32. state the filling rule for each:
a) an orbital may be occupied by only two electrons
b) electrons in the same orbital must have opposite spin
c) one electrons per sub orbital than double up
d) electrons occupy the lowest energy orbital available
33. the formula used to calculate the maximum number of electrons per level is
34. what is the maximum number of electrons that can occupy a) the third level
b) the fifth level c) the sixth level
35. how many electrons exist is each sublevel ?
a) s
b) p c) d d) f
36. what are electrons in the outermost energy level called?
37. how many electrons are in each of the following outermost energy level?
a) mg b) f c) k d) ar e) o

Question

32. state the filling rule for each:
a) an orbital may be occupied by only two electrons
b) electrons in the same orbital must have opposite spin
c) one electrons per sub orbital than double up
d) electrons occupy the lowest energy orbital available
33. the formula used to calculate the maximum number of electrons per level is
34. what is the maximum number of electrons that can occupy  a) the third level
b) the fifth level  c) the sixth level
35. how many electrons exist is each sublevel ?
a) s
b) p  c) d  d) f
36. what are electrons in the outermost energy level called?
37. how many electrons are in each of the following outermost energy level?
a) mg  b) f  c) k  d) ar  e) o

Accepted Answer

### Question 32:
#### Part (a)
# Brief Explanations:
The rule that an orbital may be occupied by only two electrons is the **Pauli Exclusion Principle** (in a more basic description for filling rules, this is part of the Pauli principle's application to electron occupancy in orbitals).
# Answer:
Pauli Exclusion Principle (basic: orbital holds 2 e⁻)

#### Part (b)
# Brief Explanations:
Electrons in the same orbital having opposite spins is also part of the **Pauli Exclusion Principle** (spin - pairing requirement for electrons in the same orbital).
# Answer:
Pauli Exclusion Principle (spin - opposite in orbital)

#### Part (c)
# Brief Explanations:
The rule of one electron per sub - orbital before doubling up is **Hund's Rule** (electrons fill degenerate orbitals singly first with parallel spins, then pair up).
# Answer:
Hund's Rule

#### Part (d)
# Brief Explanations:
Electrons occupying the lowest energy orbital available is the **Aufbau Principle** (building - up principle for electron configuration, filling from lowest energy to highest).
# Answer:
Aufbau Principle

### Question 33:
# Brief Explanations:
The formula to calculate the maximum number of electrons per energy level (n) is $2n^{2}$, where n is the principal quantum number (energy level).
# Answer:
$2n^{2}$

### Question 34:
#### Part (a) (Third level, n = 3)
# Explanation:
## Step 1: Identify the formula
We use the formula for maximum electrons per level: $N = 2n^{2}$, where n = 3 (third level).
## Step 2: Substitute n = 3 into the formula
$N=2	imes(3)^{2}=2	imes9 = 18$
# Answer:
18

#### Part (b) (Fifth level, n = 5)
# Explanation:
## Step 1: Recall the formula
The formula is $N = 2n^{2}$, with n = 5 (fifth level).
## Step 2: Calculate
$N = 2	imes(5)^{2}=2	imes25=50$
# Answer:
50

#### Part (c) (Sixth level, n = 6)
# Explanation:
## Step 1: Use the formula
The formula for maximum electrons per level is $N = 2n^{2}$, n = 6 (sixth level).
## Step 2: Compute
$N=2	imes(6)^{2}=2	imes36 = 72$
# Answer:
72

### Question 35:
#### Part (a) (s sublevel)
# Brief Explanations:
The s sublevel has 1 orbital, and since each orbital can hold a maximum of 2 electrons, the s sublevel can hold 2 electrons.
# Answer:
2

#### Part (b) (p sublevel)
# Brief Explanations:
The p sublevel has 3 degenerate orbitals. Since each orbital holds 2 electrons, the number of electrons in p sublevel is $3	imes2 = 6$.
# Answer:
6

#### Part (c) (d sublevel)
# Brief Explanations:
The d sublevel has 5 degenerate orbitals. With 2 electrons per orbital, the number of electrons in d sublevel is $5	imes2=10$.
# Answer:
10

#### Part (d) (f sublevel)
# Brief Explanations:
The f sublevel has 7 degenerate orbitals. Since each orbital holds 2 electrons, the number of electrons in f sublevel is $7	imes2 = 14$.
# Answer:
14

### Question 36:
# Brief Explanations:
Electrons in the outermost energy level of an atom are called **valence electrons** (they are involved in chemical bonding and determine the chemical properties of the atom).
# Answer:
Valence electrons

### Question 37:
#### Part (a) (Mg)
# Explanation:
## Step 1: Determine the electron configuration of Mg
Magnesium (Mg) has an atomic number of 12. Its electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}$.
## Step 2: Identify the outermost energy level
The outermost energy level is n = 3. The number of electrons in the outermost level (3s²) is 2.
# Answer:
2

#### Part (b) (F)
# Explanation:
## Step 1: Find the electron configuration of F
Fluorine (F) has an atomic number of 9. Its electron configuration is $1s^{2}2s^{2}2p^{5}$.
## Step 2: Determine the outermost electrons
The outermost energy level is n = 2. The number of electrons in the outermost level (2s²2p⁵) is 7.
# Answer:
7

#### Part (c) (K)
# Explanation:
## Step 1: Write the electron configuration of K
Potassium (K) has an atomic number of 19. Its electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}$.
## Step 2: Find the outermost electrons
The outermost energy level is n = 4. The number of electrons in the outermost level (4s¹) is 1.
# Answer:
1

#### Part (d) (Ar)
# Explanation:
## Step 1: Get the electron configuration of Ar
Argon (Ar) has an atomic number of 18. Its electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$.
## Step 2: Determine the outermost electrons
The outermost energy level is n = 3. The number of electrons in the outermost level (3s²3p⁶) is 8.
# Answer:
8

#### Part (e) (O)
# Explanation:
## Step 1: Determine the electron configuration of O
Oxygen (O) has an atomic number of 8. Its electron configuration is $1s^{2}2s^{2}2p^{4}$.
## Step 2: Find the outermost electrons
The outermost energy level is n = 2. The number of electrons in the outermost level (2s²2p⁴) is 6.
# Answer:
6

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QUESTION IMAGE

Question

Explanation:

Question 32:

Part (a)

Answer:

Part (b)