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WorksheetsBonding Unit Exam
Total questions: 34
Worksheet time: 17mins
A molecule with a region of positive charge and a region of negative charge is:
Polar
Ionic
Nonpolar
Metallic
What intermolecular force allows H2O to have a higher boiling point than H2S?
London dispersion forces
dipole-dipole forces
ionic bonding
hydrogen bonding
A dipole is formed in a ________ molecule
Polar
Nonpolar
Ionic
Which is stronger: Covalent bonds or intermolecular forces?
Covalent bonds
Intermolecular forces
The force between a positive region of one molecule and the negative region of another is called a:
orbital force
lattice force
dipole-dipole force
london dispersion force
The strength of London dispersion molecules depends on:
The molecule's mass
The molecule's number of protons
The molecule's number of electrons
The molecule's number of neutrons
What is the molecular shape of CO2, using VSEPR theory.
tetrahedral
linear
bent
trigonal planar
According to VSEPR theory, the shape of an AB3 molecule is
trigonal planar
trigonal pyramidal
bent
tetrahedral
According to VSEPR theory, the shape of a AB3E molecule is:
trigonal planar
trigonal pyramidal
trigonal bipyramidal
tetrahedral
According to VSEPR theory, the shape of an AB2 molecule is:
trigonal planar
bent
linear
tetrahedral
The theory for predicting the shape of molecules is called:
Valence Shell Electron Pair Repulsion (VSEPR) Theory
Valence Electron Shell Pair Repulsion (VESPR) Theory
Molecular Geometry Theory
Molecular Shape Theory
What happens when there is a shift in the crystal lattice structure?
It emits light
It becomes metallic
It breaks apart
It conducts electricity better
Metallic bonding gives metals all of the following characteristics, EXCEPT:
Malleability
Ductility
Low melting point
High Conductivity
Malleability is due to the ability for ions to move and slide past each other in metals.
False
True
What gives metals luster?
covalent bonds
brittle crystalline structure
positive ions
sea of valence electrons
What is a unique characteristic to metallic bonding?
Electron sea
Lewis structures
Electron cloud
Dipole
Which type of bonding has the lowest melting point?
Ionic
Covalent
Metallic
In ionic compounds, when lattice energy increases:
Bond strength increases
Bond strength decreases
The ions in an ionic compound are typically arranged into:
molecule
lewis structure
crystal lattice
trigonal planar structure
In lewis structures, all bonded atoms (except H) will have how many valence electrons?
6
8
2
5
Which of the following molecules has a Lewis structure with two bonds?
H2O
NH3
CH2Cl2
CCl4
What do you need to know when drawing a Lewis structure?
atomic mass of each atom
atomic number of each atom
bond length of each atom
the number of valence electrons in each atom
When drawing Lewis structures, all of the following are true regarding the central atom EXCEPT:
Carbon will always be in the center when present.
Hydrogen will never be in the center
the least electronegative atom will be the center atom
the most electronegative atom will be the center atom
How many valence electrons does Hydrogen need to be stable?
6
8
2
5
Which group of elements does not need to bond to achieve a full octet?
alkali metals
noble gases
halogens
alkaline earth metals
When two iodine atoms are bonded, formed I2, how many electrons are shared between the atoms?
1
2
3
4
Which of the following is an ionic compound?
CsO
H2O
O2
NH3
A molecule is held together by
ionic bonds
covalent bonds
metallic bonds
hydrogen bonds
A difference in electronegativity of 2.0 between two atoms, indicates what bond is formed?
polar covalent
nonpolar covalent
ionic
metallic
As the difference in electronegativity increases between two bonded atoms, the higher the ______________.
ionic character
covalent character
metallic character
electron sharing
which do we see more of: polar or nonpolar covalent bonding?
nonpolar covalent
polar covalent
Why are polar covalent bonds more common that nonpolar covalent bonds?
one atom usually attracts electrons more strongly than the other.
ions always form when atoms join.
the electrons usually remain equally distant from both atoms.
dipoles are rare in nature.
When two identical atoms are covalently bonded, the bond is:
Polar
Nonpolar
What electrons play a role in chemical bonding?
Lewis electrons
Dipoles
s electrons
Valence electrons
