Complete the following table: BEST Lewis structure NH4+ Draw Lewis structure: VSEPR Formula for central atom: _________________________ SOF2 Draw Lewis structure: VSEPR formula for central atom: __________________________ XeF2 Draw Lewis structure: VSEPR formula for central atom: ________________________ H2SO3 Draw Lewis structure: VSEPR formula for central atom
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
(a) Complete the following table:
BEST
Lewis structure
NH4+
Draw Lewis structure:
VSEPR Formula for central atom: _________________________
SOF2
Draw Lewis structure:
VSEPR formula for central atom: __________________________
XeF2
Draw Lewis structure:
VSEPR formula for central atom: ________________________
H2SO3
Draw Lewis structure:
VSEPR formula for central atom: ________________________
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(b) (i) In general, for what two kinds of substances do we draw Lewis structures?
______________________________________
______________________________________
(ii) Complete the following Lewis structure and answer the questions below it.
C
H
N
H
C O
O
C C N
H H
H
H
What is the empirical formula of this compound? __________________________________
How many lone pairs of electrons that this compound have? __________________________
How many multiple bonds does this compound have? _______________________________
How many nonbonding electrons does this compound have? __________________________
How many molecules are in 15.0 mg of this compound? _____________________________
How many bonding pairs of electrons does this compound have? ______________________
How many polar bonds does this compound have? __________________________________
What is the VSEPR formula for the nitrogen atom at the end of the molecule? ____________
(iii)
according to _____________________________________
Chemical bonds are also classified as multiple or _________________________ according to
______________________________ .
(c) Write a ground-state electron configuration for each of the following substances:
(i) Mo ___________________________________________________
(ii) Iron(III) ion ___________________________________________________
(iii) Ca ___________________________________________________
(iv) Hydride ion ___________________________________________________
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(d) (i) Give names of the four quantum numbers for an electron in an atom:
________________________________________________
________________________________________________
________________________________________________
________________________________________________
(ii) Give a list of the 4d-orbitals: __________________________________________________
(iii) What is the maximum number of electrons in an atom that can have the following quantum
numbers:
n = 5, mℓ = 1, ms = +½ _______________________________
n = 4, ℓ = 3, mℓ = 1 _______________________________
n = 3, ms = +½ _______________________________
n = 5, ℓ = 2, mℓ = 1, ms = –½ _______________________________
n = 4, ℓ = –3, mℓ = +1 _______________________________
n = 4, ℓ = 2, ms = +½ _______________________________
(iv) Draw a 2px orbital and describe it.
QUESTION 2
An unknown electronic transition in the H atom begins from n = 3 and it has an energy of +129.6 kJ/mol.
(i) Calculate the final energy level for this electronic transition.
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(ii) Determine the wavelength (in Å) of the radiation associated with this electronic transition.
Specifically, what type of radiation is this? Explain.
QUESTION 3
Which one of the following bonds has the highest polarity?
A. C–O
B. N–F
C. O–N
D. C–H
E. N–H
QUESTION 4
Which one of the following orbital designations is INCORRECT?
A. 5d
B. 2s
C. 3f
D. 7s
E. 3p
QUESTION 5
Which one of the following elements is classified WRONGLY?
A. Zn – a d-block element
B. Sr – a main-group element
C. Na – an alkali metal
D. Xe – an inert noble gas
E. Se – a chalcogen
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QUESTION 6
Which one of the following electronic transitions in the H atom represents absorption of visible light with the shortest wavelength?
A. n = 6 → n = 2
B. n = 2 → n = 3
C. n = 2 → n = ∞
D. n = 2 → n = 4
E. n = 1 → n = 6
QUESTION 7
How many radial nodes does a 5dxy orbital have?
A. 1
B. 2
C. 3
D. 4
E. 5
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