take a look at the periodic table square for zinc (zn):
5. what does the “30” refer to?
a. ion charge
b. average atomic mass
c. atomic number
d. family number

6. what does the “65.4” refer to?
a. ion charge
b. average atomic mass
c. atomic number
d. family number

7. what does the “2+” refer to?
a. ion charge
b. average atomic mass
c. atomic number
d. family number

8. complete the table below. this table does have ions & isotopes:
| name | nuclide symbol (with mass number, atomic number, charge, symbol labeled as in ²³₁₁na⁺) | mass # | # of protons | # of neutrons | # of electrons |
| --- | --- | --- | --- | --- | --- |
| oxygen | | | | 9 | 10 |
| | | | 53 | | 54 |
| | ⁷⁰ga³⁺ | | | | |

9. take a look at the bohr model. an electron fell from the second energy level to the first energy level. the energy was released as light.
a. label which energy level (ring) is the excited state of the electron and which is the ground state of the electron on the model (with an image showing higher - energy orbit and lower - energy orbit with an electron transition).
b. when the electron transitions from the excited to the ground state it ______ energy.

Question

take a look at the periodic table square for zinc (zn):
5. what does the “30” refer to?
a. ion charge
b. average atomic mass
c. atomic number
d. family number

6. what does the “65.4” refer to?
a. ion charge
b. average atomic mass
c. atomic number
d. family number

7. what does the “2+” refer to?
a. ion charge
b. average atomic mass
c. atomic number
d. family number

8. complete the table below. this table does have ions & isotopes:
| name | nuclide symbol (with mass number, atomic number, charge, symbol labeled as in ²³₁₁na⁺) | mass # | # of protons | # of neutrons | # of electrons |
| --- | --- | --- | --- | --- | --- |
| oxygen |  |  |  | 9 | 10 |
|  |  |  | 53 |  | 54 |
|  | ⁷⁰ga³⁺ |  |  |  |  |

9. take a look at the bohr model. an electron fell from the second energy level to the first energy level. the energy was released as light.
 a. label which energy level (ring) is the excited state of the electron and which is the ground state of the electron on the model (with an image showing higher - energy orbit and lower - energy orbit with an electron transition).
 b. when the electron transitions from the excited to the ground state it ______ energy.

Accepted Answer

### Question 5
# Brief Explanations:
In a periodic table square, the atomic number is the number of protons in an atom's nucleus, and it's typically the whole number at the top. For Zinc, "30" is the atomic number (number of protons), while ion charge is "2+", average atomic mass is "65.4", and family number isn't represented this way. So "30" refers to atomic number.
# Answer:
C. atomic number

### Question 6
# Brief Explanations:
In the periodic table square, the number at the bottom (usually a decimal) represents the average atomic mass of the element, which is the weighted average of the masses of its isotopes. "65.4" fits this description; ion charge is "2+", atomic number is "30", and family number isn't this. So "65.4" is average atomic mass.
# Answer:
B. average atomic mass

### Question 7
# Brief Explanations:
The "2+" in the Zinc square indicates the charge of the Zinc ion (how many electrons it has gained or lost). Ion charge is represented by a symbol with a sign and number, while average atomic mass is "65.4", atomic number is "30", and family number isn't this. So "2+" is ion charge.
# Answer:
A. ion charge

### Question 8 (Oxygen Row)
# Explanation:
## Step1: Find atomic number (protons)
Oxygen has an atomic number of 8, so protons = 8.
## Step2: Calculate mass number
Mass number = protons + neutrons. Neutrons = 9, protons = 8, so mass number = $ 8 + 9 = 17 $.
## Step3: Determine ion charge (electrons)
Electrons = 10, protons = 8. Charge = protons - electrons = $ 8 - 10 = -2 $, so the ion is $ \ce{^{17}_{8}O^{2-}} $.
## Step4: Name the ion
It's an oxide ion (oxygen with 2- charge), or we can call it oxygen - 17 ion (but typically oxide ion, or just note the nuclide symbol as $ \ce{^{17}_{8}O^{2-}} $).

| Name       | Nuclide Symbol       | Mass # | # of Protons | # of Neutrons | # of Electrons |
|------------|----------------------|--------|--------------|---------------|----------------|
| Oxygen (oxide ion) | $ \ce{^{17}_{8}O^{2-}} $ | 17     | 8            | 9             | 10             |

### Question 8 (Row with 53 Protons)
# Explanation:
## Step1: Identify the element
Atomic number 53 is Iodine (I).
## Step2: Calculate neutrons (assuming mass number, but let's find mass number from electrons/charge)
Electrons = 54, protons = 53. Charge = protons - electrons = $ 53 - 54 = -1 $, so it's an iodide ion. Mass number: Let's assume we need to find neutrons, but wait, we need more info? Wait, maybe the mass number is protons + neutrons, but if we don't have neutrons, maybe it's a standard isotope? Wait, Iodine - 127 is common, but let's check: protons = 53, electrons = 54 (so charge -1). Let's say mass number: if we assume neutrons, but maybe the table is for an isotope. Wait, protons = 53, electrons = 54 (charge -1). Let's find neutrons: mass number = protons + neutrons. But maybe the mass number is 126 (53 + 73? No, wait, Iodine has isotopes. Wait, maybe the mass number is 126 (53 protons, 73 neutrons? No, 53 + 73 = 126). Wait, let's proceed:

| Name       | Nuclide Symbol       | Mass # | # of Protons | # of Neutrons | # of Electrons |
|------------|----------------------|--------|--------------|---------------|----------------|
| Iodine (iodide ion) | $ \ce{^{126}_{53}I^{-}} $ | 126    | 53           | 73 (126 - 53) | 54             |

### Question 8 ( $ \ce{^{70}Ga^{3+}} $ Row)
# Explanation:
## Step1: Mass number
The nuclide symbol has mass number 70, so mass # = 70.
## Step2: Protons (atomic number of Ga)
Gallium (Ga) has atomic number 31, so protons = 31.
## Step3: Neutrons
Neutrons = mass number - protons = $ 70 - 31 = 39 $.
## Step4: Electrons (ion charge)
Charge = +3, so electrons = protons - charge = $ 31 - 3 = 28 $.
## Step5: Name
Gallium - 70 ion (or gallium(III) ion).

| Name           | Nuclide Symbol       | Mass # | # of Protons | # of Neutrons | # of Electrons |
|----------------|----------------------|--------|--------------|---------------|----------------|
| Gallium - 70 ion | $ \ce{^{70}_{31}Ga^{3+}} $ | 70     | 31           | 39            | 28             |

### Question 9a
# Brief Explanations:
In the Bohr Model, the excited state is the higher - energy orbit (where the electron has more energy, so the second energy level, as it fell from second to first). The ground state is the lower - energy orbit (first energy level, where electrons are in the lowest energy state). So label the higher - energy orbit (second level) as excited state and lower - energy orbit (first level) as ground state.
# Answer:
- Excited state: Higher - energy orbit (second energy level)
- Ground state: Lower - energy orbit (first energy level)

### Question 9b
# Brief Explanations:
When an electron transitions from an excited state (higher energy) to the ground state (lower energy), it releases energy (in the form of light, as given). So the electron emits (or releases) energy.
# Answer:
releases (or emits)

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