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Terms in this set (102)
A small amount of salt dissolved in water is an example of a
which of the following is NOT intensive property?
e. boiling point
accuracy refers to __.
how close a measured number is to the true value.
what is the formula of the compound formed between strontium ions and nitrogen ions?
which of the following pair of compounds do not have the same empirical formula?
the formula weight of potassium dichromate (K2Cr2O7 is __amu.
Gold has a density of 19.32 g/cm3. What is volume (in cm3) would be occupied by a 0.504 kg sample of gold?
v=m/d x 1000 g divide 1 kg
8.24 km = in
8.24 km | 10^3 m | 10^2 cm | 1 inch
| 1 km | 1 m | 2.54 cm
=3.24 x 10^5
the correct answer (reported to the proper number of significant figures) to the following is _.
12.67 + 19.2
1.360 + 11.3665
12.67 + 19.2 = 31.87. = 31.9
1.360 + 11.3665 12.7265 12.727
coper (II) oxide
iron (III) sulfate
Balance the equation
_ C5H12 + _ O2 -> _ CO2 + _ H20
_ Na + _ H2O _ -.> _ NaOH + _ H2
What is the empirical formula of a compound that contains 27.0% S, 13.4% O, 59.6 % Cl by mass?
Calculate the number of molecules of glucose in 30.5 grade, sample of glucose (C6H12O6).
1.02 x 10^23 C6H12O6
The reaction 2H2(g) + O2(g) -> 2 H20(g) is used to produce electricity in a hydrogen fuel cell. Suppose a fuel cell contains 150 mol H2 (g) and 100 mol O2 (g) (a) Which is the limiting reactant? (b) how many moles of water can form? [use limiting reactant concept]
b) 150 mol H2O
CaC2 (s) + 2 H2O (g) -> Ca(OH)2 + C2H2 (g)
what is the amount of Ca(OH)2 formed (in grams) after the complete reaction of 35.5 g CaC2 with express water?
41.03 g Ca(OH)2
what is the oxidation number of sulfur in Na2SO3?
acids are proton _ and bases are proton _.
in the following chemical reaction, _ is oxidized and _ is reduced.
2 Al (s) + 6 HBr (aq) -> 2 AlBr3 (aq) + 3 H2(g)
When a system ________, ΔE is always negative.
gives off heat and does work
which one of the following statements is true?
Enthalpy is a state function
The value of ΔE for a system that performs 111 KJ of work on its surrounding and gains 89 Kj of heat is _kj
which one of the following is an exothermic process?
condensation of water vapor
the kinetic-molecular theory predicts that pressure rises as the temperature of a gas increases at constant volume because
both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall.
of the following gases, _ will have the greatest rate of effusion at a given temperature.
what is the concentration (Molarity) of a NaCl solution prepared by dissolving 9.3 g NaCl in sufficient water to give 350 mL of solution?
What volume (mL) of a concentrated solution of sodium hydroxide (8.00 M) must be diluted to 100.0 mL to make a 2.00 M solution hydroxide? (dilution problem)
How many grams of Ca(OH)2 are needed to neutralize 50.0 mL of 0.500 M HNO3?
A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample increases from 21.5 C to 28.5. if the specific heat capacity (Cs) of iron is 0.450 j/g- C, what is the mass (in grams) of the sample?
The value of ΔH for the reaction below is -482 kj. Calculate the heat (kj) released to the surroundings when 38.5 g of O2 (g) reacts with excess CO. 2CO (g) + O2 (g) -> 2 CO2(g)
The pressure of a sample of CH4 gas (6.022 g) in 30.0 L vessel at 393 K is
An inflated ballon has a volume of 4.0 L at sea level (1.0 atm) and is allowed to amend until the pressure is 0.35 atm. During ascent, the temperature of the gas falls from 25 C to -12 C. Calculate the volume of the ballon at its final altitude.
v2= 10.0 L
The metabolic oxidation of glucose C16H1206 in our bodies produces CO2, which is expelled from our lungs as a gas:
C6H1206 (aq) + 6O2 (g) -> 6CO2 (g) + 6H2O (1)
Calculate the volume of dry CO2 gas produced at body temperature (37 C) and 0.970 atm when 24.5 g of glucose is consumed in this reaction.
The density of NO2 gas in a tank at 780.0 mmHg and 310 K is
Of the molecules below, the bond in _ is the most polar
The ion SO4 ^2-
How many peak maxima does red light with a wavelength of 649nm pass in one second? (Frequency)
4.6 x 10^14 s^-1
3.00 x 10^8 m/s
? nm then multiple it by 10^9 nm
Wavelength (c/frequency )
3.00 x 10^m/s
? s^-1 then multiple it by 10^9 nm
The yellow light given off by a sodium vapor lamp used for public lighting has a frequency of 5.09 x 1014 s-1. What is the wavelength of this radiation in nm?
energy (E = hυ) of light or photons
(6.00 x 10^-34 J.s ) (3.00 x 10^m/s )
? nm then multiple it by 10^9
A photon of red light has a wavelength of 649 nm. How much energy is in a single photon of this red light?
3.06 x10 ^-19 J
change in energy for electronic transitions in hydrogen atom
E ^= (-2.18 x 10^-18 J) (1/ nf ^2 - 1/ni ^2 )
What is the wavelength of light that is emitted when an electron in a hydrogen atom relaxes from the 5th energy level to the 2nd?
4.35 x 10-7 m or 435 nm
Calculate the change in energy when an electron jumps from 3rd energy level to 1st energy level?
-1.94 x 10-18 J
wavelength of light that is emitted
1) E ^= (-2.18 x 10^-18 J) (1/ nf ^2 - 1/ni ^2 )
2) (6.626x 10^-34 J.S) (3.00 x 10^8 m/s)
Heisenberg uncertainty principle
states that it is not possible to know precisely both the velocity and the position of a particle at the same time
The __ quantum number defines the shape of an orbital.
the energy of a photon of light is __proportional to its frequency and __ proportional to its wavelength.
n of orbital in a shell (multiple by itself)
Maximum electrons f-shell can hold
Maximum electrons d-shell can hold
Maximum electrons p-shell can hold
which of the following is a valid set of four quantum numbers? (n, I, mI, ms)
2, 1, 0, +1/2
which subshells below do not exist due to the constraints upon the angular momentum quantum number?
effective nuclear charge
Zeff= atomic number - period number
similar chemical properties
elements in the same group have
in the generation of most anions, the energy change (KJ/ mol) that __ an electron is __.
atoms that have the same number of electrons.
O^2- , F-, Na+, Mg2+,
the electrostatic attraction that binds oppositely charged ions together
sharing of electrons
the same element is least polar _
most polar Li and F _
closer together and farther apart
when run out of electrons for the center add a bond or even the structure
more towards the top
On a phase diagram, the triple point is where __________.
no phases are in equilibrium
On a phase diagram, the critical temperature is __________.
the temperature above which a gas cannot be liquefied
Viscosity is __________.
The resistance to flow
Large intermolecular forces in a substance are manifested by __________.
-low vapor pressure
-high boiling point
-high heats of fusion and vaporization
-high critical temperatures and pressures
all of the above
The shape of a liquid's meniscus is determined by __________.
the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container
Which one of the following hydrogen will form the strongest hydrogen bond?
When NaCl dissolves in water, aqueous Na+ and Cl- ions result. The force of attraction that exists between Na+ and H2O is called a(n) __________ interaction.
Of the following, __________ has the highest boiling point.
The strongest interparticle attractions exist between particles of a __________ and the weakest interparticle attractions exist between particles of a __________.
Of the following substances, only __________ has London dispersion forces as its only intermolecular force.
The hybridization scheme for BeF2 is __________.
ClF3 has "T-shaped" geometry. There are __________ non-bonding domains in this molecule.
PCl5 has __________ electron domains and a __________ molecular arrangement.
5, trigonal bipyramidal
The sp2 atomic hybrid orbital set accommodates __________ electron domains.
There are __________ σ bonds and __________ π bonds in H-C≡ C-C≡C-H
A typical triple bond __________.
consists of one σ bond and two π bonds
The electron domain and molecular geometry of BrO2- is __________.
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
According to valence bond theory, which orbitals overlap in the formation of the bond in HBr?
1s on H and 4p on Br
The molecular geometry of the PF3 molecule is __________, and this molecule is __________.
trigonal pyramidal, polar
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