use your periodic tables
atomic structure worksheet
1. the 3 particles of the atom are:
a. __________
b. __________
c. __________
their charges are:
a. __________
b. __________
c. __________

2. the number of protons in one atom of an element determines the atom’s __________, and the number of electrons determines __________ of an element.

3. the atomic number tells you the number of __________ in one atom of an element. it also tells you the number of __________ in a neutral atom of that element. the atomic number gives the “identity” of an element as well as its location on the periodic table. no two different elements will have the __________ atomic number.

4. the __________ of an element is the average mass of an element’s naturally occurring atoms, or isotopes, taking into account the __________ of each isotope.

5. the __________ of an element is the total number of protons and neutrons in the __________ of the atom.

6. the mass number is used to calculate the number of __________ in one atom of an element. in order to calculate the number of neutrons you must subtract the __________ from the __________.

element list (partial): lithium, helium, iron, copper, oxygen, mercury, krypton, helium (typo?)

8. give the symbol and number of electrons in a neutral atom of:
uranium __________
chlorine __________
boron __________
iodine __________
antimony __________
xenon __________

9. give the symbol and number of neutrons in one atom of:
(to get “mass number”, you must round the “atomic mass” to the nearest whole number. show your calculations.)
barium __________
rhenium __________
carbon __________
hydrogen __________
fluorine __________
magnesium __________
europium __________

Question

use your periodic tables
atomic structure worksheet
1. the 3 particles of the atom are:
   a. __________
   b. __________
   c. __________
   their charges are:
   a. __________
   b. __________
   c. __________

2. the number of protons in one atom of an element determines the atom’s __________, and the number of electrons determines __________ of an element.

3. the atomic number tells you the number of __________ in one atom of an element. it also tells you the number of __________ in a neutral atom of that element. the atomic number gives the “identity” of an element as well as its location on the periodic table. no two different elements will have the __________ atomic number.

4. the __________ of an element is the average mass of an element’s naturally occurring atoms, or isotopes, taking into account the __________ of each isotope.

5. the __________ of an element is the total number of protons and neutrons in the __________ of the atom.

6. the mass number is used to calculate the number of __________ in one atom of an element. in order to calculate the number of neutrons you must subtract the __________ from the __________.

element list (partial): lithium, helium, iron, copper, oxygen, mercury, krypton, helium (typo?)

8. give the symbol and number of electrons in a neutral atom of:
   uranium __________
   chlorine __________
   boron __________
   iodine __________
   antimony __________
   xenon __________

9. give the symbol and number of neutrons in one atom of:
   (to get “mass number”, you must round the “atomic mass” to the nearest whole number. show your calculations.)
   barium __________
   rhenium __________
   carbon __________
   hydrogen __________
   fluorine __________
   magnesium __________
   europium __________

Accepted Answer

### Question 1: The 3 particles of the atom are:
#### Brief Explanations:
Atoms are composed of three main subatomic particles. Protons are positively charged particles found in the nucleus. Neutrons are neutral (no charge) particles also in the nucleus. Electrons are negatively charged particles that orbit the nucleus in electron clouds. Their charges are: proton ($+$), neutron ($0$), electron ($-$).
#### Answers:
a. Proton
b. Neutron
c. Electron

Proton charges are: $+$
Neutron charges are: $0$ (neutral)
Electron charges are: $-$

### Question 2: The number of protons in one atom of an element determines the atom’s $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$, and the number of electrons determines $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ of and element.
#### Brief Explanations:
The number of protons in an atom is the atomic number, which defines the element’s identity (e.g., 6 protons = carbon). In a neutral atom, electrons equal protons, and electron configuration (arrangement) determines chemical properties (how the atom bonds/react).
#### Answer:
The number of protons in one atom of an element determines the atom’s **atomic number (identity)**, and the number of electrons determines the **chemical properties** of the element.

### Question 3: The atomic number tells you the number of $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ in one atom of an element. It also tells you the number of $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ in a neutral atom of that element. The atomic number gives the “identity” of an element as well as its location on the Periodic Table: No two different elements will have the $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ atomic number.
#### Brief Explanations:
Atomic number ($Z$) = number of protons (defines the element). In a neutral atom, electrons = protons, so atomic number also equals electrons. Each element has a unique atomic number (e.g., H=1, He=2, etc.).
#### Answer:
The atomic number tells you the number of **protons** in one atom of an element. It also tells you the number of **electrons** in a neutral atom of that element. No two different elements will have the **same** atomic number.

### Question 4: The $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ of an element is the average mass of an element’s naturally occurring atoms, or isotopes, taking into account the $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ of each isotope.
#### Brief Explanations:
Atomic mass (or atomic weight) is the weighted average of an element’s isotopes. “Weighted” means it accounts for the **abundance (percent occurrence)** of each isotope. For example, carbon has isotopes $^{12}\text{C}$ (98.9%) and $^{13}\text{C}$ (1.1%), so atomic mass ≈ 12.01.
#### Answer:
The **atomic mass (atomic weight)** of an element is the average mass of an element’s naturally occurring atoms, or isotopes, taking into account the **abundance (relative abundance)** of each isotope.

### Question 5: The $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ of an element is the total number of protons and neutrons in the $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ of the atom.
#### Brief Explanations:
Mass number ($A$) = protons + neutrons. Both protons and neutrons are in the **nucleus** of the atom (electrons have negligible mass).
#### Answer:
The **mass number** of an element is the total number of protons and neutrons in the **nucleus** of the atom.

### Question 6: The mass number is used to calculate the number of $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ in one atom of an element. In order to calculate the number of neutrons you must subtract the $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$ from the $\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}$.
#### Brief Explanations:
Mass number ($A$) = protons + neutrons, so neutrons = $A -$ protons. Protons = atomic number ($Z$), so neutrons = $A - Z$.
#### Answer:
The mass number is used to calculate the number of **neutrons** in one atom of an element. In order to calculate the number of neutrons you must subtract the **atomic number (number of protons)** from the **mass number**.

### Question 8: Give the symbol and number of electrons in a neutral atom of:
#### Brief Explanations:
In a neutral atom, electrons = protons = atomic number ($Z$). Find the element’s symbol and $Z$ from the periodic table.
- Uranium: Symbol $ \text{U} $, $ Z = 92 $ → electrons = 92.
- Chlorine: Symbol $ \text{Cl} $, $ Z = 17 $ → electrons = 17.
- Boron: Symbol $ \text{B} $, $ Z = 5 $ → electrons = 5.
- Iodine: Symbol $ \text{I} $, $ Z = 53 $ → electrons = 53.
- Antimony: Symbol $ \text{Sb} $, $ Z = 51 $ → electrons = 51.
- Xenon: Symbol $ \text{Xe} $, $ Z = 54 $ → electrons = 54.
#### Answers:
- Uranium: $ \text{U} $, 92 electrons
- Chlorine: $ \text{Cl} $, 17 electrons
- Boron: $ \text{B} $, 5 electrons
- Iodine: $ \text{I} $, 53 electrons
- Antimony: $ \text{Sb} $, 51 electrons
- Xenon: $ \text{Xe} $, 54 electrons

### Question 9: Give the symbol and number of neutrons in one atom of (Show calculations):
#### Brief Explanations:
Neutrons = mass number ($A$) – atomic number ($Z$). Mass number is the rounded atomic mass. Find $Z$ (protons) from the periodic table.
- Barium: Symbol $ \text{Ba} $, $ Z = 56 $, atomic mass ≈ 137 → $ A = 137 $. Neutrons = $ 137 - 56 = 81 $.
- Bismuth: Symbol $ \text{Bi} $, $ Z = 83 $, atomic mass ≈ 209 → $ A = 209 $. Neutrons = $ 209 - 83 = 126 $.
- Carbon: Symbol $ \text{C} $, $ Z = 6 $, atomic mass ≈ 12 → $ A = 12 $. Neutrons = $ 12 - 6 = 6 $.
- Hydrogen: Symbol $ \text{H} $, $ Z = 1 $, atomic mass ≈ 1 → $ A = 1 $. Neutrons = $ 1 - 1 = 0 $.
- Fluorine: Symbol $ \text{F} $, $ Z = 9 $, atomic mass ≈ 19 → $ A = 19 $. Neutrons = $ 19 - 9 = 10 $.
- Magnesium: Symbol $ \text{Mg} $, $ Z = 12 $, atomic mass ≈ 24 → $ A = 24 $. Neutrons = $ 24 - 12 = 12 $.
- Europium: Symbol $ \text{Eu} $, $ Z = 63 $, atomic mass ≈ 152 → $ A = 152 $. Neutrons = $ 152 - 63 = 89 $.
#### Answers (with calculations):
- Barium: $ \text{Ba} $, Neutrons = $ 137 - 56 = 81 $
- Bismuth: $ \text{Bi} $, Neutrons = $ 209 - 83 = 126 $
- Carbon: $ \text{C} $, Neutrons = $ 12 - 6 = 6 $
- Hydrogen: $ \text{H} $, Neutrons = $ 1 - 1 = 0 $
- Fluorine: $ \text{F} $, Neutrons = $ 19 - 9 = 10 $
- Magnesium: $ \text{Mg} $, Neutrons = $ 24 - 12 = 12 $
- Europium: $ \text{Eu} $, Neutrons = $ 152 - 63 = 89 $

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Question 1: The 3 particles of the atom are:

Answer:

Question 2: The number of protons in one atom of an element determines the atom’s \(\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}\), and the number of electrons determines \(\boldsymbol{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}\) of and element.