(a)
Interpretation:
The electronic configuration of
Concept Introduction:
The fundamental principles that are followed to write an electronic configuration include three rules as follows:
Electron in a
Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.
Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers.
(a)
Answer to Problem 2A.1AST
The electronic configuration of
Explanation of Solution
Copper is a d-block metal that loses it valence electrons to form
After a loss of one electron from the valence
(b)
Interpretation:
The electronic configuration of
Concept Introduction:
Refer to part (a).
(b)
Answer to Problem 2A.1AST
The electronic configuration of
Explanation of Solution
Copper is a d-block metal that loses its valence electrons to form
After loss of two electron from the valence
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Chapter 2 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 1TERM
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- Which of these elements is most likely to form ions with a2+charge?(a) Li (b) Ca (c) O (d) P (e) Clarrow_forwardDiscuss each conclusion from a study of redox reactions:(a) The nitride ion functions only as a reducing agent.(b) The nitrate ion functions only as an oxidizing agent.(c) The nitrite ion functions as an oxidizing or a reducing agentarrow_forwardUse the periodic table to (i) predict electron configurations for the following species: Arsenic ion, As3– Magnesium ion, Mg2+ Vanadium(II) ion, V2+ (ii) Write the electron configurations of each species in the noble gas notation. (iii) Draw an orbital diagram to represent 1 c above. Draw the Lewis electron dot structures of the following chemical species. In each case you must say whether or not the central atom obeys the Octet Rule. CS2 and H2S CF4 and SiH4 NH2Cl CO32– and BF3 PCl5 ClF3, XeF2, Calculate the formal charge on the Sulphur atom in the Sulphate anion structure shown below(picture attatched) Give the electron-pair and molecular geometries for NF3 and XeF4.arrow_forward
- Write the ground state electron configuration for atom and ion pair. Co, Co2+arrow_forwardPredict the ion generally formed by (a) Sr, (b) S, (c) Al.arrow_forwardFor many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains 77.55% Xe and 22.45% F by mass.(a) What is the formula of the compound?(b) Write a Lewis structure for the compound.(c) Predict the shape of the molecules of the compound.(d) What hybridization is consistent with the shape you predicted?arrow_forward
- Write the electron configuration for each of the followingions, and determine which ones possess noble-gasconfigurations: (a) Sr2+, (b) Ti2+, (c) Se2-, (d) Ni2+, (e) Br-,(f) Mn3 + .arrow_forwardChoosing from the elements in the third row of the Periodic Table write out thechemical formula of(i) A basic oxide.(ii) An amphoteric oxide.(iii) An acidic oxidearrow_forward3. Write a chemical equation corresponding to the second ionization energy of calcium.arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,