Corrigan Final
The liquid hydrogen halides have the normal boiling points given above. The relatively high point of HF can be explained by which of the following? HF +19 HCl -85 HBr -67 HI -35
HF bonds with Hydrogen
Explain the fact that the four bonds in methane are equivalent
Hybridization
Explain why the boiling point of HF is greater than the boiling point of HBr
Hydrogen Bonding
Which of the following represents an isotope?
It must have a higher top number than normal
Explain why iodine molecules are held together in the solid state
London Dispersion Forces
Forms a compound having the formula KXO4
Maganese
Atoms of an element X have the electronic configuration shown above. The compound most likely formed with Mg is
Mg3X2/ add up electrons
Contains the element nitrogen
N2
Which of the following elements in its elemental state, forms triple bonds?
Nitrogen
Which of the following molecules has the shortest bond length?
Nitrogen has triple bonds
The density of an unknown gas is 4.2 grams per liter at 3.00 atmospheres pressure and 127*C. What is the molecular weight of the gas?
P=303.9kPa (3 atm) V=1.00L n=? R=8.315 T=400K Rearrange to find 'n' n=PV/RT n=303.9x1/8.315x400 n=9.14x10^-2moles n=m/M M=m/n M=4.20/(9.14x10^-2) M=45.9g/mol
The ground-state configuration of a common ion of alkaline earth element
1s^2 2s^2 2p^6 3s^2 3p^6
The ground-state configuration of a negative ion of a halogen
1s^2 2s^2 2p^6 3s^2 3p^6
The ground-state configuration for the atoms of a transition element
1s^2 2s^2 2p^6 3s^2 3p^6 3d^3 4s^2
An impossible electronic configuaration
1s^2 2s^3 2p^6 3s^2
When 70. millimeter of 3.0-molar Na2CO3 is added to 30. millimeter of 1.0-molar NaHCO3 the resulting concentration of Na is?
2*.07(3mol)Na from the first one and .03(1mol)Na from the 2nd one so .42 + .03=.45mols of Na+ ions in 100ml the molarity is .45/100ml=.45/.1L which is 4.5Molar solution
has the lowest pH when placed in water
All3
The elements in which of the following have most nearly the same atomic radius?
look for what row in chart
When a sample of oxygen gas in a closed container of a constant volume is heated until its absolute tempature is CHANGED which of the following is also CHANGED?
pressure of gas
XXX + 3XXX ==> XXX According to the data in the table below, what is the value of Delta H for the reation represented above? Remember Delta H = bonds formed...
reactants added then minus the product
Has no acid/base properties
salts
Has amphoteric properties (C) A molecular solid with hydrogen bonding
solid ethyl alcohol
When phenolpthalein is used as the indicator in a titration of an HCl solution with a solution of NaOH the indicator undergoes a color change from clear to red at the end point of the titration. This color change occurs abruptly because
the solution being titrated undergoes a large PH change near the end point of the titration
The geometry of the SO3 molecule is best described as
(A) trigonal planar
N2(g)+3H2(g)==> 2NH3(g) The reaction indicated above is thermodynamically spontaneous at 298K but becomes non-spontaneous at higher temperatures. Which of the following is true at 298 K?
/\G, /\H, and /\S are all negative.
A student wishes to prepare 2.00 liters of a 0.100-molar KIO3(molecular weight XXX.) The proper procedure is to weigh out
42.8 g of KIO3 and add H2O until the solution reaches 2 moles
When XXX decays the emission consists consecutively of an A particle, then two B particles and finally another A particle. The resulting stable nucleus is
Alpha particle = -2 protons, -2 neutron | -4 nucleons Beta particle = +1 proton, -1 neutron | +0 nucleons 84 - 2 + 1 + 1 - 2 = 82 Protons + Alpha decay + Beta Decay*2 + Alpha Decay = Resultant Protons 214 - 4 + 0 + 0 - 4 = 206 Nucleons + Alpha decay etc. So the answer is C
Has the most stable electron configuration
Argon
A cube of ice is added to some hot water in a rigid insulated container, which is then sealed. There is no heat exchange with the surroundings. What has happened to the total energy and the total entropy when the system reaches equilibrium?
D) Energy decreases and entropy increases
Has amphoteric properties (A) a network solid with covalent bonding
Silicon dioxide
Forms monotomic ions with 2-charge in solutions
Sulfur
CH3CH2OH boils at 78*C and CH3OCH3 boils at -24*C although both compounds have the same composition. This difference in boiling points may be attributed to a difference in.
The ether (CH3OCH3) has only dipole-dipole forces in addition to the London dispersion forces. Hydrogen bonds are much stronger forces, so the alcohol has the higher boiling point
What is the most electronegative element above
The more electrons an atom has the more it will want more
The radioactive decay of 14 6C to XXX occurs by the process of
beta decay
The net ionic reaction between XXX and XXX is?
cancel spectator ion and split up elements soluable in water
Hydrogen gas is collected over water at 24*C. The total pressure of the sample is XXX millimeters of mercury. At 24*C the vapor pressure of water is XX millimeters of mercury. What is the partial pressure of the hydrogen gas?
use PV=nRT find P with any given mole set
The pH of 0.1-molar XXX is approximately
use X^2/x-m=Kb
Which of the following represents the ground state electron configuration for the XXX ion?
use chart
For which of the following processes would Delta S have a negative value?
when things are merging