Q2. This question is about the periodicity of the Period 3 elements. (a) State and explain the general trend in first ionisation energy across Period 3. (b) Give one example of an element which deviates from the general trend in first ionisation energy across Period 3. Explain why this deviation occurs. Page 3 of 12 (c) The table shows successive ionisation energies of an element Y in Period 3. lonisation number 1 2 3 4 6 7 8 lonisation energy / kJ mol- 1000 2260 3390 4540 6990 8490 27 100 31 700 Identify element Y. Explain your answer using data from the table. (d) Identify the Period 3 element that has the highest melting point. Explain your answer by reference to structure and bonding.

Q2. This question is about the periodicity of the Period 3 elements. (a) State and explain the general trend in first ionisation energy across Period 3. (b) Give one example of an element which deviates from the general trend in first ionisation energy across Period 3. Explain why this deviation occurs. Page 3 of 12 (c) The table shows successive ionisation energies of an element Y in Period 3. lonisation number 1 2 3 4 6 7 8 lonisation energy / kJ mol- 1000 2260 3390 4540 6990 8490 27 100 31 700 Identify element Y. Explain your answer using data from the table. (d) Identify the Period 3 element that has the highest melting point. Explain your answer by reference to structure and bonding.

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

What is the answer to this one?
The first ionization energy shows an overall increase from left to right across a period as shown in the diagram below for 2nd period elements. 2nd period 2100 1700 S 1300 900 A. 500 A Li Be B C NO F 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
3. What is the effective nuclear charge on3(a) the outer two electrons of B? 3(b) the inner two electrons of B? 3(c) Explain the four ionization energies of B being 801, 2427, 3660 and 25025kJ/mol?
What causes the changes in ionisation energy across period 2 elements?
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.
Which of the following elements would you expect to have similar properties? As Te Ar Sn He
Select the group of the periodic table containing some elements with a condensed electron configuration of [X]ns2(n-1)dnp. Period Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display MAIN-GROUP ELEMENTS Metals (main-group) Metals (transition) MAIN-GROUP ELEMENTS Metals (inner transition). - 1A (1) 1 H 2A 1.008 (2) 3 4 2 LI Be Metalloids Nonmetals 8A (18) 2 ЗА 4A 5A 6A 7A He (13) (14) (15) (16) (17) 4.003 5 6 7 8 9 10 B C N F Ne 6.941 9.012 10.81 12.01 14.01 16.00 19.00 20.18 11 12 TRANSITION ELEMENTS 13 14 15 16 " w 3 Na Mg 38 4B 5B 68 7B 8B- 1B 2B AI Si P S 22.99 24.31 (3) (4) (5) (6) (7) (8) (9) (10) (11) 19 20 21 22 23 24 25 26 27 28 29 (12) 26.98 31 28.09 30.97 32.07 17 18 CI Ar 35.45 39.95 K Ca Sc Ti V Cr Mn Fe Co Ni 37 38 40 41 42 Zr Nb Mo 95.94 55 56 57 6 Cs Ba La 73 74 W 183.9 104 105 106 7 39.10 40.08 44.96 47.88 50.94 52.00 54.94 55.85 39 5 Rb Sr Y 85.47 87.62 88.91 91.22 92.91 72 Hf Ta 132.9 137.3 138.9 178.5 180.9 87 88 89 Fr Ra Ac Rf…
How is the periodic Table arranged? (A) Horizontally ( B) Vertically (C) Atomic Mass. (D) Periods and Groups
Knowing that atomic radius and ionization energy are two important properties of an atom that are periodic in nature. First, (i) define the term ionization energy. Then, (ii) state the directions along the periodic table (up, down, left, right) that a) atomic radius and b) ionization energy increase and (iii) explain the factors that lead to each of these trends.
What are ionization energy for atoms : (a) F (b) Ca (c) Ba