(a) Interpretation: Whether the hydrogen present as H + , H − or a covalently bonded H in MgH 2 should be determined. Concept introduction: The location of each element in the periodic table determines the formula of the hydride it forms. Alkali metals form ionic hydrides and have the formula AH . Transition elements form interstitial hydrides and have no definite stoichiometric formula, AH x . Covalent hydrides are formed by nonmetals and the formula depends on their group in the periodic table.
(a) Interpretation: Whether the hydrogen present as H + , H − or a covalently bonded H in MgH 2 should be determined. Concept introduction: The location of each element in the periodic table determines the formula of the hydride it forms. Alkali metals form ionic hydrides and have the formula AH . Transition elements form interstitial hydrides and have no definite stoichiometric formula, AH x . Covalent hydrides are formed by nonmetals and the formula depends on their group in the periodic table.
Solution Summary: The author explains that the location of each element in the periodic table determines the formula of the hydrogen it forms.
Definition Definition Elements containing partially filled d-subshell in their ground state configuration. Elements in the d-block of the periodic table receive the last or valence electron in the d-orbital. The groups from IIIB to VIIIB and IB to IIB comprise the d-block elements.
Chapter 22, Problem 22.58SP
Interpretation Introduction
(a)
Interpretation:
Whether the hydrogen present as H+, H− or a covalently bonded H in MgH2 should be determined.
Concept introduction:
The location of each element in the periodic table determines the formula of the hydride it forms. Alkali metals form ionic hydrides and have the formula AH. Transition elements form interstitial hydrides and have no definite stoichiometric formula, AHx. Covalent hydrides are formed by nonmetals and the formula depends on their group in the periodic table.
Interpretation Introduction
(b)
Interpretation:
Whether the hydrogen present as H+, H− or a covalently bonded H in PH3 should be determined.
Concept introduction:
The location of each element in the periodic table determines the formula of the hydride it forms. Alkali metals form ionic hydrides and have the formula AH. Transition elements form interstitial hydrides and have no definite stoichiometric formula, AHx. Covalent hydrides are formed by nonmetals and the formula depends on their group in the periodic table.
Interpretation Introduction
(c)
Interpretation:
Whether the hydrogen present as H+, H− or a covalently bonded H in KH should be determined.
Concept introduction:
The location of each element in the periodic table determines the formula of the hydride it forms. Alkali metals form ionic hydrides and have the formula AH. Transition elements form interstitial hydrides and have no definite stoichiometric formula, AHx. Covalent hydrides are formed by nonmetals and the formula depends on their group in the periodic table.
Interpretation Introduction
(d)
Interpretation:
Whether the hydrogen present as H+, H− or a covalently bonded H in HBr should be determined.
Concept introduction:
The location of each element in the periodic table determines the formula of the hydride it forms. Alkali metals form ionic hydrides and have the formula AH. Transition elements form interstitial hydrides and have no definite stoichiometric formula, AHx. Covalent hydrides are formed by nonmetals and the formula depends on their group in the periodic table.
The elements sodium, aluminum, and chlorine are in the same period.(a) Which has the greatest electronegativity?(b) Which of the atoms is smallest?(c) Write the Lewis structure for the simplest covalent compound that can form between aluminum and chlorine.(d) Will the oxide of each element be acidic, basic, or amphoteric?
Complete and balance the following acid-base equations:(a) A solution of HClO4 is added to a solution of LiOH.(b) Aqueous H2SO4 reacts with NaOH.(c) Ba(OH)2 reacts with HF gas.
Magnesium reacts with oxygen to form magnesium oxide according to the
following reaction:
2 Mg
+ O2
2M9O
(a)
What is the oxidation state of magnesium in Mg?
(b)
What is the oxidation state of magnesium in MgO?
(c)
Which species is oxidized?
(d)
Which species is reduced?
(e)
Name the oxidizing agent.
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