The valence electrons in an atom are the electrons in the

ANSWER : The valence electrons in an atom are the electrons in the outer most principal shel

Lewis structures use Lewis symbols to show valence electrons of main-group elements as

ANSWER : Lewis structures use Lewis symbols to show valence electrons of main-group elements as dots 

surrounding the symbol of the atom.

Ionic bonds are formed by transfer of

ANSWER : Ionic bonds are formed by transfer of electrons from a metal to a non-metal. Therefore, the 

Lewis structure for these compounds is drawn by moving the electrons from metal to non-metal.

Covalent compounds are formed by

ANSWER : Covalent compounds are formed by sharing electrons. Therefore, the Lewis structures for 

these compounds are drawn by allowing neighboring atoms to share some of their valence electrons.

Ionic bonds are formed by transfer of electrons from a metal to a non-metal. Therefore, the Lewis structure for these compounds is drawn by

ANSWER : Ionic bonds are formed by transfer of electrons from a metal to a non-metal. Therefore, the 

Lewis structure for these compounds is drawn by moving the electrons from metal to non-metal.

Covalent compounds are formed by sharing electrons. Therefore, the Lewis structures for these 

compounds are drawn by

ANSWER : Covalent compounds are formed by sharing electrons. Therefore, the Lewis structures for 

these compounds are drawn by allowing neighboring atoms to share some of their valence electrons.

The electrons that are shared between the atoms are called

ANSWER : The electrons that are shared between the atoms are called bonding pair electrons, while 

those that are only on one atom are called lone pair electrons.

The electrons that are shared between the atoms are called bonding pair electrons, while those that are 

only on one atom are

ANSWER : The electrons that are shared between the atoms are called bonding pair electrons, while 

those that are only on one atom are called lone pair electrons.

The bonding pair electrons can often represented as dash lines, to emphasize that they are

ANSWER : The bonding pair electrons can often represented as dash lines, to emphasize that they are 

chemical bonds, but the lone pair electrons are always displayed as dots.

The bonding pair electrons can often represented as dash lines, to emphasize that they are chemical 

bonds, but the lone pair electrons are always displayed as

ANSWER : The bonding pair electrons can often represented as dash lines, to emphasize that they are 

chemical bonds, but the lone pair electrons are always displayed as dots.

The Lewis model also explains why halogens are

ANSWER : The Lewis model also explains why halogens are diatomic.

The Lewis model also allows atoms to share more than one pair of electrons to achieve

ANSWER : The Lewis model also allows atoms to share more than one pair of electrons to achieve octet.

When writing Lewis structures, it might be possible to write more than one good (valid) structure

ANSWER : When writing Lewis structures, it might be possible to write more than one good (valid) 

structure for some molecules.

equivalent structures are called

ANSWER : equivalent structures are called resonance structures

The Lewis structure of a molecule, in combination with valence shell electron pair repulsion (VSEPR) theory, can be used to

ANSWER : The Lewis structure of a molecule, in combination with valence shell electron pair repulsion 

(VSEPR) theory, can be used to predict the shape of a molecule.

The VSEPR theory is based on the idea that

ANSWER : The VSEPR theory is based on the idea that electron groups around the central atom of a 

molecule repel each other. The repulsion between these electron groups determine the shape of the 

molecule.

Electron groups are defined as:

ANSWER : Electron groups are defined as: lone pairs, single bonds or multiple bonds.

the shape produced by the electrons is called

ANSWER : the shape produced by the electrons is called electron geometry.

When one of more lone pairs are around the central atom, the shape of the molecule as it appears to us 

is different than the electron geometry, and is referred to as

ANSWER : When one of more lone pairs are around the central atom, the shape of the molecule as it 

appears to us is different than the electron geometry, and is referred to as molecular geometry.

The ability of an element to attract electrons within a covalent molecule is called

ANSWER : The ability of an element to attract electrons within a covalent molecule is called 

electronegativity.

The result of this uneven sharing of electrons in the O-H bond is the separation of charge in the bond, 

called

ANSWER : oxygen is more electronegative than hydrogen. This means that on the average, the shared 

electrons are more likely to be found near the oxygen atom than near the hydrogen atom.

Covanlent bonds that have dipole moment are called

ANSWER : Covanlent bonds that have dipole moment are called polar covalent bonds.

The dipole moment in a bond is sometimes shown with a vector representation, where the

ANSWER : The dipole moment in a bond is sometimes shown with a vector representation, where the 

vector points to the direction of the atom with the partial negative charge.

The magnitude of the dipole moment, and therefore the degree of polarity of the bond, depend on the

ANSWER : The magnitude of the dipole moment, and therefore the degree of polarity of the bond, 

depend on the difference in electronegativity between the two elements forming the bond and the bond 

length.

For a fixed bond length, the greater the electronegativity difference, the greater the

ANSWER : For a fixed bond length, the greater the electronegativity difference, the greater the dipole 

moment and the more polar the bond.

Note that electronegativity increases across a period and decreases

ANSWER : Note that electronegativity increases across a period and decreases down a group.

If two elements with nearly identical electronegativities form a covalent bond, they share the electron 

equally, and there is little or no dipole moment. These bonds are called

ANSWER : If two elements with nearly identical electronegativities form a covalent bond, they share the 

electron equally, and there is little or no dipole moment. These bonds are called non-polar covalent 

bonds.

When two elements with intermediate electronegativity difference form a bond, such as two nonmetals, 

the electrons are shared unequally and there is an intermediate dipole moment. These bonds are called

ANSWER : When two elements with intermediate electronegativity difference form a bond, such as two 

nonmetals, the electrons are shared unequally and there is an intermediate dipole moment. These 

bonds are called polar covalent. H and F form such a bond.

If there is a large electronegativity difference between two elements forming a bond, such as a metal 

and nonmetal, the electron is transferred and a there is a large dipole moment. These bonds are called

ANSWER : If there is a large electronegativity difference between two elements forming a bond, such as 

a metal and nonmetal, the electron is transferred and a there is a large dipole moment. These bonds are 

called ionic. Sodium and chlorine form such a bond.

Many molecules with polar bonds become non-polar, because their bond polarities cancel out one 

another due to

ANSWER : Many molecules with polar bonds become non-polar, because their bond polarities cancel out 

one another due to their shapes.

For diatomic molecules, the polarity of the molecule can easily be determined from the

ANSWER : For diatomic molecules, the polarity of the molecule can easily be determined from the 

polarity of the bond, since the bond forms the molecule. Therefore, diatomic molecules with non-polar 

bonds are non-polar, and those with polar bonds are polar.

For molecules with more than two atoms, it is more difficult to distinguish between the polar and 

non-polar molecules, because two or more polar bonds may

ANSWER : For molecules with more than two atoms, it is more difficult to distinguish between the polar 

and non-polar molecules, because two or more polar bonds may cancel each other.

Water, on the other hand, also has two polar O-H bonds, since the electronegativity difference between 

hydrogen and oxygen is 1.24. However, the bent shape of the water molecule does not allow the two 

dipole moments of the bonds to cancel one another. As a result water is a

ANSWER : Water, on the other hand, also has two polar O-H bonds, since the electronegativity difference 

between hydrogen and oxygen is 1.24. However, the bent shape of the water molecule does not allow 

the two dipole moments of the bonds to cancel one another. As a result water is a polar molecule.

Molecules with symmetrical shapes such as linear, trigonal planar and tetrahedral, allow for cancellation 

of dipole moments and are non-polar when all atoms around the central atom are

ANSWER : Molecules with symmetrical shapes such as linear, trigonal planar and tetrahedral, allow for 

cancellation of dipole moments and are non-polar when all atoms around the central atom are the 

same.

Molecules with unsymmetrical shapes such as bent and pyramidal do not allow for cancellation of dipole 

moments are always

ANSWER : Molecules with unsymmetrical shapes such as bent and pyramidal do not allow for 

cancellation of dipole moments are always polar.

to determine if a molecule is polar: First determine whether the molecule contains polar bonds. A bond 

is polar if the two atoms forming the bond have different electronegativities. If no polar bonds exist, the 

molecule is

ANSWER : to determine if a molecule is polar: First determine whether the molecule contains polar 

bonds. A bond is polar if the two atoms forming the bond have different electronegativities. If no polar 

bonds exist, the molecule is non-polar.Next determine if the polarity of the bonds cancel one another 

because of the shape. Use VSEPR model to determine the shape of the molecule and then evaluate if the 

polarity of the bonds can be cancelled due to the shape.

to determine if a molecule is polar: First determine whether the molecule contains polar bonds. A bond 

is polar if the two atoms forming the bond have different electronegativities. If no polar bonds exist, the 

molecule is non-polar.Next determine if the polarity of the bonds cancel one another because of the 

shape. Use VSEPR model to determine the shape of the molecule and then evaluate if the

ANSWER : to determine if a molecule is polar: First determine whether the molecule contains polar 

bonds. A bond is polar if the two atoms forming the bond have different electronegativities. If no polar 

bonds exist, the molecule is non-polar.Next determine if the polarity of the bonds cancel one another because of the shape. Use VSEPR model to determine the shape of the molecule and then evaluate if the polarity of the bonds can be cancelled due to the shape.

1 What is the hybridization of a linear molecule?

• sp2

• Sp (CORRECT ANSWER)

• sp3d

• sp3

2. The hybridization of the carbon atom is?

• Sp2  (CORRECT ANSWER)

• sp3

• sp3d

• sp

3. What is the correct Lewis Dot Structure for ammonia NH3

4. Which of the following simple molecular substances does NOT obey the octet rule?

• SF6(CORRECT ANSWER)

• PF3

• CO2

• CH3Cl

5. What is the hybridization of the Carbon atom indicated by the arrow?

• sp2 hybridization(CORRECT ANSWER)

• dsp3 hybridization

• sp3 hybridization

6. Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?

• C

• D

• B(CORRECT ANSWER)

• A

7. Which of the following molecules does NOT have a linear shape?

• CS2

• HCN

• OF2(CORRECT ANSWER)

8. CO2 has how many lone pairs?

• 1

• 2

• 3

• 0(CORRECT ANSWER)

9. NH3 has how many lone pairs?

• 0

• 1(CORRECT ANSWER)

• 2

• 3

10. What is the hybridization of each Carbon atom in benzene (C6H6)?

• sp3d

• sp2(CORRECT ANSWER)

• sp3

11. CCl4 has how many double bonds?

• 0(CORRECT ANSWER)

• 1

• 2

• 3

12. Xe atom undergo

• sp3d hybridization(CORRECT ANSWER)

• sp2 hybridization

• sp3 hybridization

• sp hybridization

13. Carbonate (CO32-) has how many double bonds?

• 0

• 1(CORRECT ANSWER)

• 2

• 3

14. In which of the following pairs, do the molecules have a similar shape?

• BH3 and CH2O(CORRECT ANSWER)

• SCl2 and CO2

• BF3 and NH3

15. Which molecule will undergo sp3 hybridization of its central atom?

• NO2

• SO3

• NH3(CORRECT ANSWER)

• CO2

16. Which orbitals are responsible for forming pi bonds?

• sp

• s

• p(CORRECT ANSWER)

17. In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

• Double

• Single

• Triple(CORRECT ANSWER)

18. CHCl3 has how many double bonds?

• 0(CORRECT ANSWER)

• 1

• 2

• 3

19. What is the hybridization of the central atom of a bent molecule? (AB2E2)

• sp3d

• sp2

• sp3(CORRECT ANSWER)

20. What is the hybridization of the central atom in XeF6?

• sp

• sp3d3(CORRECT ANSWER)

• sp3d

21. According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?

• Electrons closest to the nucleus

• Mobile Electrons

• Pairs of valence electrons (CORRECT ANSWER)