(a)
Interpretation:
The formula of simplest binary hydride of each element mentioned in given periodic table has to be written.
Concept Introduction:
The compound containing hydrogen and just one other element is called binary hydride. Type of hydride formed depends upon the element present in the group. Types of binary compounds are, ionic hydride, metallic hydride and covalent hydride.
Ionic hydride: Ionic hydrides are formed by alkali metals and heavier alkaline earth metals. They contain cations and
Covalent hydride: Covalent hydrides are formed by non-metals. The compound contains hydrogen which is bonded to another element by covalent bond. Most of the covalent hydrides have relatively weak intermolecular force of attraction, so they are gas or volatile liquid at normal temperature.
Metallic hydride: Metallic hydrides are formed by
(b)
Interpretation:
The hydride has lowest boiling point should be identified.
Concept Introduction:
The compound containing hydrogen and just one other element is called binary hydride. Type of hydride formed depends upon the element present in the group. Types of binary compounds are, ionic hydride, metallic hydride and covalent hydride.
Ionic hydride: Ionic hydrides are formed by alkali metals and heavier alkaline earth metals. They contain cations and
Covalent hydride: Covalent hydrides are formed by non-metals. The compound contains hydrogen which is bonded to another element by covalent bond. Most of the covalent hydrides have relatively weak intermolecular force of attraction, so they are gas or volatile liquid at normal temperature.
Metallic hydride: Metallic hydrides are formed by transition metals, lanthanides and actinide metals in which hydrogen will be present in variable amount. Metallic hydride has general formula of
(c)
Interpretation:
The one hydride that gives hydrogen gas on reaction with water has to be predicted and also the balanced net ionic equation for the reaction has to be written.
Concept Introduction:
The compound containing hydrogen and just one other element is called binary hydride. Type of hydride formed depends upon the element present in the group. Types of binary compounds are, ionic hydride, metallic hydride and covalent hydride.
Ionic hydride: Ionic hydrides are formed by alkali metals and heavier alkaline earth metals. They contain cations and
Covalent hydride: Covalent hydrides are formed by non-metals. The compound contains hydrogen which is bonded to another element by covalent bond. Most of the covalent hydrides have relatively weak intermolecular force of attraction, so they are gas or volatile liquid at normal temperature.
Metallic hydride: Metallic hydrides are formed by transition metals, lanthanides and actinide metals in which hydrogen will be present in variable amount. Metallic hydride has general formula of
(d)
Interpretation:
Among the given hydrides, on reaction with water, the hydride that gives acidic solution and the hydride giving basic solution has to be predicted.
Concept Introduction:
The compound containing hydrogen and just one other element is called binary hydride. Type of hydride formed depends upon the element present in the group. Types of binary compounds are, ionic hydride, metallic hydride and covalent hydride.
Ionic hydride: Ionic hydrides are formed by alkali metals and heavier alkaline earth metals. They contain cations and
Covalent hydride: Covalent hydrides are formed by non-metals. The compound contains hydrogen which is bonded to another element by covalent bond. Most of the covalent hydrides have relatively weak intermolecular force of attraction, so they are gas or volatile liquid at normal temperature.
Metallic hydride: Metallic hydrides are formed by transition metals, lanthanides and actinide metals in which hydrogen will be present in variable amount. Metallic hydride has general formula of
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General Chemistry: Atoms First
- Which is the stronger acid, H2SO4 or H2SeO4? Why? You may wish to review the Chapter on acid-base equilibria.arrow_forwardComplete and balance the following equations:(a) A salt like (alkaline earth metal) hydride reacting with water,CaH₂(s)+H₂O(l)→ (b) Reduction of a metal halide by hydrogen to form a metal,PdCl₂(aq)+H₂(g)→arrow_forwardSelenium is prepared by the reaction of H₂SeO₃ with gaseous SO₂. (a) What redox process does the sulfur dioxide un-dergo? What is the oxidation state of sulfur in the product? (b) Given that the reaction occurs in acidic aqueous solution,what is the formula of the sulfur-containing species? (c) Write the balanced redox equation for the processarrow_forward
- (i) The acidic character of hydrides of group 15 increases from H2O toH2Te. Why?(ii) Dioxygen is a gas while sulphur (S8) is a solid. Why?arrow_forward(a) A alkali metals react withhydrogen to form hydrides and react with halogens to formhalides. Compare the roles of hydrogen and halogens inthese reactions. Write balanced equations for the reaction offluorine with calcium and for the reaction of hydrogen withcalcium. (b) What is the oxidation number and electronconfiguration of calcium in each product?arrow_forward(a) Which poisonous gas is evolved when white phosphorus is heated with Cone. NaOH solution? Write the chemical equation. (b) Write the formula of first noble gas compound prepared by N. Bartlett. What inspired N. Bartlett to prepare this compound? (c) Fluorine is a stronger oxidising agent than chlorine. Why? (d)Write one use of chlorine gas.arrow_forward
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- (a) One of the alkali metals reacts with oxygen to form a solidwhite substance. When this substance is dissolved in water,the solution gives a positive test for hydrogen peroxide, H2O2.When the solution is tested in a burner flame, a lilac-purpleflame is produced. What is the likely identity of the metal?(b) Write a balanced chemical equation for the reaction ofthe white substance with water.arrow_forwardWrite a balanced equation for the reaction of elemental strontium with each of the following:(a) oxygen(b) hydrogen bromide(c) hydrogen(d) phosphorus(e) waterarrow_forwardWrite a balanced equation for the reaction of elemental boron with each of the following (most of these reactions require high temperature): (a) F2 (b) O2arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax