5. use the periodic table to answer the following questions: t/i-6
for the element sulfur:
a) find the location of this element on the periodic table 1 marks
- group
- period
b) write the atomic notation 1 marks
c) draw the bohr-rutherford diagram 2 marks
d) draw the lewis dot diagram 1 marks
e) identify the charge of the ion 1 mark

Question

5. use the periodic table to answer the following questions: t/i-6
for the element sulfur:
  a) find the location of this element on the periodic table 1 marks
    - group
    - period
  b) write the atomic notation 1 marks
  c) draw the bohr-rutherford diagram 2 marks
  d) draw the lewis dot diagram 1 marks
  e) identify the charge of the ion 1 mark

Accepted Answer

### Part (a)
# Explanation:
## Step 1: Recall sulfur's atomic number and properties
Sulfur has an atomic number ($Z$) of 16. In the periodic table, groups are vertical columns and periods are horizontal rows. Elements in group 16 (or 6A in some numbering) have 6 valence electrons. The period number is equal to the number of electron shells. Sulfur has 3 electron shells (electron configuration: $1s^2 2s^2 2p^6 3s^2 3p^4$), so it is in period 3.
## Step 2: Determine group and period
- Group: 16 (or 6A)
- Period: 3

# Answer:
- Group: 16 (or 6A)
- Period: 3

### Part (b)
# Explanation:
## Step 1: Recall atomic notation format
Atomic notation is written as $\ce{^A_ZX}$, where $A$ is the mass number, $Z$ is the atomic number, and $X$ is the element symbol. For sulfur, $Z = 16$ (atomic number). The most common isotope of sulfur has a mass number $A = 32$ (since protons + neutrons = 16 + 16 = 32, though other isotopes exist, 32 is the most stable and common). The element symbol $X$ is $\ce{S}$.
## Step 2: Write the atomic notation
Using the format $\ce{^A_ZX}$, substitute $A = 32$, $Z = 16$, and $X=\ce{S}$. So the atomic notation is $\ce{^{32}_{16}S}$.

# Answer:
$\ce{^{32}_{16}S}$ (or other isotopes like $\ce{^{33}_{16}S}$, $\ce{^{34}_{16}S}$ are also possible, but $\ce{^{32}_{16}S}$ is the most common)

### Part (c)
# Explanation:
## Step 1: Recall Bohr - Rutherford diagram rules
The Bohr - Rutherford diagram shows the nucleus (with protons and neutrons) and electron shells with electrons. Sulfur has $Z = 16$ (16 protons) and for the most common isotope ($A = 32$), neutrons $= A - Z=32 - 16 = 16$. Electron configuration: $2, 8, 6$ (2 electrons in the first shell, 8 in the second, 6 in the third).
## Step 2: Draw the diagram
- Draw a small circle (nucleus) and write $16p^+$ (protons) and $16n^0$ (neutrons) inside.
- Draw three concentric circles (electron shells) around the nucleus.
- Put 2 electrons on the first shell, 8 on the second, and 6 on the third.

(Text - based representation:
Nucleus: $\circ$ with $16p^+, 16n^0$
1st shell (K): $\boldsymbol{2e^-}$
2nd shell (L): $\boldsymbol{8e^-}$
3rd shell (M): $\boldsymbol{6e^-}$)

# Answer:
Nucleus (16 protons, 16 neutrons) with electron shells: K = 2, L = 8, M = 6 (represented as described above)

### Part (d)
# Explanation:
## Step 1: Recall Lewis dot diagram rules
Lewis dot diagrams show the valence electrons (electrons in the outermost shell) as dots around the element symbol. Sulfur has 6 valence electrons (from its electron configuration $3s^2 3p^4$, so the outermost shell has 6 electrons).
## Step 2: Draw the Lewis dot diagram
Write the element symbol $\ce{S}$ and place 6 dots around it, one on each side (usually, we can represent it as two dots on three sides and one side with no dots, but the total is 6). For example:
$\boldsymbol{\cdot \cdot}$
$\boldsymbol{\cdot S \cdot}$
$\boldsymbol{\cdot \cdot}$

# Answer:
Lewis dot diagram for sulfur: $\ce{\cdot \cdot S \cdot \cdot}$ (with two dots above, one on the left, one on the right, and two below, or any arrangement with 6 dots around $\ce{S}$)

### Part (e)
# Explanation:
## Step 1: Recall sulfur's electron gain/loss behavior
Sulfur is in group 16 (has 6 valence electrons). To achieve a stable octet (8 valence electrons), it tends to gain 2 electrons. When an atom gains electrons, it becomes an anion with a negative charge. The number of electrons gained is equal to the charge magnitude.
## Step 2: Determine the ion charge
Since sulfur gains 2 electrons, its ion ($\ce{S^{2-}}$) has a charge of $- 2$.

# Answer:
The charge of the sulfur ion ($\ce{S^{2-}}$) is $-2$

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QUESTION IMAGE

Question

Explanation:

Part (a)

Step 1: Recall sulfur's atomic number and properties

Step 2: Determine group and period

Step 1: Recall atomic notation format

Step 2: Write the atomic notation

Step 1: Recall Bohr - Rutherford diagram rules

Step 2: Draw the diagram

Answer:

Part (b)