2 types of bonds (continued)
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8. compare and contrast ionic and covalent bonds.
9. determine the type of bonding in cao and in so₂.
10. name the type of particle formed by covalent bonds.
11. identify the following substances as having polar or nonpolar molecules: hbr, cl₂, and h₂o.
12. predict from the given symbols, choose two elements that are likely to form an ionic bond: o, ne, s, ca, and k. next, select two elements that would likely form a covalent bond. explain your predictions.
13. math connection aluminum oxide (al₂o₃) can be produced during rocket launches. show that the sum of the positive and negative charges in a unit of al₂o₃ equals zero.

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Accepted Answer

### Question 8
# Brief Explanations:
Ionic bonds form between a metal and a non - metal through the transfer of electrons, resulting in the formation of ions (cations and anions) that are held together by electrostatic attraction. Covalent bonds form between non - metals (or sometimes a metal and a non - metal with low electronegativity difference) through the sharing of electron pairs. Both types of bonds are used to achieve a stable electron configuration (usually a full outer shell, like the noble gas configuration) for the atoms involved. The main differences are in the nature of electron transfer (ionic: transfer; covalent: sharing), the types of atoms involved (ionic: metal - non - metal; covalent: non - metal - non - metal or less electronegativity difference cases), and the physical properties of the compounds formed (ionic compounds often have high melting/boiling points, are brittle, and conduct electricity when molten or in solution; covalent compounds can be gases, liquids, or solids with lower melting/boiling points, and many do not conduct electricity).
# Answer:
Ionic bonds involve the transfer of electrons from a metal to a non - metal, forming ions (cations and anions) held by electrostatic forces. Covalent bonds involve non - metals sharing electron pairs. Both aim for stable electron configurations, but differ in electron behavior, atom types, and compound properties.

### Question 9
# Brief Explanations:
For $CaO$: Calcium ($Ca$) is a metal (alkaline earth metal) and oxygen ($O$) is a non - metal. Metals tend to lose electrons and non - metals tend to gain electrons. Calcium will lose 2 electrons to form $Ca^{2+}$ and oxygen will gain 2 electrons to form $O^{2 -}$. The electrostatic attraction between these oppositely charged ions forms an ionic bond. For $SO_2$: Sulfur ($S$) and oxygen ($O$) are both non - metals. They will share electron pairs to achieve stable electron configurations. The bond formed by the sharing of electrons between non - metals is a covalent bond.
# Answer:
In $CaO$, the bonding is ionic (between metal $Ca$ and non - metal $O$ via electron transfer). In $SO_2$, the bonding is covalent (between non - metals $S$ and $O$ via electron sharing).

### Question 10
# Brief Explanations:
Covalent bonds are formed when atoms share electron pairs. The particle formed by covalent bonds is a molecule. In a covalent bond, two or more atoms are held together by the shared electrons, and this group of atoms is called a molecule. For example, in $H_2O$, two hydrogen atoms and one oxygen atom are held together by covalent bonds to form a water molecule.
# Answer:
The type of particle formed by covalent bonds is a molecule.

### Question 11
# Brief Explanations:
- $HBr$: Hydrogen ($H$) and bromine ($Br$) are non - metals. The electronegativity of $Br$ is greater than that of $H$, so the electron pair in the $H - Br$ bond is pulled more towards $Br$. This creates a dipole moment (a separation of positive and negative charges) in the molecule, so $HBr$ has polar molecules.
- $Cl_2$: The two chlorine atoms in $Cl_2$ have the same electronegativity. The electron pair in the $Cl - Cl$ bond is shared equally between the two atoms. There is no dipole moment, so $Cl_2$ has non - polar molecules.
- $H_2O$: The electronegativity of oxygen is greater than that of hydrogen. The two $O - H$ bonds are polar, and the bent molecular geometry of $H_2O$ (due to the two lone pairs on oxygen) results in a net dipole moment for the molecule. So $H_2O$ has polar molecules.
# Answer:
$HBr$: polar; $Cl_2$: non - polar; $H_2O$: polar.

### Question 12
# Brief Explanations:
- Ionic bond prediction: Ionic bonds form between a metal and a non - metal. Among the given elements, $Ca$ (calcium, a metal) and $O$ (oxygen, a non - metal), or $K$ (potassium, a metal) and $O$ (oxygen, a non - metal), or $Ca$ and $S$ (sulfur, a non - metal), or $K$ and $S$ can form ionic bonds. For example, $Ca$ and $O$: $Ca$ will lose 2 electrons to form $Ca^{2+}$ and $O$ will gain 2 electrons to form $O^{2 -}$, and the electrostatic attraction between them forms an ionic bond. $K$ and $O$: $K$ loses 1 electron to form $K^+$ and $O$ gains 2 electrons to form $O^{2 -}$ (in a compound like $K_2O$).
- Covalent bond prediction: Covalent bonds form between non - metals. Among the given elements, $O$ (oxygen), $S$ (sulfur) are non - metals. $O$ and $S$ can form a covalent bond. They will share electron pairs to achieve stable electron configurations. Neon ($Ne$) is a noble gas with a stable electron configuration and does not form bonds easily.
# Answer:
- Ionic bond: For example, $Ca$ and $O$ (or $K$ and $O$, $Ca$ and $S$, $K$ and $S$). Explanation: Ionic bonds form between metals ( $Ca$, $K$) and non - metals ( $O$, $S$) via electron transfer.
- Covalent bond: $O$ and $S$. Explanation: Covalent bonds form between non - metals ( $O$, $S$) via electron sharing. $Ne$ is inert.

### Question 13
# Explanation:
## Step1: Determine the charges of ions
Aluminum ($Al$) in $Al_2O_3$ forms $Al^{3+}$ ions (since aluminum generally loses 3 electrons to achieve a stable electron configuration). Oxygen ($O$) forms $O^{2 -}$ ions (since oxygen generally gains 2 electrons to achieve a stable electron configuration).
## Step2: Calculate the total positive and negative charges
In one unit of $Al_2O_3$, there are 2 $Al^{3+}$ ions and 3 $O^{2 -}$ ions.
The total positive charge from $Al^{3+}$ ions is $2\times( + 3)=+6$.
The total negative charge from $O^{2 -}$ ions is $3\times( - 2)=-6$.
## Step3: Sum the charges
The sum of the positive and negative charges is $( + 6)+( - 6)=0$.
# Answer:
The sum of positive ($2\times( + 3)=+6$) and negative ($3\times( - 2)=-6$) charges in $Al_2O_3$ is $+6+( - 6) = 0$.

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