13. what is the octet rule?
14. an__________is a particle with a charge formed by losing and/or gaining electrons.
15. what is a cation (and how is it created)? a positively charged ion ( al⁺³ )
16. what is an anion (and how is it created)?
a explain the difference between mg and mg⁺².
b. explain the difference between cl and cl⁻¹.
17. what type of ion (cation or anion) will each of the following forms?
a. aluminum
b. oxygen
18. examine the following electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁴
a. will atoms of this element most likely gain or lose electrons?
b. how many electrons will be gained or lost?
19. examine the following electron configuration- 1s² 2s² 2p⁶ 3s²
a. will atoms of this element most likely gain or lose electrons?
b. how many electrons will be gained or lost?
20. the electron configuration of cl⁻ ( chloride ion) is :
(hint: chloride ion has one more electron than chlorine atom)
21. the electron configuration of na⁺ ( sodium ion) is :
(hint: sodium ion has one less electron than sodium atom)
22. why do elements in the same family/group have similar chemical properties?
23. what do the elements in the same group/column have in common ?
24. what do the elements in the same period have in common ?

Question

13. what is the octet rule?
14. an__________is a particle with a charge formed by losing and/or gaining electrons.
15. what is a cation (and how is it created)?  a positively charged ion ( al⁺³ )
16. what is an anion (and how is it created)?
   a explain the difference between mg and mg⁺².
   b. explain the difference between cl and cl⁻¹.
17. what type of ion (cation or anion) will each of the following forms?
   a. aluminum
   b. oxygen
18. examine the following electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁴
   a. will atoms of this element most likely gain or lose electrons?
   b. how many electrons will be gained or lost?
19.  examine the following electron configuration- 1s² 2s² 2p⁶ 3s²
   a. will atoms of this element most likely gain or lose electrons?
   b. how many electrons will be gained or lost?
20. the electron configuration of cl⁻ ( chloride ion) is :
 (hint: chloride ion has one more electron than chlorine atom)
21. the electron configuration of  na⁺ ( sodium ion) is :
 (hint: sodium ion has one less electron than sodium atom)
22. why do elements in the same family/group have similar chemical properties?
23. what do the elements in the same group/column have in common ?
24. what do the elements in the same period have in common ?

Accepted Answer

### Question 13: What is the octet rule?
# Brief Explanations:
The octet rule is a chemical principle stating that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with 8 valence electrons (like noble gases, except H/He). This stability drives chemical bonding and reactivity.
# Answer:
The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with 8 valence electrons (to mimic the electron configuration of noble gases, which are generally stable).

### Question 14: An ______ is a particle with a charge formed by losing and/or gaining electrons.
# Brief Explanations:
Ions are charged particles. Cations (positive) form by losing electrons, anions (negative) by gaining electrons. The blank requires the term for such charged particles.
# Answer:
ion

### Question 15: What is a cation (and how is it created)?
# Brief Explanations:
A cation is a positively charged ion. It forms when an atom loses one or more electrons, resulting in more protons than electrons (e.g., $ \text{Al} $ loses 3 electrons to form $ \text{Al}^{3+} $).
# Answer:
A cation is a positively charged ion. It is created when an atom loses one or more electrons (since losing electrons leaves the atom with more protons than electrons, giving it a positive charge). For example, an aluminum atom ($ \text{Al} $) loses 3 electrons to form the aluminum cation $ \text{Al}^{3+} $.

### Question 16: What is an anion (and how is it created)?
a. Explain the difference between $ \text{Mg} $ and $ \text{Mg}^{2+} $.
b. Explain the difference between $ \text{Cl} $ and $ \text{Cl}^- $.

#### Part 16 (Anion Definition):
# Brief Explanations:
An anion is a negatively charged ion. It forms when an atom gains one or more electrons, resulting in more electrons than protons (e.g., $ \text{Cl} $ gains 1 electron to form $ \text{Cl}^- $).
# Answer:
An anion is a negatively charged ion. It is created when an atom gains one or more electrons (since gaining electrons leaves the atom with more electrons than protons, giving it a negative charge). For example, a chlorine atom ($ \text{Cl} $) gains 1 electron to form the chloride anion $ \text{Cl}^- $.

#### Part 16a (Mg vs $ \text{Mg}^{2+} $):
# Brief Explanations:
$ \text{Mg} $ is a neutral magnesium atom with 12 protons and 12 electrons. $ \text{Mg}^{2+} $ is a magnesium cation: it lost 2 electrons, so it has 12 protons and 10 electrons (positive charge, smaller radius, different reactivity).
# Answer:
- $ \text{Mg} $: Neutral magnesium atom with 12 protons and 12 electrons (no net charge, larger atomic radius, more reactive in losing electrons).
- $ \text{Mg}^{2+} $: Magnesium cation (positively charged) with 12 protons and 10 electrons (lost 2 electrons, smaller ionic radius, stable electron configuration like a noble gas).

#### Part 16b (Cl vs $ \text{Cl}^- $):
# Brief Explanations:
$ \text{Cl} $ is a neutral chlorine atom with 17 protons and 17 electrons. $ \text{Cl}^- $ is a chloride anion: it gained 1 electron, so it has 17 protons and 18 electrons (negative charge, larger radius, stable electron configuration).
# Answer:
- $ \text{Cl} $: Neutral chlorine atom with 17 protons and 17 electrons (no net charge, smaller atomic radius, more reactive in gaining electrons).
- $ \text{Cl}^- $: Chloride anion (negatively charged) with 17 protons and 18 electrons (gained 1 electron, larger ionic radius, stable electron configuration like a noble gas).

### Question 17: What type of ion (cation or anion) will each of the following form?
a. Aluminum
b. Oxygen

#### Part 17a (Aluminum):
# Brief Explanations:
Aluminum (Al) is a metal in Group 13. Metals tend to lose electrons to form cations. Al loses 3 electrons to form $ \text{Al}^{3+} $ (a cation).
# Answer:
cation (Aluminum loses 3 electrons to form $ \text{Al}^{3+} $, a positively charged ion).

#### Part 17b (Oxygen):
# Brief Explanations:
Oxygen (O) is a nonmetal in Group 16. Nonmetals tend to gain electrons to form anions. O gains 2 electrons to form $ \text{O}^{2-} $ (an anion).
# Answer:
anion (Oxygen gains 2 electrons to form $ \text{O}^{2-} $, a negatively charged ion).

### Question 18: Examine the electron configuration: $ 1s^2 2s^2 2p^6 3s^2 3p^4 $
a. Will atoms of this element most likely gain or lose electrons?
b. How many electrons will be gained or lost?

#### Part 18a:
# Brief Explanations:
The electron configuration $ 1s^2 2s^2 2p^6 3s^2 3p^4 $ has 6 valence electrons (in $ 3s^2 3p^4 $). Atoms with 5–7 valence electrons (nonmetals) tend to gain electrons to reach 8 (octet). So this element (sulfur, S) will gain electrons.
# Answer:
gain

#### Part 18b:
# Brief Explanations:
To reach 8 valence electrons (octet), an atom with 6 valence electrons needs to gain $ 8 - 6 = 2 $ electrons. Thus, it gains 2 electrons.
# Answer:
2 (gained)

### Question 19: Examine the electron configuration: $ 1s^2 2s^2 2p^6 3s^2 $
a. Will atoms of this element most likely gain or lose electrons?
b. How many electrons will be gained or lost?

#### Part 19a:
# Brief Explanations:
The electron configuration $ 1s^2 2s^2 2p^6 3s^2 $ has 2 valence electrons (in $ 3s^2 $). Atoms with 1–3 valence electrons (metals) tend to lose electrons to reach a stable octet (e.g., lose 2 electrons to mimic $ \text{Ne} $ or $ \text{Ar} $ configuration). So this element (magnesium, Mg) will lose electrons.
# Answer:
lose

#### Part 19b:
# Brief Explanations:
To reach a stable electron configuration (octet), an atom with 2 valence electrons (Group 2) loses 2 electrons (matches the $ \text{Mg}^{2+} $ formation: $ \text{Mg} $ loses 2 electrons to form $ \text{Mg}^{2+} $).
# Answer:
2 (lost)

### Question 20: Electron configuration of $ \text{Cl}^- $ (hint: 1 more electron than Cl atom)
# Brief Explanations:
Chlorine (Cl) has electron configuration $ 1s^2 2s^2 2p^6 3s^2 3p^5 $. $ \text{Cl}^- $ gains 1 electron, so add 1 to the $ 3p $ subshell: $ 1s^2 2s^2 2p^6 3s^2 3p^6 $ (or $ [\text{Ar}] $, since $ 1s^2 2s^2 2p^6 3s^2 3p^6 $ is argon’s configuration).
# Answer:
$ 1s^2 2s^2 2p^6 3s^2 3p^6 $ (or $ [\text{Ar}] $)

### Question 21: Electron configuration of $ \text{Na}^+ $ (hint: 1 less electron than Na atom)
# Brief Explanations:
Sodium (Na) has electron configuration $ 1s^2 2s^2 2p^6 3s^1 $. $ \text{Na}^+ $ loses 1 electron (from $ 3s^1 $), so the configuration becomes $ 1s^2 2s^2 2p^6 $ (or $ [\text{Ne}] $, since $ 1s^2 2s^2 2p^6 $ is neon’s configuration).
# Answer:
$ 1s^2 2s^2 2p^6 $ (or $ [\text{Ne}] $)

### Question 22: Why do elements in the same family/group have similar chemical properties?
# Brief Explanations:
Elements in the same group have the same number of valence electrons (e.g., Group 1 has 1 valence electron, Group 17 has 7). Valence electrons determine an atom’s reactivity (how it bonds/gains/loses electrons). Thus, similar valence electron counts lead to similar chemical properties.
# Answer:
Elements in the same family/group have the same number of valence electrons. Valence electrons determine an atom’s chemical reactivity (how it forms bonds, gains/loses electrons). Since elements in a group share the same number of valence electrons, they exhibit similar chemical properties.

### Question 23: What do elements in the same group/column have in common?
# Brief Explanations:
Elements in a group (column) have the same number of valence electrons (e.g., Group 1: 1 valence electron, Group 16: 6 valence electrons). This shared valence electron count leads to similar chemical properties (reactivity, bonding behavior). They also have similar electron configurations in their outermost (valence) shells.
# Answer:
Elements in the same group/column have the same number of valence electrons (e.g., Group 1 elements have 1 valence electron, Group 17 have 7). This causes them to have similar chemical properties (reactivity, bonding behavior) and similar electron configurations in their outermost (valence) electron shells.

### Question 24: What do elements in the same period have in common?
# Brief Explanations:
Elements in a period (row) have the same number of electron shells (energy levels). For example, Period 3 elements (Na, Mg, Al, ..., Ar) all have electrons in 3 energy levels ($ n = 3 $). While their valence electrons differ, the number of electron shells is constant across a period.
# Answer:
Elements in the same period (row) have the same number of electron shells (energy levels). For example, all elements in Period 3 (e.g., Na, Mg, S, Cl) have electrons in 3 energy levels ($ n = 3 $).

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Question 13: What is the octet rule?

Answer:

Question 14: An ______ is a particle with a charge formed by losing and/or gaining electrons.