Advertisements
Advertisements
Question
The following element is given \[\ce{_14X}\]. State the electronic configuration and state whether it is a metal, non-metal, or inert gas.
Solution
\[\ce{_14X}\]: Number of electrons = 14
Electronic arrangement = [2, 8, 4]
∴ X is non-metal
APPEARS IN
RELATED QUESTIONS
Summarize the rules for writing of distribution of electrons in various shells for the first eighteen elements.
An element has atomic number 13 and an atomic mass of 27.
(a) How many electrons are there in each atom of the element ?
(b) How are these electrons distributed in the various energy levels ?
The atom of an element X has 7 electrons in its M shell.
(a) Write the electronic configuration of element X.
(b) What is the atomic number of element X?
(c) Is it a metal or a non-metal?
(d) What type of ion will be formed by an atom of element X? Write the symbol of the ion formed.
(e) What could element X be?
The electronic configuration magnesium is 2, 8, 2. From this it is understood that the valence shell of magnesium is ______.
Define the term of the electron.
The atom of aluminium is represented by 27Al13. Write down the number of the arrangement of electrons in the different orbits or shells in one atom of aluminium.
The following element is given \[\ce{_3U}\]. State the electronic configuration and state whether it is a metal, non-metal, or inert gas.
Give a reason for the following:
The shells surrounding the nucleus of an atom are also called ‘energy levels’.
State true or false. If false, correct the statement.
The maximum number of electron in L Shell is 10.
Which block of the periodic table contains metals, non-metals, and metalloids?
