Finals Flash Cards
Matter is defined as anything that occupies space and has
Mass
Which pair Is classified as a substance
Elements and Compounds
Which of the following statements is an identifying characteristic of a mixture?
Can be separated by physical means
When sample X is passed through a filter paper, a white residue, Y, remains on the paper and a clear liquid, Z, passes through. When liquid Z is vaporized, another white residue remains. Sample X is best defined as
Heterogeneous Mixture
What best describes a chemical property of the element Iodine?
It reacts with Hydrogen to form a gas
Ductility and malleability are examples of
Physical Properties
How man kilo-joules is the equivalent of 750 joules
.750 kj
Review 8-12 in the packet
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Compounds are usually broken down into their component elements by
Chemical Changes
Which Substance can be decomposed by chemical change?
Ammonia (Anything that is a substance and not an element)
What is an EXTENSIVE physical property?
Mass
How many kilo-joules of heat energy are absorbed when 100 grams of water is heated from 20 degrees Celsius to 30 degrees Celsius
4.18kj
What is the total number of joules of heat energy released when 20 grams of water is cooled from 20 degrees Celsius to 10 Degrees Celsius
836J
Homo means
Evenly Mixed
Hetero means
Unevenly Mixed
Intensive means
Value stays the same
Study 19 In Packet
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An ideal gas is made up of gas particles that
are in random motion
What are the qualities of an ideal gas
Random Motion, Little attraction for each other, Insignificant volume, Hit wall and build up pressure, Hit each other and transfer energy but total energy remains the same
What are the qualities of a real gas?
Has volume, have force of attraction
Normal Units of pressure
STP, 1 atm, 0 degrees Celsius, 760 mmHg, 273 Kelvin, 760 torr
Equation for Volume Pressure, Temperature and Moles
V1 Phave 1 = V2 P2
____________
T1 n1 = T2 n2
An assumption of the kinetic theory of gas is that the particles of a gas have
little attraction for each other and an insignificant volume
The pressure on 30 milliliters of an ideal gas icreases from 101.3 kPa to 202.6 kPa at constant temperature. The new volume is equal to
101.3 kPa
30 mL x ________
202.6 kPa
A sample of gas has a volume of 2.0 liters at a pressure of 1.0 atm. When the volume increases to 4.0 liters, at a constant temperature, the pressure will be
.5 atm
a 2.5 liter sample of gas is at STP. When the temperature is raised to 273 degrees Celsius and the pressure remains constant the new volume of the gas will be
5.0 Liters
S 16 Liter sample of CH4(g) is at 0 degrees Celsius and 1 atm. The volume of the gas sample in liters at 27 Degrees Celsius and 1 atm is equal to
300
22.4 x _____
273
When 7.0 Moles of gas A and 3.0 moles of Gas B are combined, the total pressure exerted by the gas mixture is 1.0 atm. What is the partial pressure exerted by gas A in this mixture
.7 atm
Which gas will diffuse at the rate under the same conditions of temperature and pressure
H2
A .50 mole sample of CO2(g) at 2.0 atm occupies 11.2 liters. What is the temperature of the sample
546 K
The density of a gas is 3.00 grams per liter at STP What is the gram molecular mass of the gas
22.4g
What is the formula for Lead (II) Oxide
PbO
No “o”
Hydro
O
Hydro
Ate becomes your
Ic
Ite becomes your
Ous
Complete Combustion
—–> CO2 + H2O
Incomplete Combustion
—–> CO + H2O
What order you go in when balancing equation
HCO
What is the formula for Chromium (III) Oxide
Cr2O3
Which Formula is correctly paired with its Name
CuCl2 —–> Copper (II) Chloride
What is the correct name for the compound with the formula CrPO4
Chromium (III) Phosphate
What is the name of the compound whose formula is H2SO4
Sulfuric Acid
The chemical equation 4Na(s) + O2 —> 2Na^2O(s) is best described as a
Synthesis reaction
What type of reaction is illustrated by the following chemical equation 2H2O(l) —> 2H2(g) + O2(g)
Decomposition
The chemical reaction Zn(s) + CuSO4(aq) —> ZnSO4(aq) + Cu(s) is best described as a
Single replacement reaction
What type of reaction best describes the following chemical reaction 2AlCl3(aq) + 3Na2CO3(aq) —> Al2(CO3)3(s) + 6NaCl(aq)
Double replacement reaction
C2H4(g) + 3O2(g) —> 2CO2(g) + 2H2O(g)
Complete Combustion
When the equation C2H4 + 3O2 —> 2CO2 + 2H2O balanced using the smallest whole numbers, what is the coefficient of the O2
3
Al2(SO)3 + 3ZnCl2 —> 2AlCl3 + 3ZnSO4 is correctly ballanced using the smallest whole number coefficient, the sum of the coefficients is
9
KCl(aq) + AgNO3(aq) —> KNO3(aq) + X What is the correct formula for the product representing X
AgCl
In the 1880’s JJ Thomson proved the cathode ray hadn a negative charge. What subatomic particle makes up the cathode rays
Electrons
What did the discovery of cathode rays reveal about the structure of the atom
Made of subatomic Particles
Most alpha articles passed through the gold foil undeflected. What conclusion was made about the structure of the atom based on this observation
Mostly empty space, had to be some postive ions
A few alpha particles were deflected back at the source. What did this observation reveal about the structure of the atom
Small dense positive nucleus
What term refers to the region of an atom where an electron is most likely to be found
orbital
The atomic number of an atom is always equal to the total number of
Protons and Neutrons
All atoms of an element have the same
Atomic Number
The mass number of an atom is equal to the number of
Neutrons plus electrons
What is the mass number of the atom below? 3 H
1
3
Where is mass
On top
How do you find neutrons
Subtract two numbers
In which pair of atoms do both neclei contain the same number of neutrons
Whichever two subtract to the same number
What is the total number or nucleons (protons and neutrons) in the atom below
Top number is mass and mass is equal to protons+neutrons= Nucleons
What is the mass number of an atom which contains 21 electrons, 21 protons, and 24 neutrons
45
Find the average mass of a sample of magnesium which contains 78.7% Mg-24, 10.1% Mg-25 and 11.2% Mg-26
(24)(.787)+(25)(.101)+(26)(.112)=24.3
Element X has two isotopes. If 72% of the element has an isotopic mass of 84.9 atomic mass units, and 28% of the element has an isotopic mass of 87 atomic mass units, the average atomic mass of element X is numerically equal to
(72.0 x 84.9) (28.0 x 87.0)
___________ + ____________
100 100
The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (show percents) produces this average mass?
75%^35Cl and 25%^37Cl
Which electron dot symbol could represent a metalloid (B, Si, As, Te, At)
If it has 5 dots around it
The characteristics bright-line spectrum of an element is produced when its electron
Returns to a lower energy state
Which electron configuration represents a potassium ion in the excited state
Add up then identify element if matches, ground state if not excited
What is the total number of occupied sublevels in an atom of chlorine in the ground state
5
An atom has 8 electrons in a d sublevel. How many d orbitals in this sublevel are half filled
2
How do the orbitals go
2, 8, 18, 32, 50
What is the total number of sublevels in a principal energy level
2
How much does one principal energy level go up by
1 Each Time
How many protons are in the nucleus of a magnesium atom?
12 (atomic number)
Write the electron configuration for Magnesium in the ground state
1s22s22p63s2
How does an atom of magnesium become Mg+2 ion
Loses 2 electrons
What noble gas has the same electron configuration as Mg+2
Neon
Name three elements that could be X
Oxygen, Sulfur, Selenium
The pair of elements with the most similar chemical properties are
The ones right on top and below each other are the closest
Which atom has the largest atomic radius?
The one closest to the lower left of the table
As the elements of Group 16 are considered from top to bottom on the Periodic Table , the atomic radii
Increase and the ionization energies decrease
The S-2 ions differ from the S0 atom in that the S-2 ion has a
Larger radius and more electrons
What type of energy represents in the equation Na+energy—-> Na+ + e-
Ionization energy
Define Ionization Energy
The ionization energy is the exact quantity of energy that it takes to remove the outermost electron from the atom.
In which reaction is the first ionization energy greatest
The one closest to the top right
Which element in period 2 has the greatest tendency to gain electrons (electronegativity)
One closest to upper right
Period is
Horizontal
Group is
Vertical
What group in the periodic table contains the elements to the alkaline earth family
2
When oxygen combines with any alkaline metal, M, the formula of the compound produced usually is
MO2
Which Element is a halogen
Group 7A
Ozone is an allotropic form of the element
Oxygen
Who was credited with creating the first periodic table that organized the elements according to atomic mass
Dmitri Mendeleev
A diagram with two same size circles one white, one black labeled X and Z yield one smaller circle white with X+ plus one larger circle black Z- Which particle (X or Z) most likely represents a metal atom?
X is metal because it becomes a smaller positive ion
A diagram with two same size circles one white, one black labeled X and Z yield one smaller circle white with X+ plus one larger circle black Z- which most likely represents a nonmetal atom?
Z because it become a larger negative ion
Which metal is the most reactive metal?
The closest to the bottom left is
Which is the most reactive non metal
The closest to top right
Which element has properties of both metals and non metals
Any metalloid (on the line)
Which two elements would most likely combine to form an ionic compound
The metal and non metal farthest from each other
Which element can lose electrons from its two outermost energy level
Any transition metal (One of the metals in the middle)
Which element exists as a monoatomic gas at STP
Any of the Noble Gases
Which element exists as a diatomic gas at STP
C,N,O,F,Cl,Br,I,H
Define a transition metal
Is more than one color and can take electrons from more than 1 energy level, can have more than one binary compound
Given the reaction: H2 + Cl2 —-> 2HCl
Which of the following statements best describes the energy change as bonds are formed and broken in this reaction
The forming of the H—Cl bind releases energy
Which formula represent an Ionic Compound
Any one with a metal and non metal
If the last element is an even coefficiant what is it
Non polar
If the last element is an odd coefficient what is it?
Polar
Review Questions number 89-93 + Compounds in back of packet
SKIP
Which combination of atoms can form a polar covalent bond?
H and Br
Which two compounds contain only polar molecules
2 elements with odd coefficients
In a nonpolar covalent bond, electrons are
Shared equally by two atoms
Which of the following statements best explain why a CH4 molecule is non polar
CH4 has a symmetrical charge distribution
The table below shows four compounds and the boiling point of each: Which type of molecular attraction accounts for the high boiling points Compound | Boiling Point H2O 100 C H2S -60.7 C H2Se -41.5 C H2Te -2.2 C
Hydrogen Bonding
The table below shows four compounds and the boiling point of each: Compared the boiling points of H2S, the boiling point of H2O is relatively high. Which type of bonding causes this different? Compound | Boiling Point H2O 100 C H2S -60.7 C H2Se -41.5 C H2Te -2.2 C
Hydrogen
What is the Gram Formula Mass of Al2(SO4)3
342g
What is the total number of moles contained in 115 grams of C2H5OH
2.50
A sample of nitrogen containing 3.0x10^23 molecules has the same number of molecules as a sample of
.50 (Half) Moles of Ne
What is the mass of 3.0x10^23 atoms of Neon
10 grams
Which sample of O2 contains a total of 3.01x10^23 molecules at STP
16.0 grams
The percent bny mass of oxygen in H2C2O4
64
____ x 100
90
The empirical (reduced) formula of the compound whose molecular formula is P4O10
P2O5
What is an empirical formula?
The most reduced formula
A 10 gram sample of a hydrate was heated until all the water of hydration was driven off. The mass of anhydrous product remaining was 8.00 grams. What is the percent of water in the hydrate?
Second number/First Number= T
T - 100 = Answer
20%
What is the empirical formula of a compound consisting of 29.6% Oxygen and 70.4% Fluorine by mass
Divide percents by the elements mass then divide the smalled number by all other numbers should equal .0 or .9 if not multiply by (5 3 5 2 5 3 5)
A compound contains .5 moles of sodium, .5 moles of Nitrogen, and 1 mole of hydrogen. The empirical formula of the compound is
NaNH2
A 16 gram sample of a compound containing only copper and sulfur is decomposed to produce 12.8 grams of copper and 3.2 grams of sulfur. What is the empirical formula of the compounds
Cu2S
NaOH + HCl —> NaCl + H2O
What is the total number of grams of H2O produced when 116 grams of the product, NaCl is formed?
36g
N2(g) + 3H2(g) —> 2NH3(g)
What is the total number of liters of NH3 Formed when 20 liters of N2 react completely
40L
C8H16 + 12O2 —> 8CO2 + 8H2O
How many moles of H2O are produced when 11.2 liters of C8H16 gas measure at STP react completely
4.00
In the reaction N2 + 3H2 —> 2NH3 how many grams of H2 are needed to produce exactly 1 moles of Ammonia
3 gram
4Al(s) + 3O2(g) —> 2Al2O3(s)
Calculate the gram molecular mass of Al2O3
102 grams
4Al(s) + 3O2(g) —> 2Al2O3(s)
How many moles of Al are needed for the production of 3.00 moles of Al2O3
6 moles
4Al(s) + 3O2(g) —> 2Al2O3(s)
Calculate the mass in grams of 3.00 moles of Al2O3
306 grams
What is the percent by mass of water present in 1.0 mole of CaSO4 o 2H2O
36
____ = 21%
172
What is the total number of grams of KCl (formula mass = 74.6) in 1 liter of .200 moles solution
14.9 grams
What is the molarity of a solution of KNO3 (molecular mass = 101) that contains 404 grams of KNO3 in 2.00 liters of solution
2.00 M
What is the total number of solute contained in .5 liters of 3.0 M HCl
1.5
How many grams of ammonium chloride (gram formula mass = 53.5 g) are contained in .500L of 2.00 liters of solution
53.5 grams
How many grams of KI are dissolved in 250 grams of a 20% solution
50 grams
A solution will boil at the highest temperature when it contains 1 mole of nonvolatile solute dissolved in
250 grams of solvent
When 2.00 moles of sugar (C6H12O6) are dissolved in 1.00 grams of water the boiling point of the resulting solution is closest to
101 C
Which solute, when qdded to 1000 grams of water, will produce a solution with the highest boiling point
58 grams of NaCl
The heat of reaction (Delta H) is equal to the
Heat content of the products minus the heat content of the reactants
Review 126-130 In Packet
SKIP
A(g) + B(g) –> C(g)
As the concentration of A(g) increases, the frequency of collisions of A(g) with B(g)
Increases
In a gaseous system, temperature remaining constant, an increase in pressure will
Increase reaction rate
In an gaseous system, temperature remaining constant, a decrease in pressure will
Decrease reaction rate
As the surface area of the Zn(s) used in the reaction Zn(s) + 2HCl(aq) —> ZnCl2(aq) + H2(g) is increased, the rate of the reaction will
Increase
The addition of a catalyst to a reaction will cause a change in the
Activation Energy
CAT (Catalyst)—>
ACT (Activation energy)
Delta H
- = Exo \+ = Endo
Delta S
- = Less Disorder \+ = More Disorder
Delta G
- = Spontaneous \+ = Non Spontaneous
The pair of changes would indicate that a reaction is endothermic but occurs spontaneously
A positive Delta H and a Negative Delta G
A chemical reaction will always occur spontaneously if the reaction has
Negative Delta G
BaSO4(s) = Ba+2(aq) + SO4-2(aq)
As the concentration of the SO4-2(aq) ions increases, at a constant temperature, the concentration of Cl- Ions
Decrease
CH3COOH(aq) + H2O(l) = H3O+(aq) + CH3COO-(aq)
The addition of what ion will cause the decrease in the concentration of CH3COO-(aq)
H3O-
N2(g) + 3H2(g) = 2NH3(g) + heat
Which change favors the formation of ammonia?
Increasing the concentration of N2(g)
2SO2(g) + O2(g) = 2SO3(g)
As the pressure is increased at the constant temperature, the number of moles of SO3(g) produced will
Increase
2A(g) + B(g) + 10 kcal = C(g)
Which condition would yield the most product
High temperature and high pressure
What is the equilibrium equation for the reaction 3A(g) + B(g) = 2C
[A]3[B]
Which of the following is the correct equilibrium expression for
4NH3(g) + 7O2(g) = 4NO2(g) + 6H2O(g)
[O2]7[NH3]4
A + B =AB
The greatest amount of AB would be produced if the equilibrium constant of the reaction is eqaul to
1.0x10^5
AgI(s) = Ag+(aq) + I-(aq)
Which of the following is the correct solubility product constant expression for the reaction
Ksp = [Ag+][I-]
C(s) + CO2(g) + heat —-> 2CO2(g)
Which stress on the system would favor production of CO(g)
An increase Pressure
A2(g) + 3B2(g) = 2AB3(g) + heat
State two stresses that could be applied to this system that would cause this equilibrium to shift to the right. Explain why each stress would cause a shift in the equilibrium
Temperature and Pressure because those can change the state of the substance
What is the pH of a solution that has an OH- ion concentration of 1x10^-9 mole per liter (Kw = 1 x 10^-14)
5
What is the pH of a .00001 molar HCl solution
5
If the OH- equals 1 x 10-10 at 298 k for a given soltuion, the H+ of the solution equals
1 x 10-4
What s the H+ ion concentration of an aqueous solution that has a pH of 11
1 x 10-11 mol/L
The H3O+ ion concentration of a solution is 1x10-5 mole per liter. This solution is
Acidic and has a pH of 5
Which equation represents a neutralization reaction
Any equation with the product of NaCl + H2O
What is a neutralization reaction
A reaction resulting in NaCl + H2O
If 100 milliliters of .75 M HCl is required to exactly neutralize 50 milliliters of KOH, what is the concentration of the base?
1.5 M
If you see exactly neutralized in an equation what do you do?
Multiply the first two numbers you see and then divide it by the last
In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:
Write a balance equation for HNO3 and LiOH
HNO3 + LiOH —> H2O + LiNO3
In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:If 50 milliliters of .50 M LiOH is required to exactly neutralize 100 milliliters of an HNO3 solution, what is the molarity of the HNO3 solution?
.25 M
In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:What indicator was used in the titration
Moles
What color does Phenothaline turn in Acid
Colorless
What color does Phenothaline turn in Base
Pink
What color does Litmus turn in Acid
Red
What color does Litmus turn in Base
Blue
Arrhenius Acid
Gives H+
Arrhenius Base
Gives OH-
Bronsted Lowry Acid
Gives H+ (Proton)
Bronsted Lowry Base
Accepts H+ )Proton
Lewis Acid
e- pair Acceptor
Lewis Base
e- pair Donor
How do you know what the Bronsted Lowry Bases are
Compare the two similar elements on each side and the one with the less H’s is the base
In a redox reaction there is conservation of
Both mass and charge (everything)
Review 161 and 162 In Packet
SKIP
How do you know which substance is being oxidized?
Pick the first element in the equation or the metal
How do you know a reaction is redox
Look for a single element and not compounds
If there is no metal in the equation how do you know what was oxidized?
Look for an increase in ions
0
e-
-1
Beta
4
He
2
Alpha
0
e-
1
Positron
0
V
0
Gamma
1
Beta
2
Gamma
3
Positron and Alpha
To solve a Nuclear Problem what do you do?
Equal Everything
What is the equation for Decay
TGB
——- = Decay
HL
At the end of 12 days 1/4 of an original sample of a radioactive element remains. What is the half life of the element
6 Days
An Original Sample of a radioisotope has a mass of 10 grams. After 2 days, 5 grams of the radioisotope remains unchanged. What is the half life of the radioisotope
2 Days
In 6.20 Hours a 100 gram sample of Ag-112 decays to 25 grams. What is the half life of Ag-112
3.10 Hours
The half life of carbon-14 is 5730 years. What fraction of a 1 gram sample of carbon-14 would remain after 17190 years?
1/8
Which quantity expresses the sum of the values below to the proper degree of precision 2.1 33.566 \+12.22 --------------
47.9g
Using the rules for sig fig, the sum of .027g and .0023 grams should be expressed
.029
What is the product of (2.324 cm x 1.11 cm) expressed to the correct sig fig
2.58 cm2
During a titration, a student used 50 milliliters of .1 M acid. How many moles of acid, expressed to proper significance, were used?
.005
What is the number 215 expressed in proper scientific notation with the correct number of sig fig,
2.150 x 102
A student investigated the physical and chemical properties of a sample of an unknown gas ans then identified the gas. Which of the following statements represents a conclusion rather than an experimental observation
The gas is carbon dioxide
What is the number 2.1 x 10^3 expressed in conventional form with the proper number of sig fig
2100
The solid block shows below has a mass of 146 and a length and width of 3 and a height of 6 what is the density
2.7
The process of filtration is preformed in the laboratory to
Separate insoluble substances in an aqueous mixture
Linear CH4
CO2
Tetrahedral
CH4
Bent
H2O
Trigonal Pyramidal
NH3
NP
LDF
P
DD
Equation for moles
C
Equation for Grams
C (mass)
Equation for Liters
C (22.4)
Equation for Molecules
C (6.02x10^23)
When in Doubt
PV=nRT
What is another equation for Grams
LP
What is another equation for Density
P
