For the noble gases (the Group 8A elements) 4He2, 20Ne10, 40Ar18, 84Kr36 and 132Xe54, (a) determine the number of protons and ne utrons in the nucleus of each atom, and (b) determine the ratio of neutrons to protons in the nucleus of each atom. Describe any general trend you discover in the way this ratio changes with increasing atomic number.
1 answer:
Answer:
a) ⁴He₂
Protons = 2
neutrons = 2
ratio = 1:1
b) ²⁰Ne₁₀
Protons = 10
neutrons = 10
ratio = 1:1
c) ⁴⁰Ar₁₈
Protons = 18
neutrons = 22
ratio = 1.2 : 1
d) ⁸⁴Kr₃₆
Protons = 36
neutrons = 48
ratio = 1.33:1
e) ¹³²Xe₅₄
Protons = 54
neutrons = 78
ratio = 1.44 : 1
With the increase in atomic number the ratio increases.
Explanation:
Atomic number = number of protons
Mass number = number of protons + number of neutrons
So number of neutrons = mass number - number of protons
The element is represented as
Where
A = atomic mass
Z = atomic number
a) ⁴He₂
Protons = 2
neutrons = 2
ratio = 1:1
b) ²⁰Ne₁₀
Protons = 10
neutrons = 10
ratio = 1:1
c) ⁴⁰Ar₁₈
Protons = 18
neutrons = 22
ratio = 1.2 : 1
d) ⁸⁴Kr₃₆
Protons = 36
neutrons = 48
ratio = 1.33:1
e) ¹³²Xe₅₄
Protons = 54
neutrons = 78
ratio = 1.44 : 1
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