WorksheetsVSEPR Theory Quiz
Total questions: 30
Worksheet time: 16mins
What does VSEPR stand for?
Valence Shell Electron Pair Repulsion
Valence Shell Electron Proton Reaction
Variable Shell Electron Pair Repulsion
Valence Shell Energy Pair Reaction
Who developed the concept mentioned in the introduction in 1957?
Linus Pauling and Gilbert Lewis
Ronald Gillespie and Ronald Nyholm
Marie Curie and Ernest Rutherford
Dmitri Mendeleev and John Dalton
What is the primary use of the concept for the VSEPR Theory?
Prediction of atomic mass
Prediction of polyatomic molecules and covalent bonding
Determination of isotopes
Calculation of molecular weight
What determines the shape of a molecule according to the VSEPR theory?
The type of bonds present in the molecule
The repulsions between all electron pairs in the valence shell
The number of atoms in the molecule
The mass of the central atom
What happens to electron pairs in the valence shell of the central atom according to the VSEPR theory?
They attract each other to form bonds
They repel each other and align to minimize repulsion
They remain stationary around the central atom
They are shared equally among all atoms
Which type of electron pair takes up more space around the central atom?
Bond pair
Lone pair
Shared pair
Valence pair
What is the difference between a lone pair and a bond pair of electrons?
A lone pair is shared by two nuclei, while a bond pair is not
A lone pair is attracted to one nucleus, while a bond pair is shared by two nuclei
A lone pair forms a bond, while a bond pair does not
A lone pair is in the inner shell, while a bond pair is in the valence shell
What is the result of minimizing repulsions between electron pairs in a molecule?
Maximum energy and minimum stability
Minimum energy and maximum stability
Equal energy and stability
Increased repulsion and decreased stability
Which type of electron pair interaction results in the strongest repulsion?
Lone pair near another lone pair
Lone pair near bonded pair
Bonded pair near another bonded pair
Single bond near double bond
What is the repulsion strength of a lone pair of electrons near a bonded pair compared to a lone pair near another lone pair?
Stronger
Slightly less repulsive
Weakest
Equal
Which statement is true regarding the repulsion strength of bonds?
Single bond has more repulsion than double bond
Double bond has more repulsion than triple bond
Triple bond has more repulsion than double bond
Single bond has more repulsion than triple bond
What causes a slight distortion of bond angles from the ideal shape in a molecule?
The presence of lone pairs on the central atom
The absence of lone pairs on the central atom
The presence of double bonds
The absence of bonding pairs of electrons
What does the magnitude of repulsions between bonding pairs of electrons depend on?
The electronegativity difference between the central atom and the other atoms
The size of the central atom
The number of lone pairs on the central atom
The number of bonds in the molecule
Which factor is most likely to cause a molecule to distort from its ideal bond angle?
The presence of lone pairs on the central atom
The presence of triple bonds
The absence of electronegativity differences
The symmetry of the molecule
What is the first step in predicting the geometry of a compound?
Draw the electron dot structure and bar diagram
Determine the central atom
Find the arrangement of bonding pairs
Determine the geometry based on the bonding pairs
Which of the following statements about hydrogen in a molecule is correct?
Hydrogen is always the central atom.
Hydrogen is always terminal.
Hydrogen is always bonded to the most electronegative atom.
Hydrogen is always bonded to the least electronegative atom.
What is the purpose of drawing the electron dot structure and bar diagram in predicting compound geometry?
To determine the central atom
To find the arrangement of electron pairs
To determine the geometry based on bonding pairs
To identify the terminal atoms
What is the final step in predicting the geometry of a compound?
Determine the central atom
Draw the electron dot structure and bar diagram
Determine the geometry based on the bonding pairs
Find the arrangement of electron pairs
What is the bond angle in a tetrahedral molecular shape?
180°
120°
109.5°
90°
What is the bond angle in BeH₂?
90°
120°
180°
109.5°
What is the bond angle in a molecule with a trigonal planar arrangement, such as BF₃?
90°
109.5°
120°
180°
What happens to phosphorus during promotion in the context of PCl₅ formation?
It loses an electron.
It excites an electron into an empty 3d orbital.
It gains an electron.
It forms a double bond.
In a regular octahedron, how many and what shapes make up the structure?
A net of a regular octahedron consists of 8 equilateral triangles.
A net of a regular octahedron consists of 6 squares.
A net of a regular octahedron consists of 12 pentagons.
A net of a regular octahedron consists of 4 hexagons.
Which of the following correctly describes the Lewis structure, 3D molecular geometry, and bond angles of SF₄?
SF₄ has a see-saw molecular geometry with bond angles of approximately 90°, and 120°
SF₄ has a tetrahedral geometry with bond angles of 109.5°.
SF₄ has a trigonal planar geometry with bond angles of 120°.
SF₄ has a linear geometry with bond angles of 180°.
What is the molecular geometry of a central atom with six electron pairs and two lone pairs?
Tetrahedral
Trigonal Bipyramidal
Square Planar
Octahedral
Why must the lone pairs in a molecule with six electron pairs and two lone pairs be the farthest apart?
To minimize attraction
To maximize bonding
To minimize repulsion
To maximize lone pair interaction
What is the bond angle for the CH4 molecule?
120°
107°
109.5°
90°
Which geometric molecular shape is shown?
trigonal planar
linear
bent
trigonal pyramidal
Which of the following statements is true when comparing the bonding patterns of CH4 and H2O?
CH4 would form a tetrahedral with a 109.5° bond due to four bonding pairs. H2O also has four pairs, but two are lone pairs leading to a distortion of the 109.5° angle and bent shape.
CH4 would form a tetrahedral with 109.5° bond angles. H2O would also form the same shape with the same bond angles.
CH4 would form a tetrahedral with a 120° bond due to four bonding pairs. H2O also has four pairs, but two are lone pairs leading to a distortion of the 120° angle and bent shape.
CH4 would form a tetrahedral with a 180° bond due to four bonding pairs. H2O also has four pairs, but two are lone pairs leading to a distortion of the 180° angle and bent shape.
