vi. Answer true or false. (a) Elements in the same column of the Periodic Table have the same outer-shell electron configuration. (b) All Group 1A elements have one electron in their valence shell. (c) All Group 6A elements have six electrons in their valence shell. (d) All Group 8A elements have eight electrons in their valence shell. (e) Period 1 of the Periodic Table has one element, period 2 has two elements, period 3 has three elements, and so forth. () Period 2 results from filling the 2s and 2p orbitals and, therefore, there are eight elements in period 2. (g) Period 3 results from filling the 3s, 3p, and 3d orbitals and, therefore, there are nine elements in period 3. (h) The main-group elements are s block and p block elements.

vi. Answer true or false. (a) Elements in the same column of the Periodic Table have the same outer-shell electron configuration. (b) All Group 1A elements have one electron in their valence shell. (c) All Group 6A elements have six electrons in their valence shell. (d) All Group 8A elements have eight electrons in their valence shell. (e) Period 1 of the Periodic Table has one element, period 2 has two elements, period 3 has three elements, and so forth. () Period 2 results from filling the 2s and 2p orbitals and, therefore, there are eight elements in period 2. (g) Period 3 results from filling the 3s, 3p, and 3d orbitals and, therefore, there are nine elements in period 3. (h) The main-group elements are s block and p block elements.

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter11: Atomic Theory :the Quantum Model Of The Atom

Section: Chapter Questions

Problem 11.5TC

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2.42 What is a period in the periodic table? From what does it derive its name?
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. Give one example of an element which deviates from the general trend in first (b) 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 5 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.
choose three . What are the characteristerses of a metal like element? (a) they try to get additional electrons (b) they are melleable. (c) they are lightly to give away or share electrons. (d) they are good conductors of electricity
Q1. This question is about atomic structure. (a) Write the full electron configuration for each of the following species. CH Fe2+ (b) Write an equation, including state symbols, to represent the process that occurs when the third ionisation energy of manganese is measured. (c) State which of the elements magnesium and aluminium has the lower first ionisation energy Explain your answer. (d) A sample of nickel was analysed in a time of flight (TOF) mass spectrometer. The sample was ionised by electron impact ionisation. The spectrum produced showed three peaks with abundances as set out in the table. m/z Abundance /% 58 61.0 60 29.1 61 9.9 Give the symbol, including mass number, of the ion that would reach the detector first in the sample. Calculate the relative atomic mass of the nickel in the sample. Give your answer to one decimal place. Page 2 of 12 Symbol of ion Relative atomic mass
Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
1. An element has the following electronic configuration: [Kr]4d105s25p4(a) What period does it belong to?(b) What is its group number? (Use group numbers from 1 to 18)(c) What kind of element is it? (Main group metal, transition metal, metalloid, nonmetal?)(d) How many unpaired electrons are there in an atom of this element? 3. (a) Which of the following atoms or ions is diamagnetic?Li+ Ni2+ Al Fe2+ Mn3+(b) Which of the following atoms or ions is paramagnetic?C4- S4+ V4+ Se2- Ge4+
Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
Arrange in order of increasing nonmetallic character. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 4 elements V, Ge, and K (b) the Group 5A elements N, As, and Bi Arrange in order of increasing atomic size. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 3 elements Mg, Si, and Ar (b) the Group 2A elements Ca, Ba, and Sr
(a) Identify the number of electrons in the ground-state outer shell of atomic oxygen (atomic number 8).(b) How many electrons are in the ground-state outer shell of fluorine?
( a ) Eva l u a te t h e expre s s i o n s 2 * 1, 2 * 11 + 32,2 * 11 + 3 + 52, and 2 * 11 + 3 + 5 + 72. (b) How do the atomic numbers of the noble gases relate to the numbersfrom part (a)? (c) What topic discussed in Chapter 6 is thesource of the number “2” in the expressions in part (a)?
Write the electron configuration for each element.(a) Cl (b) Si (c) Sr (d) O
(1) What is the valence electron configuration for the neon atom? (2) What is the valence electron configuration for the sulfur atom?

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