Sem. 1 Final Exam Flashcard

Relatively slow rates of chemical reation are associated with which of the following?
Strong bonds in reactant molecules
Standard enthalpy change for Na2O + H2O= 2NaOH
-150 kJ
Planar configuration
BCl3
N2 + 3H3= 2NH3
change in G, H, and S are negative
change in H for I2 + 3Cl2= 2ICl3
-390 kJ
two unshared pairs of electrons on central atom
H2S
Molecule with only one double bond
C2H4
Molecule with the largest dipole moment
H2O
trigonal pyramidal geometry
PH3
change in H for 3C2H2= C6H6
-607 kJ
most ionic compound
CaCl2
NH4SCN
change in G negative, change in H and S positive
most positive oxidation number
SO2
compound that shows resonance
SO2
PF5 does not have
d2sp3 hybridization
decrease in entropy
formation of a crystalline solid from a supersaturated solution
electrons shared by hydrogen and oxygen
spend more time around oxygen
decreasing bond polarity
HF HCl HBr HI HAt
most ionic elements
CsF
number of structures for NO3-
3
molecule that violates octet rule
SF4
number of electrons on FCl3
6
bond energy for CH4 + 4F2= CF4 + 4HF
-1924 kJ
shape of AX5 with one nonbonding pair of electrons
square pyramidal
shape of AX3 with two lone pairs of electrons
T-shaped
shapes of NH3 and BF3
trigonal pyramidal and trigonal planar
molecule that is nonpolar
CF4
polar molecule
PCl4F
square planar hybridization
sp3d2
PCl5 hybridization
sp3d
negative change in S
compressing one mole of Ne at constant temperature from .5 to 1.5 atm
first law of thermodynamics
energy cannot be created or destroyed but must be conserved
second law of thermodynamics
entropy of the universe is increasing
specific heat capacity
amount of energy required to raise one gram of a substance one degree Celsius
heat released when 9.25 moles of Fe is reacted with oxygen
-3820 kJ
change in H for P4O10 + 6PCl5 =10Cl3PO
-610 kJ
formula for P2O5
diphosphorus pentoxide
kinetic molecular theory does not say
gas particles move at speeds close to the speed of light
Cu65 isotope in nature
25%
Average atomic or molecular speed closest to N2 molecules at 0 C and 1 Atm
CO
greatest density at 0 C and 1 Atm
Xe
Values that decrease when ideal gas is cooled by 25 degrees
average distance between molecules and average speed of molecules
percent of CaCO3 by mass in limestone
35%
safest and most effective way to treat an acid splash on skin
flush affected area with water and then with a dilute NaHCO3
moles of HI needed to produce 2.5 moles of I2
5
why does water boil at a lower temperature on a mountain
equilibrium water vapor pressure equal the atmospheric pressure at a lower temperature
partial pressures of gasses
He less than Ne less than Ar
gas that deviates most form ideal behavior
SO2
the a coefficient in van der Waals equation
forces of attraction between molecules
how many protons, neutrons, and electrons are in Sr-90
38, 52, 38
Quantum numbers of ground-state gallium
4,1,1,1/2
pauli exclusion principle
indicates that an atomic orbital can hold no more than two electrons
dissolves in water to form a colorless solution
ZnCl2
not true about halogens
iodine liberates free bromine from a solution of bromide ion
barium sulfate is least soluble in a .01 molar solution of what
Al2(SO4)3
what color is the flame when a solution of sodium chloride is vaporized in a flame
yellow
use of a visible-light spectrophotometer
determining the concentration of a solution of Cu(NO3)2
based on ionization energies in chart, element X is what
Al
what happens to atomic radius as atomic number increases from 11-17
decreases
Rutherford’s gold atom experiment
neutrons are at the center of an atom
yellow precipitate forms when NaI is added to what
Pb
not soluble in water but soluble in dilute hydrochloric acid
Mg(OH)2
what will separate Pb from other ions
dilute HCl solution
contains exactly two unpaired electrons
S
contains only one electron in the highest occupied energy sublevel
Ga
purple in aqueous solution
KMnO4
white and soluble in water
KCl
isoelectronic elements
Mg, Ca, Sr
greatest percentage of which compound can be recovered by cooling a saturated solution of that compound from 90 degrees C to 30 C
KNO3
which property decreases across the periodic table form sodium to chlorine
atomic radius
why is there a different nuclear charge on Na and Ne
Na has a higher neutron-to-proton ratio than Ne
sodium chloride is least soluble in what
CCl4
all halogens are
diatomic
least soluble in water
BaCO3
with chart, which ions could be present in solution at a concentration of .1 M
Na
what pure white crystalline solid dissolves in water to yeild a base and liberate gas when acid is added to it
K2CO3
mixture is made by adding AgNO3 to Na2CrO4, what does it look like
yellow before, red precipitate
precipitate made when AgNO3 is added to Na2CrO4
Ag2CrO4
compare Cl zero and Cl negative
Cl zero atom contains fewer electrons than the Cl negative ion
increasing atomic radius
Na, K, Rb
quantum numbers for 3d^4
3,2,-1,1/2
greatest difference between its first and second ionization energies
potassium
frequency of blue light
7.5 times 10 to the 14
wavelength of sodium light
5.9 times 10 to the -7
energy of photon of red light
2.84 times 10 to the -19
ionic equation for NaCl +AgNO3= NaNO3+ AgCl
Ag + Cl= AgCl
insoluble in water
CaCO3
soluble in water
K2S
precipitate formed from ammonium phosphate and calcium sulfate
Ca3(PO4)2
orbital designation for an electron with n=4 and L=3
4f
electron configuration that isn’t possible
1s^2 2s^2 2p^6 3s^3 3p^4
not possible configuration for an atom in excited state
1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2
increasing atomic size
Br, As, V, Sc, K
electron affinity equation
atom + electron= ion
metallic elements
low ionization energies
formula for Hg2Cl2
mercury 1 chloride
not a correct formula
KCr2O7
sulfate polyatomic ion
SO4 negative 2
empirical formula of CH2 and mass of 83.5 what is molecular formula
C6H12
empirical formula for compound made of carbon and hydrogen that is 14.3% H
CH2
gram molar mass of Al(NO3)3
213
2 L container will hold 4g of what
CO2
8g of N2H4 and 92g of N2O2 mixed, how much H2O is made
9 grams
propane burns in excess oxygen, what is coefficient of O2
7
volume of H2 when excess Mg is added to .4 M HCl
448 mL
volume of O2 required to react with excess CS2 to make 4 L of CO2
12 L
mass of CuSO4 with water required to make .1 M copper sulfate
6.2 grams
compound with 1.1 mole of K, .55 moles of Te and 1.65 moles of O
K2TeO3
partial pressure of SO2 in flask
160 mmHg
greatest rate of effusion through pinhole
Ne
mass ratio of chromium to oxygen closest to 1.6 to 1
CrO2
pressure of gas at 27 C
.6 Atm
change the boiling point of a liquid
smaller container, more moles, higher altitude
info needed to calculate molarity
molar mass of sucrose
formula for hydrocarbon with 1.88 density
CH2
with info, density of sample is
2 grams per cm
what gas effuses at half rate of NH3
Cl2
mass of Au made when .05 moles of Au2S3 is reduced with excess H2
19.7 grams
coefficient of O2 for C10H12O4S +O2= CO2 + H2O
12
what happens to gas in tank when more oxygen is added
volume of gas increases
empirical formula for 62.2% Hf and 37.4% Cl
HfCl3
pressure of flask of NH4NO3 at 400 K
1 Atm
percent water in hydrate Na2Co3 times 10H2O
63%
height of column of water of barometer
33.9
object moves from moon to Earth
mass will stay same and weight will increase
formula for Hydrogen arsenide
H3As
when real gas is most like ideal gas
low pressure and high temperature
ideal gases
have no volume or attractive forces between them

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