Concept explainers
(a)
Interpretation:
The shape of
Concept introduction:
Hybridization means the formation of new hybrid orbitals by the mixing and merging of atomic orbitals. All hybrid orbitals energy is same.
(b)
Interpretation:
The shape of
Concept introduction:
Hybridisation means the formation of new hybrid orbitals by the mixing and merger of atomic orbitals. All hybrid orbitals energy is same.
(c)
Interpretation:
The shape of
Concept introduction:
Hybridisation means the formation of new hybrid orbitals by the mixing and merger of atomic orbitals. All hybrid orbitals energy is same.
(d)
Interpretation:
The shape of
Concept introduction:
Hybridisation means the formation of new hybrid orbitals by the mixing and merger of atomic orbitals. All hybrid orbitals energy is same.
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General Chemistry: Atoms First
- Write the Lewis structure for each of the following species,describe its geometry, and indicate the oxidation state ofthe nitrogen: (a) NH4+, (b) NO2- , (c) N2O, (d) NO2.arrow_forwardCompounds such as NaBH₄, Al(BH₄)₃, and LiAlH₄ arecomplex hydrides used as reducing agents in many syntheses.(a) Give the oxidation state of each element in these compounds.(b) Write a Lewis structure for the polyatomic anion in NaBH₄,and predict its shape.arrow_forward(i) Interhalogen compounds are more reactive than halogens exceptF2. Why?(ii) Give one important use of ClF3.arrow_forward
- Borane (BH3) is unstable under normal conditions, but it has been detected at lowpressure.(a) Draw the Lewis structure for borane.(b) Draw a diagram of the bonding in BH3, and label the hybridization of each orbital.(c) Predict the H¬B¬H bond anglearrow_forward4. (a) Draw the shape of the atomic valence orbitals formed by the overlaping of two fluoride 2p atomic orbitals. (b) Draw the molecular orbital diagrams for F2 and F2*. Identify their bond order and magnetic properties. (c) An unstable nucleus exhibit radioactivity. (i) Explain how the number of protons and neutrons in a radioactive nucleus can be used to predict its probable mode decay. (ii) Illustrate your answer in (i) with a schematic graph.arrow_forwardA molecular property of the Group 6A(16) hydrides changes abruptly down the group. This change has been ex-plained in terms of a change in orbital hybridization.(a) Between what periods does the change occur?(b) What is the change in the molecular property?(c) What is the change in hybridization?(d) What other group displays a similar change?arrow_forward
- (c) Suggest how the following boron species could be prepared, showing any intermediates. -B(OH)2 B(OH)2arrow_forwardDescribe the molecular structure of each of the following molecules or ions listed. (a) PH3(b) PH4+(c) P2H4(d) PO43−arrow_forwardWhat is the formal oxidation state of chlorine in ammonium perchlorate, NH4ClO4?arrow_forward
- Selenium 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_forwardCompounds such as NaBH4, Al(BH4)3, and LiAlH4 are complex hydrides used as reducing agents in many syntheses. (a) Give the oxidation state of each element in these compounds. (b) Write a Lewis structure for the polyatomic anion in NaBH4, and predict its shape.arrow_forwardThe elements sodium, aluminum, and chlorine are in the same period. (a) Which has the greatest electronegativity? (b) Which of the atoms is smallest? (c) Which is the largest possible oxidation state for each of these elements? (d) Will the oxide of each element in the highest oxidation state (write its formula) be acidic, basic, or amphoteric?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning