An ionic bond is best described as
the sharing of electrons
the transfer of electrons from one atom to another
the attraction that holds the atoms together in a polyatomic ion
the attraction between 2 nonmetal atoms
the attraction between 2 metal atoms
A covalent bond is best described as
the sharing of electrons between atoms.
the transfer of electrons
a bond between a metal and a nonmetal
a bond between a metal and a polyatomic ion
a bond between two polyatomic ion
Write the name for Sn(SO4)2. Remember that Sn forms several ions
tin (I) sulfite
tin (IV) sulfate
tin sulfide
tin (II) sulfite
tin (I) sulfate
Give a possible molecular formula for C3H5ClO.
C6H10ClO2
C5H10Cl2O2
C6H10Cl2O2
C6H10O2
C6H12Cl2O2
Determine the name for TiCO3. Remember that titanium forms several ions
titanium (II) carbonate
titanium carbide
titanium carbonite
titanium (II) carbonite
titanium (I) carbonate
Give the correct formula for aluminum sulfate.
Al2SO4
Al(SO4)3
Al3(SO4)2
Al2(SO4)3
Calculate the molar mass of Ca3(PO4)2
87.05 g/mol
215.21 g/mol
310.18 g/mol
279.21 g/mol
246.18 g/mol
How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol.
1.23 × 1023 O atoms
2.96 × 1024 O atoms
2.87 × 1025 O atoms
1.10 × 1024 O atoms
3.68 × 1023 O atoms
Calculate the mass percent composition of lithium in Li3PO4
26.75 %
17.98 %
30.72 %
55.27 %
20.82 %
Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and an empirical formula of C2H5O2.
C2H5O2
C6H15O6
C3H7O3
C4H10O4
C8H20O8
Determine the empirical formula for a compound that contains C, H and O. It contains 52.14% C and 34.73% O by mass.
C2H6O
CHO
C4H13O2
CH4O3
CH3O
Draw the Lewis structure for S2⁻
Draw the Lewis structure for Ca2+
Draw the Lewis structure for N
Give the complete electronic configuration for Br-.
1s22s22p63s23p64s24p6
1s22s22p63s23p64s24d104p6
1s22s22p63s23p64s23d104p6
1s22s22p63s23p64s23d104p5
1s22s2p63s2p64s23d104p6
Place the following in order of decreasing magnitude of lattice energy. K2O Rb2S Li2O
Li2O > K2O > Rb2S
Li2O > Rb2S > K2O
Rb2S > K2O > Li2O
Rb2S > Li2O > K2O
K2O > Li2O > Rb2S
Use Lewis theory to determine the chemical formula for the compound formed between Rb and O
RbO
RbO2
Rb2O
Rb2O3
Rb3O2
What type of bonding is found in the compound HCl?
covalent bonding
hydrogen bonding
ionic bonding
metallic bonding
Which of the following is an ionic compound?
SBr2
Mg3(PO4)2
Cl2O
CH2O
PBr5
Give the name for PCl3
phosphorus trichloride
potassium trichloride
phosphorus (III) chloride
phosphorus (II) chloride
phosphorus chloride
A single covalent bond
0 electron pairs
1 electron pairs
2 electron pairs
3 electron pairs
is the shortest
4 electron pairs
is the strongest
is the weakest
does not exist
is the longest
A double covalent bond
A triple covalent bond
A quadruple covalent bond exists
Identify the compound with the largest dipole moment in the gas phase
LiF
HF
ClF
Cl2
Identify the compound with the smallest dipole moment in the gas phase
Draw the best Lewis structure for BeF2. State the EG, the MG, and the hybridization for your answer.
Using periodic trends, place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S
Si-P < Si-Cl < Si-S
Si-P < Si-S < Si-Cl
Si-S < Si-Cl < Si-P
Si-Cl < Si-P < Si-S
Si-Cl < Si-S < Si-P
Give the number of valence electrons for ICl5.
36
40
42
44
46
Draw the best Lewis structure for XeI2. State the EG, the MG, and the hybridization for your answer.
Draw the best Lewis structure for SF4. State the EG, the MG, and the hybridization for your answer.
Draw the best Lewis structure for NO3⁻. State the EG, the MG, and the hybridization for your answer
Which of the following resonance structures for OCN⁻ will contribute most to the correct structure of OCN⁻? (LP=lone pair)
O(2 LP’s) C N (2 LP’s)
O(1 LP) C-N(3 LP’s)
O(1 LP) C(2 LP’s) N(1 LP)
O(3 LP’s)—C N(with 1 LP)
They all contribute equally to the correct structure of OCN⁻
Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule.
PF3 < OF2 < PF4⁺
OF2 < PF4⁺ < PF3
PF4⁺ < OF2 < PF3
PF4⁺ < PF3 < OF2
OF2 < PF3 < PF4⁺
How many of the following molecules are polar? PCl5 COS XeO3 SeBr2
2
1
0
4
3
Give the hybridization for the O in OF2. State the EG and the MG for your answer
Give the hybridization for the Br in BrF5. State the EG and the MG for your answer
A single covalent bond has sigma and pi bonds
A Double covalent bond has sigma and pi bonds
A triple covalent bond has sigma and pi bonds
Describe a pi bond
side by side overlap of parallel p orbitals
s orbital overlapping with the end of a d orbital
end to end overlap of p orbitals
overlap of two d orbitals
p orbital overlapiing with an f orbital
describe a sigma bond
s orbital overlapping with the side of a p orbital
p orbital overlapping with an f orbital
