18 Questions
In VSEPR theory, what is the bond angle for a molecule with a trigonal bipyramidal shape?
90° and 120°
Which type of bond is known as a non-polar covalent bond?
Single covalent bond
What is the bond angle for a molecule with a bent shape?
104.5°
Which molecule has a trigonal planar shape?
BF3
How does VSEPR theory explain molecular geometry?
By considering the number of lone pairs and atoms around the central atom
Which molecule exhibits an octahedral shape?
SF6
What does it mean for a molecule to have a net dipole?
The individual bond dipoles do not cancel each other out and create a positive and negative end.
Which theory explains how atomic orbitals overlap to form a new orbital with a pair of opposite-spin electrons?
Valence Bonding Theory
In Valence Bonding Theory, when does a covalent bond form?
When two atomic orbitals overlap and each has an unpaired electron.
How can you determine if a molecule is polar or non-polar?
By considering the shape of the molecule and the type of bonds.
What is the result when the sum of individual bond dipoles in a molecule is zero?
The molecule is non-polar.
Which type of molecules can have polar bonds but still be non-polar overall?
Molecules with symmetric geometry.
What is the purpose of VSEPR Theory?
To determine the shape of molecules based on minimizing repulsive forces
How does sulfur hexafluoride (SF6) violate the octet rule?
By having more than 8 valence electrons
In a coordinate covalent bond, where do the electrons involved in the bond come from?
Only one atom
What is the general trend for following the octet rule among C, N, O, and F atoms?
All follow the octet rule consistently
What type of bond occurs when S atoms exceed the octet rule by filling vacant nearby d orbitals?
Coordinate Covalent Bond
What does Three-Dimensional Structure in chemistry refer to?
The shape of a molecule and how atoms are arranged in 3D space
Learn about exceptions to the octet rule in Lewis structures, where bonding electrons are represented by solid lines and lone pairs are shown. Understand why some elements like Boron may have an unfilled octet, while others like C, N, O, and F follow the octet rule. Explore examples like BF3 (boron trifluoride) and its reactivity with electron-rich molecules.
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