Interpretation:
The masses of iron and
Concept Introduction:
The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of
Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:
Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.
Answer to Problem 8.105QE
Explanation of Solution
The
According to the balanced chemical equation, one mole of
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Chapter 8 Solutions
Chemistry: Principles and Practice
- Indicate whether each of the following statements is trueor false (a) H2(g) and D2(g) are allotropic forms of hydrogen.(b) ClF3 is an interhalogen compound. (c) MgO(s) isan acidic anhydride. (d) SO2(g) is an acidic anhydride.(e) 2 H3PO4(l)----> H4P2O7(l) + H2O(g) is an example ofa condensation reaction. (f) Tritium is an isotope of theelement hydrogen. (g) 2SO2(g) + O2(g)---> 2SO3(g) is anexample of a disproportionation reaction.arrow_forwardhow can you diffrentiate between lanthanides and actinides ?arrow_forwardWhat is the formal oxidation state of chlorine in ammonium perchlorate, NH4ClO4?arrow_forward
- Given a hypothetical element, X, which forms two oxides: X203 and XO2. The oxide X2O3 is a reducing agent while XO2 is an oxidizing agent. Which of the following statements best explains the chemical behavior of these oxides? a) The higher oxidation state of X in XO2 makes it a stronger reducing agent. b) The lower oxidation state of X in X2O3 indicates it donates electrons more readily, acting as a reducing agent. c) XO2 acts as a reducing agent because it has a higher oxygen content. d) The presence of more oxygen atoms in X203 makes it a better oxidizing agent. Uploading 3 rd time. Again and again got ai answer. Please provide valuable answerarrow_forwardExplain the following :(a) The enthalpies of atomization of transition metals are quite high.(b) The transition metals and many of their compounds act as good catalysts.arrow_forwardSolid Mg2B205 contains the "pyroborate" anion. Draw the structure for this ion. What are other isoelectronic species? asap please.arrow_forward
- Iron(II) fumerate (also called ferrous fumerate) is prescribed for patients suffering from iron- deficiency anaemia. Sketch the chemical structure of iron(II) fumerate.arrow_forwardDefine actinidesarrow_forwardDespite the expected decrease in atomic size, there is an un-expected drop in the first ionization energy between Groups2A(2) and 3A(13) in Periods 2 through 4. Explain this pattern interms of electron configurations and orbital energies.arrow_forward
- Which group(s) of the periodic table is (are) described byeach of the following general statements?(a) The elements form compounds of VSEPR class AX₃E.(b) The free elements are strong oxidizing agents and formmonatomic ions and oxoanions.(c) The atoms form compounds by combining with two otheratoms that donate one electron each.(d) The free elements are strong reducing agents, show only onenonzero oxidation state, and form mainly ionic compounds.(e) The elements can form stable compounds with only threebonds, but as a central atom, they can accept a pair of electronsfrom a fourth atom without expanding their valence shell.(f) Only larger members of the group are chemically activearrow_forwardWhat is the basis in assigning a central atom?arrow_forwardArrange the following elements in order of increasing the first ionizination energy :Na,K,Clarrow_forward
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