Question

directions: complete the following table using the information provided. unless otherwise indicated, assume the atom is neutral.

atom/ion	mass number	protons (p)	neutrons (n°)	electrons (e)	complete symbol
cl⁻	35	17	18	18
c	14	6	8	2
s²⁻	32	16	16
cs⁺	133	55	78
zn²⁺	65	30
b	10	5		2
i	127	53
h⁺	3	1
fe³⁺		26	30
	14		7
na⁺	23	11
h	2	1		0
kr	84	36	48
h⁺	1	1

Explanation:

Step1: Recall atomic - related rules

For a neutral atom, number of protons = number of electrons. For an ion, the number of electrons is adjusted according to the charge. Mass number = number of protons+number of neutrons. The atomic symbol is written as $_{Z}^{A}X^{n\pm}$, where $A$ is the mass number, $Z$ is the atomic number (number of protons), $X$ is the chemical symbol, and $n\pm$ is the charge.

Step2: Analyze $Cl^{-}$

The mass number $A = 35$, number of protons $Z=17$, number of neutrons $n = 35 - 17=18$. Since it is a $1 -$ charged anion, number of electrons $e=17 + 1=18$. The symbol is $_{17}^{35}Cl^{-}$.

Step3: Analyze $_{6}^{14}C$

The mass number $A = 14$, number of protons $Z = 6$, number of neutrons $n=14 - 6 = 8$. Since the number of electrons $e = 2$, it is a $4+$ charged cation. The symbol is $_{6}^{14}C^{4+}$.

Step4: Analyze $S^{2-}$

The mass number $A = 32$, number of protons $Z = 16$, number of neutrons $n=32 - 16 = 16$. Since it is a $2 -$ charged anion, number of electrons $e=16+2 = 18$. The symbol is $_{16}^{32}S^{2-}$.

Step5: Analyze $Cs^{+}$

The mass number $A = 133$, number of protons $Z = 55$, number of neutrons $n=133 - 55 = 78$. Since it is a $1+$ charged cation, number of electrons $e=55 - 1=54$. The symbol is $_{55}^{133}Cs^{+}$.

Step6: Analyze $Zn^{2+}$

The mass number $A = 65$, number of protons $Z = 30$, number of neutrons $n=65 - 30 = 35$. Since it is a $2+$ charged cation, number of electrons $e=30 - 2 = 28$. The symbol is $_{30}^{65}Zn^{2+}$.

Step7: Analyze $_{5}^{10}B$

The mass number $A = 10$, number of protons $Z = 5$, number of neutrons $n=10 - 5 = 5$. Since the number of electrons $e = 2$, it is a $3+$ charged cation. The symbol is $_{5}^{10}B^{3+}$.

Step8: Analyze $I$

The mass number $A = 127$, number of protons $Z = 53$, number of neutrons $n=127 - 53 = 74$. For a neutral iodine atom, number of electrons $e = 53$. The symbol is $_{53}^{127}I$.

Step9: Analyze $H^{+}$

The mass number $A = 3$, number of protons $Z = 1$, number of neutrons $n=3 - 1 = 2$. Since it is a $1+$ charged cation, number of electrons $e=1 - 1 = 0$. The symbol is $_{1}^{3}H^{+}$.

Step10: Analyze $Fe^{3+}$

The number of protons $Z = 26$, number of neutrons $n = 30$, mass number $A=26 + 30=56$. Since it is a $3+$ charged cation, number of electrons $e=26 - 3 = 23$. The symbol is $_{26}^{56}Fe^{3+}$.

Step11: Analyze the element with $A = 14$ and $n = 7$

Number of protons $Z=14 - 7 = 7$. It is nitrogen. For a neutral atom, number of electrons $e = 7$. The symbol is $_{7}^{14}N$.

Step12: Analyze $Na^{+}$

The mass number $A = 23$, number of protons $Z = 11$, number of neutrons $n=23 - 11 = 12$. Since it is a $1+$ charged cation, number of electrons $e=11 - 1 = 10$. The symbol is $_{11}^{23}Na^{+}$.

Step13: Analyze $H$

The mass number $A = 2$, number of protons $Z = 1$, number of neutrons $n=2 - 1 = 1$. For a neutral hydrogen atom, number of electrons $e = 1$. The symbol is $_{1}^{2}H$.

Step14: Analyze $Kr$

The mass number $A = 84$, number of protons $Z = 36$, number of neutrons $n=84 - 36 = 48$. For a neutral krypton atom, number of electrons $e = 36$. The symbol is $_{36}^{84}Kr$.

Step15: Analyze $H^{+}$

The mass number $A = 1$, number of protons $Z = 1$, number of neutrons $n=1 - 1 = 0$. Since it is a $1+$ charged cation, number of electrons $e=1 - 1 = 0$. The symbol is $_{1}^{1}H^{+}$.

Answer:

Atom/Ion	Mass Number	Protons ($p$)	Neutrons ($n$)	Electrons ($e$)	Complete Symbol
$Cl^{-}$	35	17	18	18	$_{17}^{35}Cl^{-}$
$_{6}^{14}C$	14	6	8	2	$_{6}^{14}C^{4+}$
$S^{2-}$	32	16	16	18	$_{16}^{32}S^{2-}$
$Cs^{+}$	133	55	78	54	$_{55}^{133}Cs^{+}$
$Zn^{2+}$	65	30	35	28	$_{30}^{65}Zn^{2+}$
$_{5}^{10}B$	10	5	5	2	$_{5}^{10}B^{3+}$
$I$	127	53	74	53	$_{53}^{127}I$
$H^{+}$	3	1	2	0	$_{1}^{3}H^{+}$
$Fe^{3+}$	56	26	30	23	$_{26}^{56}Fe^{3+}$
$_{7}^{14}N$	14	7	7	7	$_{7}^{14}N$
$Na^{+}$	23	11	12	10	$_{11}^{23}Na^{+}$
$_{1}^{2}H$	2	1	1	1	$_{1}^{2}H$
$Kr$	84	36	48	36	$_{36}^{84}Kr$
$H^{+}$	1	1	0	0	$_{1}^{1}H^{+}$