13. if protons and neutrons have the same mass, what is the approximate mass of a proton and neutron in atomic mass units (amu)?
14. the mass of (_6^{14} ext{c}) is about 14 amu. does this agree with what you determined in questions 11 and 13?
15. the charge (in the upper right hand corner of the element symbol) is (-1) for a fluorine ion. why isn’t it (+1) or some other number?
16. what is the charge on every atom? why is this the charge?
17. how do you determine the charge on an ion?
18. an oxygen ion has a (-2) charge. (use your periodic table if necessary)
a) how many protons does the oxygen ion have?
b) how many electrons does the oxygen ion have?
19) what is the mass # of zinc - 70? what is the isotopes charge?
20 determine the elements name, # of protons, electron and neutrons
a) at
name=
#protons =
#electrons =
#neutrons =
b) w
name:
#protons =
#electrons =
#neutrons =
copyright 2002 - 2004 by jason neil. all rights reserved.
to make copies permission must be obtained from www.chemistryinquiry.com

Question

13. if protons and neutrons have the same mass, what is the approximate mass of a proton and neutron in atomic mass units (amu)?
14. the mass of (_6^{14}	ext{c}) is about 14 amu. does this agree with what you determined in questions 11 and 13?
15. the charge (in the upper right hand corner of the element symbol) is (-1) for a fluorine ion. why isn’t it (+1) or some other number?
16. what is the charge on every atom? why is this the charge?
17. how do you determine the charge on an ion?
18. an oxygen ion has a (-2) charge. (use your periodic table if necessary)
    a) how many protons does the oxygen ion have?
    b) how many electrons does the oxygen ion have?
19) what is the mass # of zinc - 70? what is the isotopes charge?
20 determine the elements name, # of protons, electron and neutrons
    a) at
       name=
       #protons =
       #electrons =
       #neutrons =
    b) w
       name:
       #protons =
       #electrons =
       #neutrons =
copyright 2002 - 2004 by jason neil. all rights reserved.
to make copies permission must be obtained from www.chemistryinquiry.com

Accepted Answer

### Question 13
# Explanation:
## Step1: Recall atomic mass unit concept
Protons and neutrons have approximately the same mass, and 1 atomic mass unit (amu) is defined as approximately the mass of 1 proton or 1 neutron. So, the mass of a proton and a neutron is approximately 1 amu each.
# Answer:
The approximate mass of a proton and a neutron is 1 amu.

### Question 14
# Explanation:
## Step1: Analyze carbon - 14 mass
Carbon - 14 ($_{6}^{14}	ext{C}$) has 6 protons and 8 neutrons (since mass number = number of protons+number of neutrons, so number of neutrons = 14 - 6 = 8). From question 13, we know that protons and neutrons have a mass of approximately 1 amu each. So the total mass should be (number of protons×1 amu)+(number of neutrons×1 amu)=(6×1)+(8×1)=14 amu. So it agrees with the determination from questions 11 and 13.
# Answer:
Yes, it agrees. The mass of $_{6}^{14}	ext{C}$ (14 amu) is equal to the sum of the masses of its 6 protons and 8 neutrons (each with ~1 amu mass).

### Question 15
# Brief Explanations:
Fluorine is in group 17 (halogens) of the periodic table. Halogens have 7 valence electrons. To achieve a stable octet (8 valence electrons), a fluorine atom gains 1 electron. When an atom gains an electron, it becomes an anion with a charge of - 1 (since electrons have a negative charge, gaining 1 electron gives a net charge of - 1). It can't be + 1 because fluorine has a high electronegativity and tends to gain electrons, not lose them (losing electrons would require a lot of energy as it is close to having a stable octet by gaining one electron).
# Answer:
Fluorine gains 1 electron to achieve a stable octet, so its ion has a - 1 charge. It doesn't have + 1 as it gains, not loses, electrons.

### Question 16
# Brief Explanations:
Every atom has a charge of 0 (neutral). This is because the number of protons (positive charge) in an atom is equal to the number of electrons (negative charge). The positive charges from protons and negative charges from electrons cancel each other out, resulting in a net charge of 0.
# Answer:
The charge on every atom is 0. This is because the number of protons (positive) equals the number of electrons (negative), so their charges cancel.

### Question 17
# Brief Explanations:
To determine the charge on an ion, we compare the number of protons and electrons. If the number of electrons is greater than the number of protons, the ion has a negative charge (anion), and the magnitude of the charge is (number of electrons - number of protons). If the number of protons is greater than the number of electrons, the ion has a positive charge (cation), and the magnitude of the charge is (number of protons - number of electrons). Also, for main - group elements, we can use the group number: metals in groups 1, 2, 13 tend to lose electrons (charge equal to group number or group number - 10 for group 13), and non - metals in groups 15 - 17 tend to gain electrons (charge equal to 18 - group number or group number - 10 with a negative sign).
# Answer:
The charge on an ion is determined by the difference between the number of protons and electrons. For main - group elements, group number (or 18 - group number for non - metals) also helps: metals lose electrons (positive charge), non - metals gain electrons (negative charge).

### Question 18
#### Part (a)
# Explanation:
## Step1: Recall proton number for oxygen
The atomic number of oxygen is 8. The atomic number is equal to the number of protons in an atom or ion of that element. So, an oxygen ion has 8 protons.
# Answer:
The oxygen ion has 8 protons.

#### Part (b)
# Explanation:
## Step1: Recall ion charge and electron - proton relationship
The charge of an ion is given by the formula: Charge = number of protons - number of electrons. We know the charge of the oxygen ion is - 2 and the number of protons is 8. Rearranging the formula: number of electrons=number of protons - charge. Substituting the values: number of electrons = 8-(-2)=8 + 2 = 10.
# Answer:
The oxygen ion has 10 electrons.

### Question 19
# Explanation:
## Step1: Determine mass number of zinc - 70
The mass number of an isotope is given in its name. For zinc - 70, the mass number is 70.
## Step2: Determine isotope charge
A neutral zinc atom has 30 protons (atomic number of Zn is 30) and 30 electrons. If there is no indication of a charge (for a neutral isotope), the charge of the zinc - 70 isotope (assuming it's neutral) is 0. If it were an ion, we would need more information, but typically, when we talk about an isotope like zinc - 70 without specifying charge, it's neutral.
# Answer:
The mass number of zinc - 70 is 70. The charge of the zinc - 70 isotope (assuming neutral) is 0.

### Question 20
#### Part (a) - For $^{}_{}	ext{At}$ (Astatine)
# Explanation:
## Step1: Determine atomic number of Astatine
The atomic number of Astatine (At) is 85. The number of protons in an atom is equal to its atomic number, so the number of protons is 85.
## Step2: Determine number of electrons (neutral atom)
In a neutral atom, the number of electrons is equal to the number of protons. So, the number of electrons is 85.
## Step3: Determine number of neutrons (assuming mass number)
The most common isotope of Astatine has a mass number of 210. Number of neutrons = mass number - atomic number=210 - 85 = 125. (If no specific mass number is given, we can use the common isotope or note that we need more info, but for a general case with the symbol At, atomic number = 85, protons = 85, electrons (neutral)=85, neutrons depend on isotope, but for the most common, 125).
# Answer:
- Name: Astatine
- # Protons: 85
- # Electrons: 85 (for neutral atom)
- # Neutrons: 125 (for $^{210}_{85}	ext{At}$)

#### Part (b) - For $^{}_{}	ext{W}$ (Tungsten)
# Explanation:
## Step1: Determine atomic number of Tungsten
The atomic number of Tungsten (W) is 74. So, the number of protons is 74.
## Step2: Determine number of electrons (neutral atom)
In a neutral atom, the number of electrons is equal to the number of protons. So, the number of electrons is 74.
## Step3: Determine number of neutrons (assuming mass number)
The most common isotope of Tungsten has a mass number of 184. Number of neutrons = mass number - atomic number=184 - 74 = 110. (If no specific mass number is given, we can use the common isotope or note that we need more info, but for a general case with the symbol W, atomic number = 74, protons = 74, electrons (neutral)=74, neutrons depend on isotope, but for the most common, 110).
# Answer:
- Name: Tungsten
- # Protons: 74
- # Electrons: 74 (for neutral atom)
- # Neutrons: 110 (for $^{184}_{74}	ext{W}$)

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QUESTION IMAGE

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Explanation:

Question 13

Step1: Recall atomic mass unit concept

Step1: Analyze carbon - 14 mass

Answer:

Question 14