Atomic Structure Notes Quiz

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Questions and Answers

What is the bond length of a carbon-carbon triple bond?

1.40 pm

1.34 pm

1.54 pm

1.21 pm (correct)

Which statement correctly describes pi-bonds?

They are stronger than sigma bonds.

They are easier to break than sigma bonds. (correct)

They do not contribute to reactivity of compounds.

They are found in saturated compounds.

Which element serves as the coordination center in hemoglobin?

Iron (correct)

Magnesium

Nickel

Copper

Where do ortho and para substituents refer to in relation to a benzene ring?

Adjacent and opposite positions on the ring. Signup and view all the answers

Which complex is associated with a red color formation?

Tetracycline and calcium. Signup and view all the answers

What happens to benzene when an OH group is added?

Resonance implications arise. Signup and view all the answers

What is the bond angle in sp3 hybridization?

109.5° Signup and view all the answers

What is true about pi bonds?

They are formed by the overlapping of orbitals. Signup and view all the answers

How does bond order relate to bond length?

Higher bond order results in shorter bond length. Signup and view all the answers

What is the bond order of the compound NO2?

1.33 Signup and view all the answers

Which of these statements about bond order is correct?

It determines the energy required to break a bond. Signup and view all the answers

In resonance structures, what is the effect on bond order?

Bond order is calculated as total bonds divided by resonating species. Signup and view all the answers

Which theory explains the formation of bonds based on the overlapping of atomic orbitals?

Valence Bond Theory Signup and view all the answers

What type of hybridization involves the mixing of one s orbital and three p orbitals?

sp³ Signup and view all the answers

Which of the following correctly describes a pi bond?

Formed from lateral overlap of p orbitals Signup and view all the answers

In which molecule would you expect to find sp² hybridization?

Ethylene (C₂H₄) Signup and view all the answers

Which of the following statements is true about valence electrons?

They are involved in forming chemical bonds. Signup and view all the answers

What geometry is associated with sp hybridization?

Planar Signup and view all the answers

According to Hund's Rule, how should electrons be filled in orbitals?

Electrons should be filled singly before any pairing occurs. Signup and view all the answers

What does the energy level formula (n+l) indicate about orbital designations?

It establishes the order of filling for different orbitals. Signup and view all the answers

Which of the following is the correct electron configuration for Beryllium?

1s2 2s2 Signup and view all the answers

What occurs when atoms gain electrons?

They become negatively charged anions. Signup and view all the answers

What happens to sodium when it forms a sodium ion (Na+)?

It loses an outermost electron. Signup and view all the answers

Which type of bond is characterized by the sharing of electron pairs?

Covalent bonds Signup and view all the answers

How are elements arranged in the periodic table?

Based on the number of electrons in the outermost shell. Signup and view all the answers

How many orbitals are found in a d subshell?

5 Signup and view all the answers

Which group in the periodic table is characterized as inert?

Group 8 Signup and view all the answers

What is electronegativity?

The power of an atom to accept an electron. Signup and view all the answers

Which bonding type involves the transfer of electrons between atoms?

Ionic bonding Signup and view all the answers

What is a characteristic of coordinate covalent bonds?

One atom provides both electrons for the bond. Signup and view all the answers

What is the charge of zinc in the complex ion [Zn(H₂O)₄]²⁺?

+2 Signup and view all the answers

What type of interaction occurs between organophosphate insecticides and acetylcholinesterase?

Covalent interaction Signup and view all the answers

What is the oxidation state of platinum in the complex [Pt(NH₃)₂Cl(NO₂)]?

+1 Signup and view all the answers

In the complex K₂[PdCl₄], what is the oxidation state of palladium (Pd)?

+2 Signup and view all the answers

What does the K₃[Fe(CN)₅Cl] complex represent?

Iron (III) complex Signup and view all the answers

What is considered the strongest type of chemical bond?

Covalent bond Signup and view all the answers

Which of the following is NOT a characteristic of drugs?

All drugs are natural substances Signup and view all the answers

Which compound is an example of an electron deficient atom?

BF3 Signup and view all the answers

What type of bond does hydrogen bonding exemplify?

Hydrogen bond Signup and view all the answers

Which substance interacts with open wounds to create a peppery sensation?

Iodine in water Signup and view all the answers

In the context of chemical bonding, what does a dative bond involve?

Donation of a lone pair from one atom to another Signup and view all the answers

What is a consequence of the complex formation in drug interactions?

Reduced bioavailability of the drug Signup and view all the answers

What does EDTA primarily detect in compounds like milk?

Magnesium and Calcium Signup and view all the answers

Which of the following is NOT a member of the tetracycline class?

Ciprofloxacin Signup and view all the answers

What type of analysis is indicated by the term 'assay'?

Quantitative Analysis Signup and view all the answers

What characteristic relates to most ligands in coordination chemistry?

They are primarily neutral and negatively charged Signup and view all the answers

What does a negative change of a complex ion indicate regarding its metal naming convention?

The metal name ends with 'ate'. Signup and view all the answers

Which of the following ligands is classified as bidentate?

Ethylene diamine Signup and view all the answers

What is the primary role of chelating agents?

To facilitate quantitative analysis of metals. Signup and view all the answers

Which of the following is NOT a type of bonding interaction listed?

Ionic bonding Signup and view all the answers

What term describes a ligand's ability to form a ring-like structure when bonded to a metal?

Chilite Signup and view all the answers

Which of the following statements about denticity is true?

Denticity refers to the number of donor atoms in a ligand. Signup and view all the answers

What is formed when metals react with ligands?

Complex ion Signup and view all the answers

Which of the following is a characteristic of homoleptic complexes?

They have only one type of ligand. Signup and view all the answers

How is the oxidation number determined in a complex ion?

By the total charge of the entire complex. Signup and view all the answers

What defines a bidentate ligand?

It can form two coordinate bonds to a single metal. Signup and view all the answers

What does the coordination number indicate?

The number of ligands surrounding a central metal atom. Signup and view all the answers

Which of the following is an example of a heteroleptic complex?

[Pt(NH3)2Cl2] Signup and view all the answers

Which ligand is known as 'aqua' when coordinated to a metal?

H2O Signup and view all the answers

What happens to the name of a complex ion if its charge is negative?

The complex ion is named at the end. Signup and view all the answers

Study Notes

Atomic Structure and Electron Configuration

Hund's Rule: Electrons fill orbitals singly before pairing.
Energy Level Rule:
- Defined by the formula (n+l).
- Different orbitals: s (l=0), p (l=1), d (l=2), f (l=3), g (l=4).
- Number of orbitals = 2l + 1; Electrons = 2(2l + 1).
- A maximum of 4l + 2 or 2n^2 electrons for energy levels.
Electronic Configuration:
- Hydrogen: 1s¹, Helium: 1s².
- For Lithium: [He] 2s¹; Beryllium: [He] 2s²; Boron: [He] 2s² 2p¹; Nitrogen: [He] 2s² 2p³; Oxygen: [He] 2s² 2p⁴; Neon: [He] 2s² 2p⁶; Sodium: [Ne] 3s¹.

Ion Formation and Group Characteristics

Ion Formation:
- Example: H₂O + H⁺ → H₃O⁺ involves lone pair electrons.
- Group 1, 2, 3 elements prefer losing outermost electrons.
Periodic Table Groups:
- Group 8 is inert, while groups 5, 6, 7 are reactive.

Theories of Chemical Bonding

Molecular Bond Theory: Atomic orbitals combine to form molecules through mixing.
Valence Bond Theory: Only valence electrons (outer shell) participate in reactions; overlapping of atomic orbitals forms bonds.

Hybridization and Bond Types

Hybridization:
- Mixing of atomic orbitals to form equivalent orbitals.
- Examples:
  - sp³ (tetrahedral),
  - sp² (trigonal planar),
  - sp (linear).
Pi Bonds: Formed from overlapping orbitals. Sigma bonds precede pi bonds.

Bond Energies and Reactions

Bond Lengths:
- CH₄ (1.54 pm), C=C (1.34 pm), C≡C (1.21 pm).
- Sigma bonds are stronger and require more energy to break than pi bonds.
Resonance: Bond order indicates reactivity and can yield fractional values in cases of resonance (e.g., NO₂ has a bond order of 1.33).

Chemical Bonding Basics

Bonds can be ionic or covalent (including ordinary and coordinate covalent).
Electronegativity: Measure of an atom’s ability to attract electrons, critical in determining bond types.

Coordination Chemistry

Complex ions consist of a metal ion bonded to ligands; can be homoleptic (one type of ligand) or heteroleptic (multiple types).
Ligands: Can be unidentate, bidentate, or polydentate based on the number of donor atoms.
Coordination Number: Represents the number of ligands surrounding a metal ion.

Drug Interactions and Applications

Tetracycline: A drug that interacts with calcium, leading to reduced bioavailability when taken with dairy products.
EDTA: Chelating agent used for detecting metals and treating lead poisoning.
Chemical Interactions: Various types influence medicinal chemistry and drug design, including covalent interactions.

Additional Notes

Coordination Compounds: Formed from metals, primarily transition metals, and ligands. Naming depends on the charges and types of ligands.
Dative Bonds: Formed when an electron-deficient atom accepts an electron pair from another atom, creating strong bonds.
Electron Deficient Atoms: Examples include BF₃ and BeCl₂, which can form coordinate bonds through their electron deficiency.

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Test your knowledge of atomic structure concepts, including Hund's Rule, Energy Level Rule, and Electronic Configuration.