Chapter 2, Problem 11Q

Give the number of protons, neutrons, and electrons in each of these neutral atoms.

1. a. oxygen-18 ${(}_8^{18}\text{O})$
2. b. sulfur-35 ${(}_{16}^{35}\text{S})$
3. c. uranium-239 ${(}_{82}^{239}\text{U})$
4. d. bromine-82 ${(}_{35}^{82}\text{Br})$
5. e. neon-19 ${(}_{10}^{19}\text{Ne})$
6. f. radium-226 ${(}_{88}^{226}\text{Ra})$

Interpretation Introduction

Interpretation:

The number of protons, neutrons and electrons in the given neutral atom oxygen- 18

(${}_8{O}^{18}$ ) has to be determined.

Concept Introduction:

In a periodic table, an element is represented as shown below,

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

The atomic mass can be calculated using the formula,

$Atomicmass=Numberofprotons\left(N_P\right)+Numberofneutrons\left(N_n\right)$

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Isotopes are species which have the same number of protons and different mass number.

Examples: ${}_1{H}^1,{}_1{H}^{2}and{}_1{H}^3$

Explanation of Solution

The given neutral atoms is,

${}_8{O}^{18}$

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

Thus,

Number of proton and electron in this atom is 8.

Number of neutrons in this neutral atom can be determined using the following equation,

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Thus, the number of neutrons in ${}_8{O}^{18}$= $18-8=10$

Interpretation Introduction

Interpretation:

The number of protons, neutrons and electrons in the given neutral atom sulfur- 35

(${}_{16}{S}^{35}$ ) has to be determined.

Concept Introduction:

In a periodic table, an element is represented as shown below,

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

The atomic mass can be calculated using the formula,

$Atomicmass=Numberofprotons\left(N_P\right)+Numberofneutrons\left(N_n\right)$

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Isotopes are species which have the same number of protons and different mass number.

Examples: ${}_1{H}^1,{}_1{H}^{2}and{}_1{H}^3$

Explanation of Solution

The given neutral atoms is,

${}_{16}{S}^{35}$

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

Thus,

Number of proton and electron in this atom is 16.

Number of neutrons in this neutral atom can be determined using the following equation,

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Thus, the number of neutrons in ${}_{16}{S}^{35}$= $35-16=19$

Interpretation Introduction

Interpretation:

The number of protons, neutrons and electrons in the given neutral atom uranium- 239

(${}_{82}{U}^{239}$ ) has to be determined.

Concept Introduction:

In a periodic table, an element is represented as shown below,

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

The atomic mass can be calculated using the formula,

$Atomicmass=Numberofprotons\left(N_P\right)+Numberofneutrons\left(N_n\right)$

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Isotopes are species which have the same number of protons and different mass number.

Examples: ${}_1{H}^1,{}_1{H}^{2}and{}_1{H}^3$

Explanation of Solution

The given neutral atoms is,

${}_{82}{U}^{239}$

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

Thus,

Number of proton and electron in this atom is 82.

Number of neutrons in this neutral atom can be determined using the following equation,

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Thus, the number of neutrons in ${}_{82}{U}^{239}$= $239-82=157$

Interpretation Introduction

Interpretation:

The number of protons, neutrons and electrons in the given neutral atom bromine- 82

(${}_{35}B{r}^{82}$ ) has to be determined.

Concept Introduction:

In a periodic table, an element is represented as shown below,

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

The atomic mass can be calculated using the formula,

$Atomicmass=Numberofprotons\left(N_P\right)+Numberofneutrons\left(N_n\right)$

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Isotopes are species which have the same number of protons and different mass number.

Examples: ${}_1{H}^1,{}_1{H}^{2}and{}_1{H}^3$

Explanation of Solution

The given neutral atoms is,

${}_{35}B{r}^{82}$

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

Thus,

Number of proton and electron in this atom is 35.

Number of neutrons in this neutral atom can be determined using the following equation,

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Thus, the number of neutrons in ${}_{35}B{r}^{82}$= $82-35=47$

Interpretation Introduction

Interpretation:

The number of protons, neutrons and electrons in the given neutral atom neon- 19

(${}_{10}N{e}^{19}$ ) has to be determined.

Concept Introduction:

In a periodic table, an element is represented as shown below,

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

The atomic mass can be calculated using the formula,

$Atomicmass=Numberofprotons\left(N_P\right)+Numberofneutrons\left(N_n\right)$

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Isotopes are species which have the same number of protons and different mass number.

Examples: ${}_1{H}^1,{}_1{H}^{2}and{}_1{H}^3$

Explanation of Solution

The given neutral atoms is,

${}_{10}N{e}^{19}$

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

Thus,

Number of proton and electron in this atom is 10.

Number of neutrons in this neutral atom can be determined using the following equation,

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Thus, the number of neutrons in ${}_{10}N{e}^{19}$= $19-10=9$

Interpretation Introduction

Interpretation:

The number of protons, neutrons and electrons in the given neutral atom radium- 226

(${}_{88}R{a}^{226}$ ) has to be determined.

Concept Introduction:

In a periodic table, an element is represented as shown below,

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

The atomic mass can be calculated using the formula,

$Atomicmass=Numberofprotons\left(N_P\right)+Numberofneutrons\left(N_n\right)$

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Isotopes are species which have the same number of protons and different mass number.

Examples: ${}_1{H}^1,{}_1{H}^{2}and{}_1{H}^3$

Explanation of Solution

The given neutral atoms is,

${}_{88}R{a}^{226}$

Atomic number is equal to the number of proton ($N_P$), which also equal to the number of electrons ($N_e$).

Thus,

Number of proton and electron in this atom is 88.

Number of neutrons in this neutral atom can be determined using the following equation,

$Numberofneutrons\left(N_n\right)=Atomicmass(A)-Numberofprotons\left(N_P\right)$

Thus, the number of neutrons in ${}_{88}R{a}^{226}$= $226-88=138$