The statement "An atom with high ionization energy will form a positive ion more easily than an atom with low ionization energy" is false.
In this context , we will define ionization energy as the minimum energy required to remove a valence electron from a neutral atom in it's gaseous state. In a sense the ionization energy is a measure the amount of 'difficulty' of making something an ion. A high ionization energy means that it takes a lot of energy to remove a valence electron from that atom. A low ionization energy means that it is easy to remove a valence electron from the atom. It is known that group 1 elements generally have a low ionization energy. On the other hand, it is harder for noble gasses and group 7 atoms to loose electrons because they have higher ionization energy.
To form a positive ion, you have to remove an electron. When an electron is removed from an atom, there ion formed has more positive charges than negative charges in it, making it net positive. We have established that atoms with low ionization energy loose elections much more easily. We have also established that atoms with high ionization energy do not loose electrons easily. From this we can gather that the statement is false. An atom with high ionization energy will not form a positive ion more easily that an atom with low ionization energy.
Answer:
6.61 × 10∧-29 m³
Explanation:
Given data:
Atomic radius= 143 pm = 143 × 10∧-12 m
volume = ?
Formula:
r = a/2√2
143 × 10∧-12 m = a/ 2√2
a= 143 × 10∧-12 m × 2√2
a= 404.4 × 10∧-12 m
where a is edge length, so we can calculate the volume by using following formula:
volume= a³
V= (404.4 × 10∧-12 m)³
v= 6.61 × 10∧-29 m³
The correct option is C.
An atom can be either in the ground state or in an excited state. An atom is said to be in the ground state, if the total energy of its electron can not be lowered by moving one or more electrons into different orbitals. At the ground state, the electrons in the atom have the lowest energy possible and they are stable. On the other hand, an atom is said to be in an excited state, if the energy of its electrons can be lowered by transferring one or more electrons into different orbitals. An atom in an excited state has more energy and is less stable.
C :) shshdjehwjdjdjsjsjsbsbbsdp
Answer:
The structures shown by dots and lines to give the exact number of electrons in the outer most shell is explained by Lewis Structures.
Explanation:
Lewis structures are those structures in which the diagram is shown using the electron representation. They are easy to understand as the diagram completely depicts where the electrons are shared and where they are transferred. The diagram also explains where there is a single bond and where there is a di covalent bond or tri covalent bond explaining where the single , double or triple electron pair is shared. The electrons are shown by dots or lines.
For example CCl₄ can be shown as follows
..
.. Cl..
.. ..
..Cl..----------C----------..Cl..
..
.. Cl..
The picture shows that each chlorine has six electrons in its outer shell and then a pair of electron is shared with carbon forming a single covalent bond.
Similarly methane CH4 can also be shown.
The hydrogen has one electron and it shares an electron from carbon stabilising itself forming methane.
