q2 chemistry: u4l10 covalent lewis dot diagrams day 1 date:
9. which groups/elements cannot form more than one bond (a single bond) in a covalent compound? why?

10. **of single, double, and triple bonds, which are the:
a. shortest?
b. longest?
c. strongest?
d. require least e to break?
e. consists of 6 shared e-?
f. consists of 4 shared e-?
11. **explain the differences between ionic and covalent compounds including the following vocabulary:
electrons, electrostatic force, electronegativity, types of elements.

(teacher use):
☑ ionic bonding
definition (includ how electron move electroneg differences,
and types of elements)
☑ covalent bonding
definition (includes
how electron moves,
electroneg differences,
and types of elements)
☑ vocabulary
out of 5

re-submit grades for question 11 (for teacher use only):
☑ ionic bonding definition (includes how electron moves, electroneg
differences, and types of elements)
☑ covalent bonding definition (includes how electron moves, electroneg
differences, and types of elements)
☑ vocabulary
out of 5

Question

q2 chemistry: u4l10 covalent lewis dot diagrams day 1  date:
9. which groups/elements cannot form more than one bond (a single bond) in a covalent compound? why?

10. **of single, double, and triple bonds, which are the:
    a. shortest?
    b. longest?
    c. strongest?
    d. require least e to break?
    e. consists of 6 shared e-?
    f. consists of 4 shared e-?
11. **explain the differences between ionic and covalent compounds including the following vocabulary:
    electrons, electrostatic force, electronegativity, types of elements.

(teacher use):
☑ ionic bonding
definition (includ how electron move electroneg differences,
and types of elements)
☑ covalent bonding
definition (includes
how electron moves,
electroneg differences,
and types of elements)
☑ vocabulary
 out of 5

re-submit grades for question 11 (for teacher use only):
☑ ionic bonding definition (includes how electron moves, electroneg
differences, and types of elements)
☑ covalent bonding definition (includes how electron moves, electroneg
differences, and types of elements)
☑ vocabulary
 out of 5

Accepted Answer

### Question 9 # Brief Explanations: Elements in Group 17 (halogens, like F, Cl, Br, I) and Group 1 (alkali metals, but in covalent compounds, H is key here) – specifically, hydrogen (H) and halogens (Group 17) usually form single bonds. Hydrogen has 1 valence electron, needs 1 more to fill its shell (duet rule). Halogens have 7 valence electrons, need 1 more to fill their octet. So they can only form one bond (share one electron pair) to achieve stability. # Answer: Group 1 (Hydrogen) and Group 17 (Halogens, e.g., F, Cl, Br, I) cannot form more than one bond (single bond) in covalent compounds. Because H needs 1 electron to complete its duet, and halogens need 1 electron to complete their octet, so they only share one pair of electrons (form one bond). ### Question 10 #### Part a # Brief Explanations: Triple bonds have the most shared electron pairs (3 pairs), so the nuclei of bonded atoms are pulled closer together, making the bond length shortest. # Answer: Triple bonds #### Part b # Brief Explanations: Single bonds have only 1 pair of shared electrons, so the attraction between nuclei is the weakest, leading to the longest bond length. # Answer: Single bonds #### Part c # Brief Explanations: Triple bonds have more shared electron pairs (3 pairs), so more energy is required to break them, making them the strongest. # Answer: Triple bonds #### Part d # Brief Explanations: Single bonds have the fewest shared electron pairs (1 pair), so the least energy is needed to break them. # Answer: Single bonds #### Part e # Brief Explanations: A triple bond consists of 3 pairs of electrons, which is 6 shared electrons (3 × 2 = 6). # Answer: Triple bonds #### Part f # Brief Explanations: A double bond consists of 2 pairs of electrons, which is 4 shared electrons (2 × 2 = 4). # Answer: Double bonds ### Question 11 # Brief Explanations: - **Electrons**: In ionic compounds, electrons are transferred from a metal (low electronegativity) to a non - metal (high electronegativity). In covalent compounds, electrons are shared between non - metals (or non - metal and metalloid) with similar electronegativities. - **Electrostatic Force**: Ionic compounds are held together by electrostatic forces between oppositely charged ions (cations and anions). Covalent compounds are held together by the electrostatic attraction between shared electrons and the nuclei of bonded atoms. - **Electronegativity**: Ionic compounds form between elements with a large electronegativity difference (usually metal - non - metal, electronegativity difference > 1.7). Covalent compounds form between elements with a small electronegativity difference (non - metal - non - metal or non - metal - metalloid, electronegativity difference < 1.7, or even 0 for non - polar covalent). - **Types of Elements**: Ionic compounds typically form between metals (left of the staircase on the periodic table) and non - metals (right of the staircase). Covalent compounds typically form between non - metals (and sometimes metalloids). # Answer: - **Ionic Compounds**: Form from metal - non - metal combinations. Electrons are transferred from metal (low electronegativity) to non - metal (high electronegativity) due to a large electronegativity difference (> 1.7). Held together by electrostatic forces between cations and anions. - **Covalent Compounds**: Form from non - metal - non - metal (or non - metal - metalloid) combinations. Electrons are shared between atoms with small electronegativity differences (< 1.7). Held together by the attraction between shared electrons and atomic nuclei.

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Question 9

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Question 10

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