1. define polar covalent bond.
2. define non - polar covalent bond.
3. define electronegativity.
4. polar bonds occur between
5. non - polar bonds occur between
determine whether the following molecules are polar or nonpolar.
6. n₂
7. h₂o
8. co₂
9. nh₃
10. ch₄
11. so₃
12. hf
13. ch₃oh
14. h₂s
15. i₂
16. chcl₃
17. o₂

Question

Accepted Answer

### Question 1: Define polar covalent bond
# Brief Explanations:
A polar covalent bond is a type of covalent bond where the electrons are shared unequally between two atoms. This unequal sharing occurs because the atoms have different electronegativities, leading to a partial positive charge on one atom and a partial negative charge on the other.
# Answer:
A covalent bond where electrons are shared unequally between atoms (due to different electronegativities), creating partial charges (δ⁺ and δ⁻) on the atoms.

### Question 2: Define non - polar covalent bond
# Brief Explanations:
A non - polar covalent bond is a covalent bond in which the electrons are shared equally between two atoms. This happens when the two atoms involved in the bond have the same (or very similar) electronegativities, so there is no separation of charge across the bond.
# Answer:
A covalent bond where electrons are shared equally between atoms (same or similar electronegativities), with no partial charges.

### Question 3: Define electronegativity
# Brief Explanations:
Electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons (or electron density) towards itself when it is part of a chemical bond. It helps in determining the nature of the bond (polar or non - polar) between atoms.
# Answer:
The tendency of an atom to attract shared electrons in a chemical bond towards itself.

### Question 4: Polar bonds occur between
# Brief Explanations:
Polar bonds occur between two atoms that have different electronegativities. The atom with the higher electronegativity will attract the shared electrons more strongly, resulting in a partial negative charge on that atom and a partial positive charge on the less electronegative atom. Typically, polar bonds form between atoms of different non - metal elements (or between a metal and a non - metal in some cases, but more commonly between non - metals with different electronegativities).
# Answer:
Atoms with different electronegativities (usually different non - metal atoms or a metal and a non - metal atom).

### Question 5: Non - polar bonds occur between
# Brief Explanations:
Non - polar bonds occur between atoms that have the same (or very similar) electronegativities. Since the electronegativities are the same, the shared electrons are distributed equally between the two atoms, and there is no separation of charge. This is commonly seen in diatomic molecules made up of the same element, like $N_2$, $O_2$, etc., or between atoms of elements with very similar electronegativities.
# Answer:
Atoms with the same (or very similar) electronegativities (e.g., in diatomic molecules of the same element like $N_2$, $O_2$).

### Question 6: Determine if $N_2$ is polar or non - polar
# Brief Explanations:
$N_2$ is a diatomic molecule composed of two nitrogen atoms. The two nitrogen atoms have the same electronegativity. In the covalent bond between them, the electrons are shared equally. Also, the molecular geometry of $N_2$ is linear. Since there is no separation of charge (no dipole moment) and the bond is non - polar, the molecule is non - polar.
# Answer:
Non - polar

### Question 7: Determine if $H_2O$ is polar or non - polar
# Brief Explanations:
In $H_2O$, the oxygen atom is more electronegative than the hydrogen atoms. The $O - H$ bonds are polar covalent bonds. The molecular geometry of $H_2O$ is bent (angular) with a bond angle of approximately $104.5^{\circ}$. The polar bonds do not cancel each other out, and there is a net dipole moment in the molecule. So, $H_2O$ is a polar molecule.
# Answer:
Polar

### Question 8: Determine if $CO_2$ is polar or non - polar
# Brief Explanations:
In $CO_2$, the $C = O$ bonds are polar covalent bonds because oxygen is more electronegative than carbon. However, the molecular geometry of $CO_2$ is linear, with the two $C = O$ bonds arranged in a straight line (180° apart) from the carbon atom. The dipole moments of the two $C = O$ bonds are equal in magnitude but opposite in direction, so they cancel each other out. Thus, $CO_2$ is a non - polar molecule.
# Answer:
Non - polar

### Question 9: Determine if $NH_3$ is polar or non - polar
# Brief Explanations:
In $NH_3$, the $N - H$ bonds are polar covalent bonds as nitrogen is more electronegative than hydrogen. The molecular geometry of $NH_3$ is trigonal pyramidal. The three $N - H$ bond dipoles do not cancel each other out, and there is a net dipole moment in the molecule (pointing towards the nitrogen atom). So, $NH_3$ is a polar molecule.
# Answer:
Polar

### Question 10: Determine if $CH_4$ is polar or non - polar
# Brief Explanations:
In $CH_4$, the $C - H$ bonds are considered to be non - polar (or very slightly polar) because the electronegativity difference between carbon and hydrogen is small. The molecular geometry of $CH_4$ is tetrahedral, with the four $C - H$ bonds symmetrically arranged around the carbon atom. The bond dipoles (if any) cancel each other out, resulting in a net dipole moment of zero. So, $CH_4$ is a non - polar molecule.
# Answer:
Non - polar

### Question 11: Determine if $SO_3$ is polar or non - polar
# Brief Explanations:
In $SO_3$, the $S = O$ bonds are polar covalent bonds. The molecular geometry of $SO_3$ is trigonal planar, with the three $S = O$ bonds arranged symmetrically around the sulfur atom (bond angles of 120°). The dipole moments of the three $S = O$ bonds cancel each other out, so there is no net dipole moment. Thus, $SO_3$ is a non - polar molecule.
# Answer:
Non - polar

### Question 12: Determine if $HF$ is polar or non - polar
# Brief Explanations:
In $HF$, fluorine is much more electronegative than hydrogen. The $H - F$ bond is a polar covalent bond, and since there is only one bond in the $HF$ molecule, there is a net dipole moment (with the fluorine atom having a partial negative charge and the hydrogen atom having a partial positive charge). So, $HF$ is a polar molecule.
# Answer:
Polar

### Question 13: Determine if $CH_3OH$ (methanol) is polar or non - polar
# Brief Explanations:
Methanol ($CH_3OH$) has a polar $O - H$ bond and also has a polar $C - O$ bond. The molecule has a tetrahedral arrangement around the carbon and a bent arrangement around the oxygen (due to the two lone pairs on oxygen). The polar bonds do not cancel each other out, and there is a net dipole moment in the molecule (with the oxygen atom being partially negative and the hydrogen atom in the $O - H$ bond being partially positive). So, $CH_3OH$ is a polar molecule.
# Answer:
Polar

### Question 14: Determine if $H_2S$ is polar or non - polar
# Brief Explanations:
In $H_2S$, the $S - H$ bonds are polar covalent bonds because sulfur is more electronegative than hydrogen. The molecular geometry of $H_2S$ is bent (similar to $H_2O$ but with a larger bond angle). The two $S - H$ bond dipoles do not cancel each other out, resulting in a net dipole moment. So, $H_2S$ is a polar molecule.
# Answer:
Polar

### Question 15: Determine if $I_2$ is polar or non - polar
# Brief Explanations:
$I_2$ is a diatomic molecule composed of two iodine atoms. The two iodine atoms have the same electronegativity, so the electrons in the covalent bond are shared equally. There is no separation of charge, and the molecular geometry is linear (for a diatomic molecule). Thus, $I_2$ is a non - polar molecule.
# Answer:
Non - polar

### Question 16: Determine if $CHCl_3$ (chloroform) is polar or non - polar
# Brief Explanations:
In $CHCl_3$, the $C - Cl$ bonds are polar (chlorine is more electronegative than carbon) and the $C - H$ bond is relatively non - polar. The molecular geometry of $CHCl_3$ is tetrahedral, but the four bonds ($3$ $C - Cl$ and $1$ $C - H$) are not symmetrically arranged in terms of electronegativity. The dipole moments of the $C - Cl$ bonds do not cancel out the (small) dipole moment of the $C - H$ bond, resulting in a net dipole moment. So, $CHCl_3$ is a polar molecule.
# Answer:
Polar

### Question 17: Determine if $O_2$ is polar or non - polar
# Brief Explanations:
$O_2$ is a diatomic molecule made up of two oxygen atoms. The two oxygen atoms have the same electronegativity, so the electrons in the covalent bond are shared equally. There is no separation of charge, and the molecular geometry is linear. Therefore, $O_2$ is a non - polar molecule.
# Answer:
Non - polar

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Question 1: Define polar covalent bond

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Question 2: Define non - polar covalent bond