What is the bond axis?

The imaginary line joining two nuclei

Why is H2O molecule polar?

Because of the bent shape of the molecule

Because of the straight shape of the molecule

Because of the curved shape of the molecule

Because of the round shape of the molecule

Ultimate Quiz On Hybridisation

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Questions: 10 | Attempts: 3,681 | Updated: Dec 27, 2023

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Do you understand Hybridization well? Take this ultimate quiz on Hybridisation. Hybridization, also referred to as orbital Hybridization, deals with the concept of mixing atomic orbitals into new hybrid orbitals suitable for pairing electrons to form chemical bonds in valence bond theory. The new hybrid orbitals possess different energy, shapes, etc. Than the component atomic orbitals. If you understand all this well, this quiz will be an easy one for you. All the best! Share the quiz with others interested in this module of chemistry.

Questions and Answers

1.

Which of the following first developed the hybridization theory?
- A.
  
  Linus Pauling
- B.
  
  James Baldwin
- C.
  
  James Watson
- D.
  
  Rosalind Franklin
Correct Answer
A. Linus Pauling

Explanation
Linus Pauling is the correct answer because he was the first to develop the hybridization theory. This theory explains the mixing of atomic orbitals to form new hybrid orbitals during the bonding process. Pauling's work on hybridization greatly contributed to our understanding of chemical bonding and molecular structure.

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2.

How many sigma bonds exist in ethene?
- A.
  
  3
- B.
  
  5
- C.
  
  6
- D.
  
  9
Correct Answer
B. 5

Explanation
In ethene (ethylene), C2H4, each carbon atom forms five sigma (σ) bonds.
Each carbon atom forms a sigma bond with one hydrogen atom and a sigma bond with the other carbon atom. This results in a total of five sigma bonds in ethene.
So, in ethene, there are five sigma (σ) bonds.

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1
5
3.

Lone pairs can be seen through which of the following?
- A.
  
  Lewis structure
- B.
  
  Pauling's theory
- C.
  
  Archimedes principle
- D.
  
  Pauli's exclusion
Correct Answer
A. Lewis structure

Explanation
The correct answer is Lewis structure. Lewis structures are diagrams that show the bonding and lone pair electrons in a molecule. Lone pairs are represented by pairs of dots placed next to the atom. By looking at the Lewis structure, we can determine the presence and location of lone pairs in a molecule. Pauling's theory is related to chemical bonding, Archimedes principle is related to buoyancy, and Pauli's exclusion principle is related to electron configuration and the behavior of electrons in atoms. None of these theories or principles directly provide information about lone pairs.

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3
0
4.

Which of the following is not an example of sp hybridization?
- A.
  
  Sp
- B.
  
  Sp²
- C.
  
  Sp²d²
- D.
  
  Sp³d³
Correct Answer
C. Sp²d²
5.

How many nuclear reactions are there?
- A.
  
  5
- B.
  
  4
- C.
  
  7
- D.
  
  3
Correct Answer
B. 4
6.

What is the bond axis?
- A.
  
  The line joining two neclei
- B.
  
  The bond coordination
- C.
  
  The joining planeg
- D.
  
  The imaginary line joining two nuclei
Correct Answer
D. The imaginary line joining two nuclei

Explanation
The bond axis refers to the imaginary line that connects the two nuclei in a molecule. This axis represents the direction along which the atoms are bonded together. It helps to define the orientation and geometry of the molecule, as well as the arrangement of the atoms around the bond axis.

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2
0
7.

Chemical bonds where two lobes of an orbital on one atom overlap two lobes of an orbital on another atom laterally are called what?
- A.
  
  Sigma bond
- B.
  
  Hybrid bond
- C.
  
  Sonsodial bond
- D.
  
  Pi-bond
Correct Answer
D. Pi-bond

Explanation
Pi-bonds are chemical bonds where two lobes of an orbital on one atom overlap two lobes of an orbital on another atom laterally. This type of bond is formed by the sideways overlap of p orbitals, resulting in the formation of a bond with electron density above and below the plane of the atoms. Pi-bonds are commonly found in double and triple bonds and are weaker than sigma bonds. They play a crucial role in the formation of organic molecules and are important for the stability and reactivity of compounds.

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8.

Which of the following is the strongest covalent chemical bond?
- A.
  
  Pi bond
- B.
  
  Bent bond
- C.
  
  Sigma bond
- D.
  
  Metal-to-metal bonding
Correct Answer
C. Sigma bond

Explanation
A sigma bond is the strongest covalent chemical bond. It is formed by the overlap of atomic orbitals along the axis between the two bonding atoms. This overlap allows for maximum electron density between the atoms, resulting in a strong bond. In contrast, a pi bond is formed by the sideways overlap of atomic orbitals, which is weaker than the head-on overlap of a sigma bond. Bent bonds and metal-to-metal bonding are not covalent bonds and are not as strong as sigma bonds.

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2
0
9.

How many valence electrons does oxygen have?
- A.
  
  8
- B.
  
  4
- C.
  
  6
- D.
  
  9
Correct Answer
C. 6

Explanation
Oxygen has 6 valence electrons. Valence electrons are the electrons in the outermost energy level of an atom, and they determine the atom's chemical properties. Oxygen is in group 16 of the periodic table, which means it has 6 valence electrons.

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0
10.

Why is H2O molecule polar?
- A.
  
  Because of the straight shape of the molecule
- B.
  
  Because of the bent shape of the molecule
- C.
  
  Because of the curved shape of the molecule
- D.
  
  Because of the round shape of the molecule
Correct Answer
B. Because of the bent shape of the molecule

Explanation
The correct answer is "Because of the bent shape of the molecule." This is because the water molecule (H2O) has a bent or V-shaped structure due to the two lone pairs of electrons on the oxygen atom. This arrangement causes an uneven distribution of charge, with the oxygen atom being slightly negatively charged and the hydrogen atoms being slightly positively charged. As a result, the bond between the oxygen and hydrogen atoms is polar, meaning there is an unequal sharing of electrons.

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