)
Term
An _________ like lithium or a ________ like salt can both be considered pure substances.
Definition
An element like lithium or a compound like salt can both be considered pure substances
Term
A compound can be broken down into elements by what kind of change?
Definition
a chemical change
Term
Horizontal rows on the periodic table are called _________.
Definition
periods
Term
Vertical columns on the periodic table are called _________.
Definition
groups
Term
What is the scientific method?
Definition
A logical approach to solving problems
Term
List the four steps to the scientific method.
Definition
observe, hypothesize, experiment, conclude
Term
There are two types of data. What are they? How can you tell the difference between the two?
Definition
1) qualitative - data that deals with descriptive information
2) quantitative- data that deals with numerical information
Term
When testing a hypothesis the experimenter should use controls, why?
Definition
To have a way to compare the results of your experiment
Term
Use the definition of dependent variable and independent variable to distinguish the two terms.
Definition
dependent variable- the variable that changes because of the independent variable
independent variable- the variable that is changed by the scientist
Term
If you were to do an experiment to test to see which paper towel was the most absorbent, list three controls.
Definition
1) amount of paper towel used
2) amount of liquid used
3) type of liquid used
Term
Based on the paper towel experiment, what would be the independent variable and the dependent variable?
Definition
independent variable- paper towel brand
dependent variable- how much liquid was absorbed
Term
What is the next step if the hypothesis is not supported by the experiment?
Definition
Either revise or reject the hypothesis.
Term
What is a theory? What is a hypothesis?
Definition
theory- a broad generalization that is supported by many experiments

hypothesis- a testable statement
Term
What two things make up a measurement?
Definition
1) number
2) unit
Term
The SI Units are used across the world for science. Why is it important that scientists all use the same units?
Definition
So that scientists across the world use the same units which allows results to be shared
Term
List the seven SI base units.
Definition
meter, gram, second, kelvin, mole, ampere, candela
Term
How are the base units manipulated to account for large and small measurements?
Definition
prefixes are added
Term
How does mass differ from weight?
Definition
mass is not dependent on gravity, weight is
Term
What does volume measure? List three units for volume.
Definition
Volume measures the amount of space an object takes up.
Units for volume:
1) cm cubed
2) mL
3) L
Term
What is the formula for density? What is the unit for density?
Definition
D= m/v
density = mass divided by volume.
the unit for density is g/mL or g/cm^3
Term
Can density be measured directly? How did we determine the density of a penny in the penny lab?
Definition
No. In the penny lab we used a scale to find the mass, then the water displacement method to find volume. We then calculated density with the formula.
Term
Why does ice float in water?
Definition
Ice has a lower density than water.
Term
Convert 435g to mg.
Definition
435,000 mg
Term
convert 3.54 cm^3 to L.
Definition
3.54cm^3 = 3.54mL = 0.00354 L
Term
What is the difference between accuracy and precision?
Definition
accuracy- the closeness of a measurement to the accepted value
precision- the closeness of a set of measurements to each other
Term
Are the following test scores accurate, precise, neither or both? 74, 70, 76
Definition
They are precise but not accurate
Term
What does the percent error tell you about your experiment? Is a high percentage or a low percentage a more accurate experiment?
Definition
How close your data is to the accepted data. A low % is a more accurate experiment
Term
If the actual value for the density of copper is 7.34 g/mL and the value you recorded after your lab was 8.42 g/mL, what is the percent error of your experiment?
Definition
[(accepted-experimental)/accepted]*100
[(8.42-7.34)/7.34]*100=14.7%
Term
How many significant figures in each of the following numbers?
a) 52.5200
b)3003
c)20300
d)3.500
e)0.00254
f)900
g)200500.0
h)8290
i)0.00520
Definition
a)5
b)4
c)3
d)4
e)3
f)1
g)7
h)3
i)3
Term
Who was the first person to believe that matter was made up of smaller particles?
Definition
Democritus
Term
Was Democratis supported? why or why not?
Definition
no, there was no proof for his ideas
Term
Why did it take nearly 2,000 years before anyone developed these ideas of whether matter is made of smaller particles or not?
Definition
It was not until then that there was technology that allowed proof
Term
State the laws of definite and multiple proportions; be able to identify both on the exam.
Definition
law of definite proportions- a compound contains the same elements in the same proportions by mass regardless of the size or source of the compound

law of multiple proportions- if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always in a ratio of small whole numbers
Term
Who developed atomic theory?
Definition
Dalton
Term
What is the first statement of the atomic theory?
Definition
all matter is composed of small particles called atoms
Term
What are the two modifications that have been made to the atomic theory?
Definition
1) atoms are divisible
2) not all atoms of the same element are identical
Term
Define atom
Definition
the smallest particle of an element that retains the chemical properties of that element
Term
What are the three subatomic particles that make up the atom?
Definition
proton, neutron, and electron
Term
Who discovered that subatomic particles existed by performing the cathode ray experiment?
Definition
Thomson
Term
How did scientists determine that the cathode ray was composed of negatively charged particles?
Definition
When a negative plate was put up to the glass tube, the cathode ray inside bent away from the negative charge.
Term
Describe the setup of Rutherford's gold foil experiment.
Definition
Rutherford shot alpha particles at a sheet of gold foil, the experiment was surrounded by zinc sulfide which would flash if hit by the alpha particle.
Term
What surprised scientists when observing the gold foil experiment?
Definition
That some of the alpha particles hit the gold foil and bounced back
Term
What result of the gold foil experiment proved that the atom was made mostly of empty space?
Definition
Most of the alpha particles went straight through undisturbed.
Term
What result of the gold foil experiment proved that the nucleus was dense?
Definition
Whatever caused the large alpha particle to stop and change direction must be massive, a large mass and a small volume means that the particle is dense
Term
What result of the gold foil experiment proved that the nucleus was positively charged?
Definition
The positive charged alpha particles were deflected. Like charges repel one another
Term
What do nuclear forces do?
Definition
They hold the nucleus together
Term
What two particles are located inside the nucleus?
Definition
proton and neutron
Term
The number of protons in an atom can also be called the ________.
Definition
atomic number
Term
Isotopes differ in two ways. What are the two ways?
Definition
1) number of neutrons
2) mass
Term
Name three ways that isotopes are the same.
Definition
1) number of protons
2) number of electrons
3) chemical behavior
Term
The total number of protons and neutrons can also be called the ______.
Definition
mass number
Term
What does amu stand for?
Definition
atomic mass unit
Term
The unit amu is based on which isotope?
Definition
carbon-12
Term
Identify the mass in amus for the proton, neutron, and electron
Definition
proton = 1 amu
neutron = 1 amu
electron = 0 amu
Term
List three types of electromagnetic radiation.
Definition
gamma rays, X-rays, UV rays
Term
List the one thing that all waves have in common.
Definition
They all travel at the speed of light. (3.00 *10^8 m/s)
Term
List three ways that waves are different.
Definition
1) wavelength
2) frequency
3) energy
Term
Describe the difference between frequency and wavelength.
Definition
wavelength- the distance between equivalent points on adjacent waves

frequency- the number of waves that pass a given point in one second
Term
Wavelength and frequency are related ________.
Definition
indirectly
Term
Energy and frequency are related _________.
Definition
directly
Term
Who first came up with the idea that energy was emitted as particles not as waves?
Definition
Planck
Term
Einstein came up with the dual __________-___________ nature for electromagnetic radiation.
Definition
dual wave-particle nature.
Term
What is a photon?
Definition
a particle of electromagnetic radiation carrying a quantum of energy
Term
Describe how an electron moves from ground state to excited state and back to ground state.
Definition
An electron in its lowest energy state is in its ground state, when it absorbs energy it moves to an excited state, it gives off a photon and moves back to ground state.
Term
What is released when an electron moves from excited state to ground state?
Definition
a photon
Term
What is the difference between ground state and excited state?
Definition
ground state- lowest energy level
excited state- higher energy level
Term
Each atom has its own ___________ ________________ ______________ that can be used to identify the element, much like a fingerprint.
Definition
atomic emission spectrum
Term
How did Bohr describe the movement of electrons?
Definition
moved around the nucleus in organized orbits like planets orbit around the sun
Term
The further the electron is away from the nucleus the ( more / less ) energy it has.
Definition
more
Term
What is the difference between absorption and emission?
Definition
absorption- taking in energy
emission- giving off energy
Term
What three scientists contributed to the current Quantum Model of the Atom?
Definition
de Broglie, Heisenberg, Schrodinger
Term
What is predicted by the Schrodinger equation?
Definition
the probability of finding an electron in a given orbital
Term
State the Heisenberg Uncertainty Principle
Definition
The position and velocity of an electron cannot be determined simultaneously.
Term
What is an atomic orbital?
Definition
a region of space where an electron is likely to be found
Term
How many energy levels are possible in an atom?
Definition
7
Term
Each energy level contains sub levels. What are the four sub-levels and their shapes?
Definition
1) s -sphere
2) p -dumbbell
3) d -4 leaf clover
4) f -complicated
Term
Each sub-level contains orbitals. How many orbitals are in each type of sub-level?
Definition
s-1
p-3
d-5
f-7
Term
How many electrons are required to fill the first energy level?
Definition
2
Term
How many electrons can go into the third energy level?
Definition
18
Term
What information can be determined from the description 5s^2?
Definition
electrons are located in the 5th energy level in a spherical shaped sub-level and there are 2 electrons present.
Term
How is a nuclear equation different from a chemical equation? (give at least two differences)
Definition
nuclear equations- change atoms from reactant to product; give off large amounts of energy

chemical equations- atoms stay the same from reactant to product; give off small amounts of energy
Term
What are the main subatomic particles involved in a chemical equation?
Definition
electrons
Term
What are the main subatomic particles involved in a nuclear equation?
Definition
protons and neutrons
Term
Which type of reaction, chemical or nuclear, give larger releases of energy?
Definition
nuclear
Term
What are the three types of radiation?
Definition
alpha, beta, and gama
Term
Rank the three types of radiation from most massive to least massive.
Definition
alpha, beta, gamma
Term
Rank the three types of radiation from most penetrating to least penetrating.
Definition
gamma, beta, alpha
Term
How did Rutherford determine that there were three types of radiation?
Definition
placed a positive and negative plate above and below a radioactive substance; beta was attracted to the positive plate, alpha was attracted to the negative plate, and gamma was unaffected
Term
What was Roentgen's contribution to nuclear chemistry?
Definition
developed the X-ray
Term
What was Becquerel's contribution to nuclear chemistry?
Definition
determined that radioactive substances spontaneously give off radiation
Term
What was the Curie's contribution to nuclear chemistry?
Definition
isolated radium and plonium
Term
Cobalt-60 has a half-life of 5.27 years. How much of a 165g sample remains after 26.35 years?
Definition
5.16 g
Term
How are fission and fusion similar?
Definition
fission and fusion are both nuclear processes.
Term
How are fission and fusion different?
Definition
fission- splitting of a large atom to release energy
fusion- joining of smaller atoms to release energy
Term
What are the only two fissionable isotopes?
Definition
uranium and polonium
Term
How is fission a chain reaction?
Definition
fission begins when a neutron hits an unstable uranium atom. When this reaction is complete, 3 neutrons are given off allowing the reaction to continue.
Term
How is the speed of the fission reaction controlled in a nuclear reactor?
Definition
by using control rods to absorb neutrons and slow down the reaction
Term
The reactor heats the water which generates steam. The steam turns the _____ which generates _____.
Definition
turbine; electricity
Term
What is the only substance that produces energy from fusion?
Definition
the sun
Term
What are the current limitations that are keeping us from using fusion as a main power source?
Definition
temperature required is very high; also, we have to develop a container to hold this extremely high temperature.
Term
What is a spent fuel rod?
Definition
a rod that use to contain fissionable uranium atoms, but has used all the uranium
Term
What is done with the spent fuel rods after they are removed from the nuclear reactor?
Definition
they are put in spent fuel pools (swimming pools)
Term
What are some benefits to using nuclear reactors to make energy compared to other methods?
Definition
cheap, release no harmful gases into atmosphere, easy to do
Term
What are some drawbacks to using nuclear reactors to make energy compared to other methods.
Definition
give radioactive product that must be stored, plants are expensive to build
Term
What is the unit used to measure the dose of radiation absorbed by humans?
Definition
rem
Term
What are three methods used to detect radiation?
Definition
film bodge, Geiger counter
Term
List 5 uses of nuclear chemistry.
Definition
bombs, X-rays, cancer treatment, to make energy, smoke detectors
Term
______ came up with arranging the elements in order of their repeating properties. He arranged the elements in order of increasing atomic mass.
Definition
Mendeleev
Term
_______ later revised the periodic table by arranging the elements in order of increasing _____ ________.
Definition
Moseley; atomic number
Term
State the periodic law.
Definition
when the elements are arranged in order of increasing atomic number their properties will repeat.
Term
What is the name of group 1 elements?
Definition
Alkali metals
Term
What is the name of group 2 elements?
Definition
Alkaline Earth metals
Term
What is the name of group 17 elements?
Definition
Halogens
Term
What is the name of group 18 elements?
Definition
Noble Gases
Term
What is the name of groups 3-12?
Definition
transition metals
Term
What are the names of the two rows that make up the f-block?
Definition
Lanthanides and Actinides
Term
What are metalloids? Where are they located on the periodic table?
Definition
substances that have properties of both metals and nonmetals
Term
List three properties of metals. Where are they located on the periodic table?
Definition
good conductors, malleable, ductile; to the left of the stair-step line
Term
list three properties of nonmetals. Where are they located on the periodic table?
Definition
bad conductors, not malleable, brittle; right of the stair-step line
Term
List three properties of s-block metals.
Definition
soft, very reactive, good conductors
Term
List two properties of p-block metals.
Definition
harder than s-block metals, not as reactive as s-block metals
Term
list four properties of d-block metals.
Definition
shinny, good conductors, hard, malleable
Term
Explain why group 18 is referred to as the noble gases?
Definition
because their outer energy level is full and they do not interact (bond) with any other elements
Term
Explain what the atomic radius measures.
Definition
distance from nucleus to edge of electron cloud
Term
How is the atomic radius of an atom actually measured?
Definition
distance between 2 nuclei divided by 2
Term
What is the period trend or the atomic radius? The group trend?
Definition
period trend= decreases to the right
group trend= increases going down
Term
Rank the following elements from largest radius to smallest radius: Cl, I, Br, C, F, Li
Definition
I, Br, Cl, Li, C, F
Term
What is the group trend for ionic radius?
Definition
increases as go down groups
Term
What is the difference between a cation and an anion? Include how each is formed.
Definition
-cation is a positive ion that forms when electrons are lost
-anion is a negative ion that forms when electrons are gained
Term
What is the period trend for ionization energy? The group trend?
Definition
period: increases to the right
group: decreases going down
Term
What is ionization energy?
Definition
the energy required to remove an electron from an atom
Term
When an electron is removed from an element a ( cation / anion ) is formed. Are metals or nonmetals more likely to do this?
Definition
cation; metals
Term
What is electronegativity?
Definition
the attraction for electrons in a chemical bond
Term
What is the most electronegative element?
Definition
fluorine
Term
Why do elements bond?
Definition
to become stable
Term
What electrons are involved in the bonding process?
Definition
valence electrons
Term
What types of elements are combined in a compound? what type of bonding? List one example of a compound.
Definition
metal and nonmetal; ionic; NaCl
Term
List three properties of ionic compounds.
Definition
high melting point, conduct when liquid, brittle
Term
What is the overall charge of ionic compounds?
Definition
zero (neutral)
Term
How are ionic bonds formed?
Definition
metal cation is attracted to a nonmetal anion
Term
Why can ionic compounds not conduct electricity in the solid state?
Definition
because the anions are not free to move; surrounded by cations
Term
What is a cation? Give an example.
Definition
an ion with a positive charge
Ex: Mg 2+
Term
What is an anion? Give an example?
Definition
An ion with a negative charge.
Ex: O2-
Term
Why, when writing the name of a compound that contains a transition metal, does a Roman numeral have to be included?
Definition
Because transition metals do not always form the same ion; the correct one is indicated with a Roman numeral
Term
What is a binary compound? All binary compounds, whether ionic or covalent, will end with what suffix?
Definition
a combination of 2 elements; will end with -ide
Term
What is a polyatomic ion?
Definition
an ion composed of more than one atom.
Term
What is the term used in metallic bonding that describes the fact that electrons do not belong to one particular atom?
Definition
delocalized electrons
Term
Why are electrons delocalized in metals?
Definition
because the outer energy levels overlap
Term
Why are metals good conductors of heat and electricity?
Definition
because the delocalized electrons are free to move
Term
Why are metals shiny?
Definition
because delocalized electrons are free to move
Term
What types of elements are combined in a molecule? what type of bonding? List one example of a molecule.
Definition
nonmetal and nonmetal; covalent; CO2
Term
What is a diatomic molecule?
Definition
a molecule containing 2 atoms
EX: Cl2 or CO
Term
Which bonds are stronger, ionic or covalent?
Definition
ionic
Term
What would melt first, a block of ice or a grain of salt? Why?
Definition
block of ice; ice is covalent and salt is ionic; because ionic is stronger than covalent, covalent will melt first
Term
How many electrons are shared in a single bond?
Definition
two
Term
How many electrons are shared in a double bond?
Definition
4
Term
How many electrons are shared in a triple bond?
Definition
6
Term
Rate single, double, and triple bonds from longest to shortest. From strongest to weakest.
Definition
longest-shortest: single, double, triple
strongest-weakest: triple, double, single
Term
What is the difference between a lone pair of electrons and a shared pair of electrons?
Definition
lone pair belong only to one atom, shared pair is shared between two atoms
Term
State the octet rule
Definition
each atom will lose, gain, or share to achieve 8 electrons in their outer energy level
Term
What are the two exceptions to the octet rule?
Definition
Hydrogen and helium (they only want 2, not 8)
Term
What three things must be checked in order for a Lewis structure to be correct?
Definition
total number of electrons, octet rule, used correct number of atoms
Term
Lewis structures represent molecules in 2D, in order to represent molecules in 3D what theory must be used?
Definition
VSEPR theory
Term
What is the VSEPR theory?
Definition
describes the 3D arrangement of atoms in a molecule
Term
When assigning variables to molecules in order to determine the VSEPR shape, what does A represent? What does B represent? what does E represent?
Definition
A- central atom
B- atoms bonded to central atom
E- lone pairs of electrons on the central atom
Term
Why do the trigonal planar and bent shapes have bond angles less than 109.5ยบ?
Definition
because more than one correct lewis structure can be drawn
Term
Polar bonds and nonpolar bonds are the two types of covalent bonds. How are they different? Give an example of each.
Definition
polar bonds- electrons shared unequally (partial charges present) EX: H-F
nonpolar bonds- electrons shared equally (no partial charge present) EX: O-O
Term
How is an intermolecular force different from an ionic or covalent bond?
Definition
intermolecular forces occur between molecules; intro molecular forces (ionic and covalent) occur within molecules
Term
List three types of intermolecular forces
Definition
dispersion, dipole, hydrogen bonding
Term
How can you determine the strength of a covalent bond?
Definition
electronegativity difference
Term
Hydrogen bonding occurs when hydrogen bonds to which 3 elements?
Definition
F, O, N
Term
London dispersion forces exist between ________ molecules.
Definition
all
Term
Dipole-dipole forces exist only between _____ molecules.
Definition
polar
Term
Why are partial charges used in polar molecules?
Definition
there is an unequal distribution of electrons
Term
How is it determined which atom in the bond gets the partial negative charge?
Definition
the more electronegative atom gets the partial negative.
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