hey all.
i have my uni chem exam coming up.. which involves alot from year 12 chem.
ive done about 300 questions and here are just some that im struggling little bit with.
ive done most of them , however if people could do them i can also get some proper working out + check my answers and id really really appreciate the help.
Question 2 Multiple Choice 1 points
Question 2 text Iron (II) sulfate reacts with potassium hydroxide in aqueous solution to form a precipitate. The ionic equation for this reaction is:
Question 2 answers
2 K+ + SO4-2→ K2SO4
Fe2+ + 2 OH-→ Fe(OH)2
K+ + Fe2+→ Fe3+
Fe+2 + SO4-2→ FeSO4
2 Fe3+ + 3 SO4-2→ Fe2(SO4)3
Question 3 Multiple Choice 1 points
Question 3 text How many 3d electrons does an Fe3+ ion have ?
Question 3 answers
6
5
3
8
4
Question 4 Multiple Choice 1 points
Question 4 text Tellurium has which of the following electron configurations?
Question 4 answers
[Xe] 5s24d105p4
[Kr] 5s25p4
[Kr] 5s24d104f145p4
[Kr] 4s23d104p4
none of these
Question 5 Multiple Choice 1 points
Question 5 text Arrange sodium, oxygen, fluorine, and strontium in order of increasing first ionization energy.
Do not look up the values! Make a prediction based upon the periodic trend.
Question 5 answers
Na < Sr < F < O
Sr < Na < O < F
Sr < Na < F < O
Na < Sr < O < F
Question 6 Multiple Choice 1 points
Question 6 text Contact lenses can focus light due to the ______ of the waves.
Question 6 answers
diffraction
dispersion
reflection
refraction
Question 7 Multiple Choice 1 points
Question 7 text The shape of an atomic orbital is associated with
Question 7 answers
the magnetic quantum number (ml)
the angular momentum quantum number (l)
the spin quantum number (ms)
the principal quantum number (n)
Question 8 Multiple Choice 1 points
Question 8 text A possible set of quantum numbers for the last electron added to complete an atom of phosphorus in its ground state is n l ml ms
Question 8 answers
3 0 +1 -1/2
4 0 0 +1/2
4 2 +2 -1/2
4 1 -1 +1/2
3 1 +1 -1/2
Question 9 Multiple Choice 1 points
Question 9 text Arrange aluminum, nitrogen, phosphorus and indium in order of decreasing electronegativity. Do not look up the values - predict based upon the trend.
Question 9 answers
P > N > In > Al
N > P > Al > In
N > P > In > Al
N > Al > P > In
Question 10 Multiple Choice 1 points
Question 10 text Which of the following covalent bonds is the most polar (highest percent ionic character)?
Question 10 answers
Si - P
Al - I
Al - Cl
Si - I
Si - Cl
Question 11 Multiple Choice 1 points
Question 11 text The Lewis structure for hydrogen bromide shows around the bromine
Question 11 answers
1 single bonded hydrogen and 3 lone pair of electrons
1 single bonded hydrogen and 2 lone pairs of electrons
1 double bonded hydrogen and 1 lone pair of electrons
1 single bonded hydrogen only
1 single bonded hydrogen and 1 lone pair of electrons
Question 12 Multiple Choice 1 points
Question 12 text Which of the following atoms MUST ALWAYS obey the octet rule?
Question 12 answers
S
Cl
O
Si
Question 13 Multiple Choice 1 points
Question 13 text Predict the shape of NO2+
Question 13 answers
bent (bond angle about 120°°)
tetrahedral
linear
pyramidal (ie trigonal pyramid)
bent (bond angle about 109.5°°)
Question 14 Multiple Choice 1 points
Question 14 text Predict the shape of SO2
Question 14 answers
Linear
Bent (bond angle about 109.5°)
Tetrahedral
Bent (bond angle about 120°)
Trigonal planar
Question 15 Multiple Choice 1 points
Question 15 text
In the Lewis structure for carbon dioxide, CO2, what is the total number of reasonable resonance structures that can be drawn?
Question 15 answers
4
2
3
1
Question 16 Multiple Choice 1 points
Question 16 text Complete this sentence: The ICl5 molecule has
Question 16 answers
nonpolar bonds, but is a polar molecule.
polar bonds, and is a nonpolar molecule.
polar bonds, and is a polar molecule.
nonpolar bonds, and is a nonpolar molecule.
Question 17 Multiple Choice 1 points
Question 17 text Bonds are formed between atoms because...
Question 17 answers
the energy state of the bonded atoms is greater than when they are separated
they want to trade electrons
the energy state of the bonded atoms is less than when they are separated.
the energy of the bonded atoms is an even number
An inflated balloon has a volume of 0.910 L at sea level where the temperature is 15°C and the pressure is 0.870 atm. The balloon rises to a height of 4.23 km where the temperature is
-24°C and the pressure is 0.310 atm. What is the final volume of the balloon ?
Question 20 answers
2.208 L
1.877 L
4.086 L
1.987 L
17.626 L
Q2: ans is Fe2+ + 2 OH-→ Fe(OH)2, it is a precipitation reaction in which Fe2+ and OH- come together
Q3: 5; Fe3+ is [Ar]3d^5
Q4: none of these; the actual configuration is [Kr] 5s24d105p4
Q5: Sr < Na < O < F, Sr is HUGE (easy to rip electron), Na+ is stable, O and F are small and O+ and F+ are unstable, F+ more so than O+ because of higher core charge on F.
Q6: refraction - light can change direction coz of a lens
Q7: the angular momentum quantum number (l) [this determines whether the shell is s, p, d, etc.] although ml is also really important as it can determine orientation...i'd go with ml i think...
Q8: 3 1 +1 -1/2; use Aufbau principle and Hund's Rule. P is 1s2 2s2 2p6 3s2 3p3
Q9: N > P > Al > In. The further down and further left of periodic table you go, the electronegativity decreases.
Q10: Al - Cl, use electronegativity values
Q11: 1 single bonded hydrogen and 3 lone pair of electrons. Draw lewis structure of H-Br.
Q12: O - electrons cannot be promoted to a d-subshell as electrons only in first and 2nd shells. For molecules to break octet rule, it must be possible to promote electrons to a d-subshell for the central atom (exceptions include BeCl2 and AlCl3...where metalloids are involved)
Q13: linear. draw Lewis structure, then use VSEPR
Q14: Bent (bond angle about 120°). Draw lewis structure...there are two oxygens and a lone pair around the sulfur.
Q15: 3. double bonds from C to both Os, one bond to one O and 3 to another, and the reverse.
Q16: polar bonds, and is a polar molecule. Electronegativities are highly different, and molecule is square planar (5 bonding pairs + 1 lone pair around I)
Q17: the energy state of the bonded atoms is less than when they are separated. Main principle is that atoms want to be at lower energies
last Qn: 2.208 L. Use P1V1/T1 = P2V2/T2.
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