Chemistry I Final
The oxidation numbers of P, S and Cl in H2PO2+, H2S and KClO4 are respectively
+1, +2, +7
What is the charge on the thallium ion in TI2O3?
+3
A typical double bond
- imparts rigidity to a molecule - consists of one sigma bond and one pie bond - consist of 2 shared electron pairs - is stronger and shorter than a single bond
The flow of energy (q) and work (w) in an endothermic process
- q and w coming into the system - q coming in and w going out to surrounds - q coming in
Consider the following two reactions: A-->2B heat of reaction = 456.7 kJ/mol A-->C heat of reaction = -22.1 kJ/mol Determine the enthalpy change for the process 2B-->C
-478.8 kJ/mol 2B-->A -456.7 kJ/mol A-->C -22.1 kJ/mol add together
Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which Iron(s) is/are spectator ions in the reaction?
. Na+ and I-, since BaSO4 is the precipitate all other ions are considered spectators
a certain liquid has a density of 2.67 g/cm3. 30.4 mL of the liquid would have a mass of________ kg
0.0814
If there are 0.505g of NaCl (58.44 g/mol) left in a beaker that originally contained 75.0 mL of saltwater, what must have been the concentration of the original solution?
0.115 M
A mixture of Xe, Kr, and Ar has a total pressure of 6.70 atm. What is the mole fraction of Kr if the partial pressures of Xe and Ar are 1.60 atm and 2.80 at, respectively
0.343 P of Kr = 1.6 +2.3 = 4.4 Pi = xPT x = 2.3 atm/6.7 = 0.343
A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10L to 15L. the final pressure is ______ moles, temp and R constant
0.67 atm P1V1=P2V2
How many molecules of CH4 are in 48.2 g of this compound?
1.81 x 10^24 48.2g/16.042g x 6.022x10^23molecules/mol
The reaction of molybdenum (V) Chloride with sodium slide is give by the unbalanced chemical equation MoCl5(s) + Na2S(s) ---> MoS2(s) + NaCl(s). How many moles of S (s) are formed for every one mole of MoCl5 reacting according to the balanced version of this equation?
1/2
What volume (mL) of a concentrated solution of magnesium chloride (9.00 M) must be diluted to 250. mL to make 2.75 M solution of magnesium chloride?
107 mL
Orbitals with l=5 are called h orbitals, How many electrons with ms= +1/2 could occupy the 6h orbitals? (sec 6.75,.77)
11
The formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is
123.11
The central iodine atom in IF5 has _______ unbounded electron pairs and ______ bonded electron pairs in its valence shell
1;5
Then the oxidation-reduction reaction shown is balanced using the smallest whole-number coefficients, how many electrons are transferred for each atom of copper that reacts? Ag+(aq) + Cu(s) ---> Ag(s) + Cu2+(aq)
2
orbitals with l=5 are called h orbitals. How many electrons could occupy the 6h orbitals?
22
The mass % of H in methane (CH4) is ______
25.13 4(1.008g/mol)/16.04g/mol X100
The Mind process produces pure nickel metal via the thermal decomposition of nickel tetracarbon Ni(CO)4(l) ---> Ni(s) + 4CO(g) What volume (L) of CO is formed from the complete decomposition of 444g of Ni(CO)4 at 0.9895 atm and 22.0 deg C
255 L 444g/170.73g * 4mol/1mol= 10.40 mol 22+273 = 295 K PV=nRT V= nRT/P = 254.5
The central iodine atom in the ICl4- ion has _______nonbonded electron pairs and _________ bonded electron pairs in its valence shell
2;4
The wavelength of photon that has an energy of 5.25 x 10^-19 is ________ m
3.79 x 10^-7 E= hc/wavelength wavelength= hc/E 6.626x10^-34 x 3x10^8 both divided by 5.25 x 10^-19
The element X has two naturally occurring isotopes. The masses (amu) and % abundance of the iso are given in that table below. The average atoms mass of the element is ______ amu.
33.20 31.13(0.3516) + 34.30(0.6484)
The number of electrons in a 90Sr2+ iron is
36
What is the total ionic equation for the reaction of hydrochloric acid with solid chromium (III) hydroxide? None of products are solids.
3H+(aq) + 3Cl-(aq) +Cr(OH)3 (s) ----> Cr3+(aq) + 3Cl-(aq) + 3H20(l)
An electron in a Bohr hydrogen atoms has an energy of -1.362 x 10^-19 J. The value of n for this electron is _______
4 En = -2.18 x 10^-18 (1/n^2) n^2= -2.18 x 10^-18 J/ 1.362 x 10^-15 J n= square root of 16.005 = 4
You synthesize a new radon compound in which the central atom is bonded to 4 fluorine atoms and 2 oxygen atoms. How many valence electrons does its Lewis structure contain?
48
The wavelength of light emitted from a traffic light having a frequency of 5.75 x 10^14 Hz is
522 nm C=wavelength times frequency meters to nanometers
There are _______ electrons, ________ protons, and _________ neutrons in an atom of 132 54 Xe
54, 54, 78
Mixing 20 mL of a solution with 100mL off water will reduce the concentration by a factor of
6 20+100mL =120mL -->V2
The number of neutrons in an atoms of 131 I is
78
Which of the following correctly represents the third ionization of aluminum
Al 2+(g) ---> Al3+(g) + e-
Which of the following ionic compound is insoluble in water? a. NaOh b. BaSO4 c. ZnCl2 d. KBr e. Ca(NO3)2
B. BaSO4
The standard enthalpy of formation of CO2(g) at 25 deg C is equal to the enthalpy of reaction for...
C(s,gr) +O2(g) ---> CO2(g)
Which equation correctly represents the electron affinity of calcium?
Ca (g) + e- ---> Ca-(g)
_______ is isoelectronic with argon and ________ is isoelectronic with neon
Cl- and F-
Of the following, Heat of Reactions is NOT zero for... a. N2 (g) b. O2 (g) c. Cl2 (g) d. C (graphite) e. F2 (s)
E. F2 (standard state is gas phase)
The effective nuclear charge (Zeff) felt by the outermost electrons is the greatest for which (sec 7.13,18) a. F b. C c. B d. Be e. Li
F
(Ar)4s2 3d3 4p3 is an excited state for what neutral atom
Fe
the formula iron (II) phosphate is
Fe3(PO4)2
Hund's Rule
Have to fill with up arrows across boxes before you can do down arrows
What is the net ionic equation for the reaction between sodium chloride and mercury (I) nitrate?
Hg2 2+(aq) + 2Cl-(aq) --> Hg2Cl2(s)
the first eight successive ionizations energies (IE1, IE2...) for Al are 578, 1817, 2745, 11,577, 14,842, 18,379, 23,326, and 27,465 kJ/mol. What is the probable explanation for the large jump in energy observed between IE3 and IE4?
IE4 reflects that inner shell electrons with a lower n value are starting to be removed.
Hess's Law
If a reaction is carried out in a series of steps, the deltaH for the reaction will equal the samba of the enthalpy changes for the individual steps
The first law of thermodynamics
If the surrounding gain energy from the the system, then the system must lose an equal amount of energy
Order for decreasing atomic radius Ge, As, Ca, Kr, K
K > Ca > Ge > As >Kr
For which of these atoms is there an especially large difference between its second ionization energy and its third ionization energy? (Sec 7.91) a. Na b. Mg c. Al d. Si e. P
Mg
Identify the base in the following acid-base reaction. NH3(aq) + H2O(l) ---> NH4+(aq) + OH-(aq)
NH3
Which element IS in its standard state at 25 deg C and 1 atm?
O2(g)
Three mono sulfur fluorides are observed: SF2, SF4, and SF6. Of these ________ is/are polar
SF2 and SF4 only
When an electron jumps from the 4d to a 3p orbital, a _______ is _________
a photon is emitted
The molecular geometry consists of
a single bond and multiple bond only not nonbonding pair of electrons
Which information is not shown in Lewis structures of molecules? a. how atoms are arranged in space? b. the number of bonding pairs of electrons between atoms c. nonbonding electrons on atoms d. the order in which atoms are linked e. the number of valence electrons in the molecule
a.
Which of the following regarding Lewis dot symbols, Lewis Structures, and the octet rule is FALSE? a. a molecule cannot have an odd number of valence electrons b. there are some atoms that do not obey the octet rule c. the number of unpaired dots shows the typical bonding capacity of an atom d. Lewis dot structures can be written for atoms and for ions e. atoms tend to gain, lose, or share electrons in order to attain eight valence electrons.
a.
Which one is a redox reaction? a. 2Na(g) + Cl2(g) ---> 2NaCl(s) b. Ba2+(aq) + SO4 2-(aq) ---> BaSO4(s) c. K2Cr2O7(aq) + 2KOH(aq) ---> 2K2CrO4(aq) +H20(l) d. Na2CO3(s) + 2HCl(aq) ---> 2NaCl(aq) + CO2(g) +H20(l) e. H2O(l) ---> H+(aq) + OH-(aq)
a.
which of the following will lead to an decrease in the kinetic energies of electrons emitted from a metal surface when light is shining on the surface? a. increase in light's wavelength b. increase in light intensity c. decrease in wavelength d. decrease in light frequency d. decrease in intensity
a.
An electron cannot have the quantum numbers n=, l=, ml= a. 3,2,3 b. 1,0,0 c. 3,2,1 d. 3,2,-2 e. 6,1,0
a. 3,2,3
Which of the following species is NOT isoelectronic to the others? a. Ca2+ b. Kr c. As3- d. Br- e. Y3+
a. Ca2+
Which of the following bonds is the most polar? a. Mg-O b. Si-O c. O-O d. C-O e. N-O
a. Mg-O
One mole of _______ contains the smallest number of atoms a. NaCl B. S8 c. C10H8 d. Na3PO4 e. Al2(SO4)3
a. NaCl
What is not an example of a chemical reaction? a. condensation of water vapor b. formation of polyethylene from ethylene c. dissolution of a penny in nitric acid d. a burning candle e. a homogeneous mixture
a. condensation of water vapor
Which of the following statements is false? a. as the wavelength of a photon decreases, energy increases b. the speed of a photon decreases as its wavelength decreases c. light can be viewed as packets of energy d. as the frequency of a photon decreases, its energy decreases e. a high-energy photon has a wavelength shorter than that of a low-energy photon
b.
Which of the following statements is false? a. as wavelength of a photon decreases, energy increases b. the speed of a photon decreases as its wavelength decreases c. light can be viewed as packets of energy d. as the frequency of a photon decreases, its energy decreases e. a high-energy photon has a wavelength shorter than that of a low-energy photon
b.
Which solution has the largest number of moles of chloride ions? a. 4 mL o 1.000 M NaCl b. 7.50 mL of 0.500 FeCl3 c. 25 mL of .400 M Kcl d. 10.0 mL of .500 M BaCl e. 30 mL of .100 M CaCl2
b.
Which statement about a balanced chemical equation is alway correct? a. the total number of moles of the products equals the total number of moles of the reactants b. the number of atoms of each kind is the same for products and reactants c. the sum o the stoichiometric coefficients for the products equals the sum for the reactants d. the same of the masses of all gaseous products equals the sum of the masses of the gaseous reactants e. the sum of the masses of solid products equals the same of the masses of solid reactants.
b.
which of the following sets of quantum numbers is NOT allowed? a. n=4, l=1, ml=-1, ms=-1/2 a. n=2, l=1, ml=0, ms=-1 a. n=6, l=4, ml=-1, ms=-1/2 a. n=3, l=2, ml=2, ms=+1/2 a. n=7, l=3, ml=-2, ms=+1/2
b.
which of the following sets of quantum numbers is allowed? a. n=2, l=1, ml=-2, ms=-1/2 a. n=7, l=3, ml=0, ms=+1/2 a. n=6, l=-1, ml=-1, ms=-1/2 a. n=1, l=2, ml=0, ms=+1/2 a. n=2, l=1, ml=0, ms=-1
b.
Which electron transitions, in a multi-electron atom, is associated with the absorption of light? a. 3d ---> 4s b. 7s ---> 5f c. 5f ---> 6s d. 3p ---> 3s e. 5f ---->5d
b. 7s ---> 5f
Of the following species ________ has the larges radius a. Ar b. Br- c. Kr d. Sr 2+ e. Rb +
b. Br-
Arrange the interactions between pairs of electrons in order of increasing strength bonding and lone pair
bonding-bonding < lone pair-bonding pari < lone pair-lone-pair
For an endothermic process
both q and w MUST be positive
Which of the following is INCORRECTt? a. ionic bonding results from the transfer of electrons from one atom to another b. dipole moments result from the unequal distribution of electrons in a molecule c. linear molecules cannot have a dips moment d. a molecule with very polar bonds can be nonpolar e. the electron density in a polar bond is found nearer to the more electronegative element
c.
Which solution has the same number of moles of NaOh as 50.00mL of 0.100M solution of NaOH? a. 30 mL of 0.145M NaOH b. 20 mL of 0.200M c.. 100. mL of 0.0500M d. 25.00 mL of 0.175M e. 50 mL of 0.125 M
c.
Which is associated with an emission of light? a. 4s --> 3d b. 6s---5f c. 4f---> 6s d. 3s--> 3p e. 5d---> 5f
c. 4f ----> 6s
Which is there an especially large difference between its third ionization energy and its fourth? a. Na b. Mg c. Al d. Si e. P
c. Al
Of the ions below, only _________ has noble gas electron configuration a. S3- b. K- c. Cl- d. O2+ e. I+
c. Cl-
indicate which of the following is NOT and element in its standard state at 25 degrees C and 1 atm a. O2(g) b. H2(g) c. N(g) d. Ne(g) e. C(s, gr)
c. N(g)
Which of the following bonds is the least polar? a. mg-O b. Si-O c. O-O d. C-O e. N-O
c. O-O
The de Broglie wavelength of a _______ will have the shortest wavelength when traveling at 30 cm/s a. uranium atom b. car c. planet d. hydrogen atom e. marble
c. planet (largest mass) as mass increases, wavelength increases
You hold a 50g sphere of copper (s=0.4 J/(g degC) in one hand and a 25g sphere of aluminum (s=0.9 J/(g degC) in other hand. If both absorb energy at the same rate, which will come to your body temp first and why?
copper, because the heat capacity is smaller
Atoms with similar electronegativity values would be expected to form __________ bonds
covalent
Which of the following is in the correct order of decreasing radii from largest to smallest. a. Li+, Na+, K+ b. Na+, Cs+, I- c. F-, Mg+, Cs d. As3-, Br-, K+ e. Be, Ba+, )2-
d.
Which statement regarding the Bohr model of the atom is NOT correct. a. changes in the energy of the atom involve the electron transitioning between allowed orbits b. the atom has discrete energy levels described by quantum number n c. the electron does not radiate energy and spiral into the nucleus if it is an allowed orbit d. the atom has zero energy when in its ground state e. the energy of an orbit is inversely proportional to n2
d.
Which of the following will have the weakest ionic bond? a. MgO b. CaO c. SrO d. BaO e. BeO
d. BaO
According to kinetic-molecular theory, in which of the following gases will the root-mean-square speed of the molecules be highest at 200 deg C a. Cl2 b. SF6 c. HCl d. H2O e. none
d. H2O Urms= square root of 3RT/m m decreases as Urms increases
If you had equal masses of each of the following substances, which would occupy the greatest volume? a. ice (d=0.917) b. water (d=0.997) c. beeswax (d=0.960) d. cocoa butter (d=0.910) e. aluminum (d=2.70)
d. cocoa butter
Which of the following effects will make PV/nRT less than 1 for a real gas? a. gas molecule are large enough to occupy a substantial amount of space b. a large number of molecules have speeds greater than the average speed c. the gas molecules have a very low molar mass d. the gas molecules attract one another e. none of these explain this behavior
d. gas molecules attract one another
Which quantum number determines the energy of an electron in a hydrogen atom? A.E b. l c. Ml d. n e. n and l
d. n
An unknown gas held in a 25.0mL flask at 45 degree F exerts a pressure of 25 motor. By using this info with the ideal gas law, it is possible to determine... a. identify the gas b. the mass of the gas in the container c. the molecular geometry d. the number of molecules e. nothing more about the gas
d. the number of molecules of the gas in the container
An element is the upper right corner of the PT is
definitely a non-metal
Name the compound Cl2O5
dichlorine pentoxide
The first ionization energies (IE1) of phosphorus and of sulfur are 1012 and 1000 kJ/mol. Why is IE1 for S lower than that of P when the usual trend is or IE to increase across a now? a. an electron from phosphorus must be removed from a lower-energy subshell b. Zeff decreases from left to right on the periodic table c. sulfur is smaller than phosphorus d. more electrons in a sub shell decreases orbital energy e. removing an electron from sulfur produces a half-filled sub shell and reduces electron-electron repulsions
e.
Which ionic compound is expected to be insoluble in water? a. (NH4)2S b. FeBr2 c. Na2SO4 d. Pb(NO3)2 e. Cu(OH)2
e.
Which of the following is a statement of the first law of thermodynamics? a. a negative deltaH corresponds to an exothermic process b. deltaE = Efinal - Einitial c. Ek = 1/2mv^2 d. 1 cal= 4.184 J exactly e. energy lost by the system must be gained by the surroundings
e.
Which of the following is not a quantum number? a. n b. l c. ml d. ms e. Z
e.
Which of the following statements is INCORRECT a. atoms of one element are different from the atoms of all other elements b. the size of the atomic nucleus of is much smaller than the size of the atom c. elements are composed of atoms d. in a compound, the ratio of the number of atoms of any two of the elements present can be a fraction e. atoms can be created during a chemical reaction
e.
Which of the following statements regarding kinetic molecular theory is FALSE> a. energy can be transferred but not lost as gas particles collide with each other and the container walls b. the gas particles are in constant, rapid, random motion c. the gas particles are assumed to occupy negligible volume d. the average kinetic energy of the gas particles is directly proportional to the absolute temperature e. at a given temperature, the gas particles have the same velocity
e.
Which regarding state and non-state (path) functions is FALSE? a. the value of a path function depends on how change occurs b. the value of a state function does not depend on history of the system c. heat and work describe the manner in which a system attains its current energy d. the internal energy of a system can be the result of many combinations of work and heat e. the value of a state function depends on the nature in which it was attained.
e.
Which of the following will have the strongest ionic bond? a. MgO b. CaO c. SrO d. BaO e. BeO
e. BeO
Which of the following bonds is the least polar? a. H-N b. H-Cl c. H-F d. H-O e. H-B
e. H-B
the internal energy of a system is always increased by a. having the system do work on the surroundings b. a volume compression c. withdrawing heat from the system d. adding heat to the system and having the system do work on the surroundings e. adding heat to the system
e. adding heat to the system deltaU= q+w
Which one of the following ions has the same charge as the hydroxide ion? a. sulfide b. ammonium c. sulfate d. carbonate e. nitrate
e. nitrate
if matter is uniform through and cannot be separated into other substances by physical means, it is
either an element or a compound
The basis of the VSEPR model of molecular bonding is
electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions
the capacity to do work is a definition of
energy
Heat is best defined as
energy transferred as the result of a temperature difference OR the total energy that a substance has
Puli Exclusion Principle
have to have an up and down arrow, can't have 2 up or 2 down in the same box
which of the following will lead to an increase in the kinetic energies of electrons emitted from a metal surface when light is shining on the surface? a. increase in light's wavelength b. increase in light intensity c. decrease in wavelength d. decrease in light frequency d. decrease in intensity
increase in the light's intensity
in ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii ________
increases, increase, decresae
Statements regarding bond strength and length. Bond strength ________ as the distance between 2 atoms ________ the length of a bond is generally ___________ proportional to its ___________
increases; decreases inversely; strength
The effective nuclear charge of an atom is primarily affected by
inner electrons or nuclear charge
Atoms with different electronegativities would form _______ bonds
ionic
Oxidation is the ________ of electrons and reduction is the _________
loss; gain
When several metals are of equal masses initially at room temperature absorb equal amounts of heat, the metal with the ___________ specific heat will have the highest final temperature.
lowest
According to the Heinsenberg Uncertainty Principle, it is impossible to know precisely both the position and the _______ of an electron.
momentum
The quantum number that labels an electron but not an orbital is
ms
all atoms o a given element have the same
number of protons
Which electron jumps from the 3p to a 4d orbital? a ______ is ________
photon; absorbed
isotopes have the same number of ______
protons
orbitals within a given sub shell have the _______ principal and ________ quantum numbers
same; angular
A covalent bond is the
sharing of electrons between atoms
In liquids, the attractive intermolecular forces are
strong enough to hold molecules relatively close together but NOT strong enough to keep molecules from moving past each other
Which element forms an ionic compound with Na2X? a. magnesium b. carbon c. sulfur d. iodine e. phosphorus
sulfur
the electron domain and molecular geometry of BrO2- is
tetrahedral; bent 2 bonded, 2 non-bonded
principle quantum number n gives info about
the energy and size of an orbital
magnetic quantum number ml gives info about
the spatial orientation of an orbital
In a VALID Lewis Dot Structure for a neutral molecule...
the sum of the formal charges on the atom always equals zero
Electron affinity is the energy change that occurs
when a gas-phase atom or ion in tis ground state gains an electron
