The first ionization energy shows an overall increase from left to right across a period as shown in the diagram below for 2"nd period elements. 2nd period 2100 1700 1300 90 500 A Li Be B C N OF Ne a) Define the first ionization energy a) Why the first ionization energy of boron (B) is less than that of beryllium (Be) and why the first ionization energy of oxygen (O) is less than that of nitrogen (N)? Explain 1st ionization energy KJ mol

The first ionization energy shows an overall increase from left to right across a period as shown in the diagram below for 2"nd period elements. 2nd period 2100 1700 1300 90 500 A Li Be B C N OF Ne a) Define the first ionization energy a) Why the first ionization energy of boron (B) is less than that of beryllium (Be) and why the first ionization energy of oxygen (O) is less than that of nitrogen (N)? Explain 1st ionization energy KJ mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Arrange the following atoms in order of increasing ionization energy. F, N, Be, and Mg < <
10. Which of the following element has paramagnetic property? (a) Mg (b) P (c) Ne (d) Hg 11. Which of the following element is a main group (representative group) element? (a) Zn (b) S (c) Cu (d) Co 12. The energy required to remove an electron from an atom in its ground state is called (a) atomic number (b) electronegativity (c) electron affinity (d) ionization energy
From top to bottom, down the periodic table, ionization energy tends to decrease. This is best explained by: a) the greater distance of the electron from the nucleus. b) the instability of atoms at the bottom of the periodic table. c) the greater repulsion between electrons as more are added. d) the strong pull of the nucleus on outer electrons.
6 please
Which element would you expect to be more metallic? (a) Ra O Mg (b) O I Br (c) In O Al
8 please
Strontium has a visible line in its spectrum at 539.8 nm. What is its energy in kJ/mol?
7.125. How do ionization energies change with increasing atomic number (a) down a group of elements in the periodic table and (b) from left to right across a period of elements?
Order the following by ionization energy. 1 has the lowest ionization energy, 4 has the highest ionization energy. Sn xe sb Br