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Chapter 2: Problem 67

One isotope of a metallic element has mass number 65 and 35 neutrons in the nucleus. The cation derived from the isotope has 28 electrons. Write the symbol for this cation.

Short Answer

Expert verified
The symbol for the cation derived from this isotope is \(\^65Zn^{+2}\)

Step by step solution

01

Calculate Number of Protons

The mass number of an atom is the sum of the number of protons and the number of neutrons. In this case, the mass number is 65 and the number of neutrons is 35. So, the number of protons can be calculated as \(65 - 35 = 30\). So, this atom has 30 protons.
02

Identify the Element

The atomic number of an element is the number of protons in an atom of that element. With 30 protons, the element is identified to be Zinc, denoted as Zn.
03

Calculate Charge of the Cation

This cation derived from the isotope has 28 electrons. Since there are 30 protons and 28 electrons, the cation has a charge of \(+2\) (as protons are positively charged and electrons are negatively charged). Hence the cation has a charge of \(+2\) due to the loss of 2 electrons.
04

Write the Symbol for this Cation

The isotope's symbol is written with the atomic number superscripted on the left of the element symbol, and in this case, as it's a cation with charge of \(+2\), it's written as \(\^65Zn^{+2}\)

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Most popular questions from this chapter

Element X reacts with element Y to form an ionic compound containing \(\mathrm{X}^{4+}\) and \(\mathrm{Y}^{2-}\) ions. Write a formula for the compound and suggest in which periodic groups these elements are likely to be found. Name a representative compound.

Name these compounds: (a) \(\mathrm{KClO}\) (b) \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) (c) \(\mathrm{FeCl}_{2}\), (d) \(\mathrm{KMnO}_{4}\), (e) \(\mathrm{CsClO}_{3}\), (f) \(\mathrm{HIO},(\mathrm{g}) \mathrm{FeO}\), (h) \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (i) \(\mathrm{TiCl}_{4},(\mathrm{j}) \mathrm{NaH},(\mathrm{k}) \mathrm{Li}_{3} \mathrm{~N},\) (1) \(\mathrm{Na}_{2} \mathrm{O}\) (m) \(\mathrm{Na}_{2} \mathrm{O}_{2},\) (n) \(\mathrm{FeCl}_{3} \cdot 6 \mathrm{H}_{2} \mathrm{O}\).

Write the appropriate symbol for each of the following isotopes: (a) \(Z=11, A=23\) (b) \(Z=28, A=64\).

What do we call atoms of the same elements with different mass numbers?

Pair the following species that contain the same number of electrons: \(\mathrm{Ar}, \mathrm{Sn}^{4+}, \mathrm{F}^{-}, \mathrm{Fe}^{3+}, \mathrm{P}^{3-}, \mathrm{V}, \mathrm{Ag}^{+}, \mathrm{N}^{3-}\)
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