(a)
Interpretation:
The element with the largest atomic radius in group 2A is to be determined.
Concept Introduction:
In periodic table elements are arranged in increasing order of their
(b)
Interpretation:
The element with the smallest atomic radius in group 2A is to be stated.
Concept Introduction:
In periodic table elements are arranged in increasing order of their atomic number, there are total 18 columns and 7 rows in periodic table, elements of each column show similar properties.
(c)
Interpretation:
The element with the largest atomic radius in 2nd period is to be stated.
Concept Introduction:
In periodic table elements are arranged in increasing order of their atomic number, there are total 18 columns and 7 rows in periodic table, elements of each column show similar properties.
(d)
Interpretation:
The element with the largest atomic radius in second period is to be stated.
Concept Introduction:
In periodic table elements are arranged in increasing order of their atomic number, there are total 18 columns and 7 rows in periodic table, elements of each column show similar properties.
(e)
Interpretation:
The element in group 7A with the largest ionization energy is to be determined.
Concept Introduction:
In periodic table elements are arranged in increasing order of their atomic number, there are total 18 columns and 7 rows in periodic table, elements of each column show similar properties.
Ionization energy is measure of how difficult it is to remove the most loosely held electron from an atom in the gaseous state, higher the difficulty in removing the atom; higher will be the ionization energy.
(f)
Interpretation:
The element in the group 7A with the smallest ionization energy is to be stated.
Concept Introduction:
In periodic table elements are arranged in increasing order of their atomic number, there are total 18 columns and 7 rows in periodic table, elements of each column show similar properties.
Ionization energy is measure of how difficult it is to remove the most loosely held electron from an atom in the gaseous state, higher the difficulty in removing the atom; higher will be the ionization energy.
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Introduction to General, Organic and Biochemistry
- 2-89 Assume that a new element has been discovered with atomic number 117. Its chemical properties should be similar to those of astatine (At). Predict whether the new element’s ionization energy will be greater than, the same as, or smaller than that of: (a)At (b)Raarrow_forwardArrange in order of increasing atomic size (a) the Period 2 Elements C, Ne, and Be(b) the Group 4A elements Si, Pb, and Gearrow_forwardQ2. 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.arrow_forward
- Write the electron configuration for each element.(a) Cl (b) Si (c) Sr (d) Oarrow_forwardHow is the periodic Table arranged? (A) Horizontally ( B) Vertically (C) Atomic Mass. (D) Periods and Groupsarrow_forward1. 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+arrow_forward
- 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 massarrow_forward(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?arrow_forwardBoron, 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?arrow_forward
- Which one has the largest atomic radius? (A) Be (B) Mg (C) Ca (D) Ba Which one has the largest atomic radius? (A) Li (B) C (C) N (D) Oarrow_forwardThe graph at the right shows the atomic radius for the19 elements in the periodic table.(a) Describe the trend in atomic radius in going fromH (atomic number 1) to K (atomic number 19).(b) Find the three elements represented with blue dotson a periodic table. What do their placements in thetable have in common?(c) Find the three elements represented with red dotson a periodic table. What do their placements in thetable have in common?(d) Based on the graph, what is the radius of C?arrow_forwardBoron, 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?arrow_forward
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