Chemistry diagnostic test (Topic 12)
1.
B – the p4 config. of S is less stable, electron- electron repulsion.
2.
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A – B is lower than Be because two s electrons shield the 2p electrons
E – Au and Ag both have full d orbitals(10electrons) (s1 )
E – electronegativity increases from lower left to upper right (F-most
electronegative)
B – sulfur’s oxidation numbers: 2-, 2+, 4+, 6+
A – atomic radii increase right to left and top to bottom
C – cations are smaller, the higher the charge the smaller the cation
A – Group 1 has low 1st ionization energy, but 2nd is pulling an inner core
electron(big jump)
E – equal moles - 0.25
D – greatest molar mass
D – greatest mass/volume
E – all same temp
E – Phosphorus – high reactivity with oxygen not found free in nature
B – not all have a 2+ oxidation
A – all substances contain London dispersion forces
D – hydrogen must be bonded to nitrogen, oxygen or fluorine
A – propane (molar mass – 44) dispersion forces only – lowest temp
Ethanol (molar mass – 46) also has hydrogen bonding
Water (molar mass – 18) very strong hydrogen bonds
C
A – balanced equation is
Na2CO3 + 2HCl  2NaCl + CO2 + H20
Limiting is sodium carbonate
C – (0.300 moles/L)(.300L) = 0.0900 mol Cl- ion – requires 1/3 as much
aluminum chloride or 0.0300 mol
0.0300 mol/0.500Mormol/L = 0.0600L = 60.0 ml
B - 0.500 M x 0.250L x 200g/mol = 25.0 g
D- 2 C3H8O + 9O2  6CO2 + 8H2O
C – 3.00 carbon = ¼ mole of C therefore ½ mol of Z combines
0.5 mol Z x 36.0 g/mol(3timesC) = 18.0 g Z
E – 4 moles of O
C – an alkali metal reacts with water to produce hydrogen gas and an
aqueous alkali metal hydroxide
D – H2SO4 + NaOH  NaHSO4 + H2O (diprotic acid and monobasic
base
E – X has a 3+ charge
E
B – 1 mole of magnesium requires 2 moles of HCl therefore HCl is
limiting
D – a formation reaction produces 1 mole of a product
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50.
D – A change of phase from gas to liquid to solid is always exothermic.
Phase changes from solid to liquid to gas are always endothermic
D – Tin is the only metal in that family
A – sodium is bright yellow
B – chromium because half-full d orbitals is more stable thatn filled 4s
C – {Ne}3s2 3p4
s
p
C–4p
A – Methane has the smallest molar mass
A – multiple bonds are stronger. CO – triple bond; O2 & NO double;
others single bonds
A – triple bonds are shortest N2 – triple bond
D – single bonds longer and larger atoms – longer bonds
C – 4 bonding pairs 1 nonbonding
C – nitrate, sulfur trioxide and carbonate are all iso electronic (24 valence
electrons) Lewis structure the same – 2 single bonds to oxygen and 1
double bond to oxygen. Sulfite has 26 valence electrons – 3 single bonds
and 1 nonbonding pair on S.
C
D – ammonia is very polar and can hydrogen bond with water. All others
are non-polar and cannot hydrogen bond
C – (see #42)
C – reduction gains electrons. N from 0 to -3
E – sulfur has an oxidation number of 6+. In sulfide S oxidation number
is 2-, a difference of 8 electrons
D – NaOH + Hcl  NaCl +H2o
B – M = (2.00 M)(125.0 mL/500.0 mL) = 0.500M
A – Nitric acid is a strong acid therefore it is a strong electrolyte. It
ionizes completely in aqueous solution