General Chemistry

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Questions and Answers

What is a characteristic of hypervalent compounds?

They utilize empty d orbitals for bonding. (correct)

They can only form with period 2 elements.

They can only exist as ionic compounds.

They always follow the octet rule.

Which factor has the least influence on the covalent character of ionic bonds?

Electronegativity of the anion (correct)

Charge of the cation

Size of the anion

Size of the cation

Which statement best describes the octet rule?

The octet rule applies solely to noble gases.

Atoms cannot exceed an outer shell of 8 electrons.

All elements obey the octet rule including transition metals.

Atoms aim for a full outer shell of 8 electrons. (correct)

How does a small cation affect its ionic bond with an anion?

It attracts the anion's electrons more strongly. (A) Signup and view all the answers

What is the relationship between electronegativity difference and ionic character in covalent molecules?

Greater electronegativity difference leads to greater ionic character. (A) Signup and view all the answers

Which property is characteristic of ionic compounds in their solid state?

They are poor conductors of electricity. (A) Signup and view all the answers

What is the main characteristic of metallic bonding?

Attraction between cations and a sea of delocalized electrons. (A) Signup and view all the answers

What does the octet rule state regarding electron configuration?

Atoms gain, lose, or share electrons to achieve eight valence electrons. (C) Signup and view all the answers

Which statement about covalent compounds is true?

They typically have low melting and boiling points. (D) Signup and view all the answers

What is the main difference between ionic and covalent bonding?

Covalent bonding involves sharing electrons, while ionic bonding involves transferring electrons. (D) Signup and view all the answers

Which of the following best describes electron-deficient molecules?

They do not achieve an octet due to a shortage of electrons. (D) Signup and view all the answers

Which of the following is an example of a hypervalent molecule?

PCl5 (C) Signup and view all the answers

What happens to ionic compounds when they are melted?

They conduct electricity due to free-moving ions. (A) Signup and view all the answers

What is the primary reason metals are good conductors of electricity?

Metals have delocalized electrons that move freely. (A) Signup and view all the answers

Which property of metallic bonding explains why metals are malleable?

The overlapping of atomic orbitals allows layers to slide. (B) Signup and view all the answers

Which statement correctly describes an exception to the octet rule?

Hypervalent molecules have a central atom with more than eight electrons. (B) Signup and view all the answers

Which of the following is true about ionic compounds formed by metals?

Ionic compounds are primarily formed when metals lose electrons. (A) Signup and view all the answers

What defines an electron-deficient molecule?

A molecule that lacks sufficient electrons for a noble gas configuration. (C) Signup and view all the answers

What is a distinguishing characteristic of covalent bonds compared to ionic bonds?

Covalent bonds are typically weaker than ionic bonds. (D) Signup and view all the answers

Which factor primarily contributes to the shiny appearance of metals?

Electrons oscillating at the atomic level. (B) Signup and view all the answers

Which of the following statements is true regarding the bonding behavior of metals?

Metals lose electrons and form positive ions. (C) Signup and view all the answers

Study Notes

Course Information

Course: HNDT 1001 - General Chemistry for Nutrition
Lecturer: Keisha Mascoll
Semester: 1 2024/2025

Class Attendance

All students must scan the QR code and complete required fields for class attendance.
Download a QR code reader app (App Store or Google Play Store) if device is incompatible.

Course Meeting Times and Location

Lecture: Thursday 1:00 PM - 3:00 PM - MSR3
Lab: Thursday 3:00 PM - 5:00 PM - MLTC (lab)
Tutorial: Friday 9:00 AM - 10:00 AM - MSR3

Course Rubric

Mode of Delivery: Face-to-face
Laboratory Session: Face-to-face
Labs: 5, 25% weight, 5 weekly written reports on lab work assignments
Quizzes: 2, 20% weight, multiple choice, short answer, & calculations. 1.5 hours
Mid-Term Test: 1, 15% weight, multiple choice, short answer, & calculations, 1.5 hours
Final Examination: 1, 40% weight, multiple choice, short answer, & calculations, 2 hours

Test Dates

Quiz 1: Friday, October 4th, 2024, 1 hour, closed book
Mid-term: Thursday, October 24th, 2024, 1 hour 30 minutes, closed book
Quiz 2: Thursday, November 14th, 2024, 1 hour, closed book

Laboratory Schedule

Week 4, Lab #1: Mole Ratio & Reaction Stoichiometry, Date: 26th September 2024
Week 8, Lab #2: Titration of Acids & Bases, Date: 24th October 2024
Week 10, Lab #3: Determination of Equilibrium Constant, Date: 7th November 2024
Week 11, Lab #4: Calorimetry, Date: 14th November 2024
Week 12, Lab #5: Worksheet, Date: 21st November 2024

Required/Essential Text

Blackman, A., et al. (2019). Chemistry (4th ed.). New Jersey: John Wiley & Sons.
ISBN-13: 978-0730363268, ISBN-10: 0730363287
McMurry, J., et al. (2016). Fundamentals of General, Organic and Biological Chemistry (8th ed.). London: Pearson. ISBN-13: 978-0134015187, ISBN-10: 0134015185
Petrucci, R., et al. (2016). General Chemistry: Principles and Modern Applications (11th ed.). London: Pearson. ISBN-13: 978-0132931281, ISBN-10: 0132931281

Learning Outcomes

Describe the atom's structure (protons, neutrons, electrons), relative charges, and masses.
Use chemical symbols to express isotopes' subatomic compositions, using atomic numbers and mass numbers.
Describe the periodic table's organization by atomic number and chemical behavior (periods and groups).
Identify locations of metals and nonmetals in the periodic table.
Review electronic configurations.
Differentiate between molecular and ionic substances.
Explain ion formation (electron gain/loss) and predict common ion charges.

Topics

Atomic Number & Mass Numbers
Isotopes
Periodicity
Chemical Bonding
Covalent Bonding
Ionic Bonding
Metallic Bonding
Valence
Octet Rule
Ionic vs. Covalent Bonding

Atomic & Molecular Prospective

Matter: atoms, ions, or molecules.
Atom: smallest part of an element or compound that participates in chemical reactions.
Molecule: groups of atoms held together with a specific connectivity and shape.
Matter classified by: State (gas, liquid, solid), Composition (element, compound, mixture).

Elements, Compounds & Mixtures

Pure Substance: fixed composition and distinct properties.
Elements: identical atoms, e.g., oxygen (O2), gold (Au), silicon (Si), diamond (C).
Compounds: more than one type of atom bonded, e.g., water (H2O), ethanol (C2H6O), sodium chloride (NaCl).
Mixtures: variable composition, separable into components, properties depending on component amounts.

Molecular View of Elements & Compounds

Classification of elements and compounds.
Diagram showing atomic and molecular views of elements and compounds (e.g. Ne, O2, H2O, NaCl).

Homogeneous & Heterogeneous Mixtures

Homogeneous Mixture: uniform throughout (e.g., air, coffee, vodka, blood, brass).
Heterogeneous Mixture: non-uniform throughout (e.g., smog, ice cubes in drink, sand in water, concrete).

Structure of the Atom

Protons (positive charge, mass 1), Neutrons (neutral charge, mass 1), Electrons (negative charge, negligible mass).
Protons and neutrons located in nucleus, electrons orbit the nucleus.

Atomic & Mass Numbers

Mass Number: sum of protons and neutrons.
Atomic Number: number of protons (or electrons).

Isotopes

Isotopes: atoms of the same element with different masses due to different neutron numbers.

Uses of Isotopes

Stable isotopes used in nutritional studies.
Practical applications: calcium and iron absorption, diet, physical activity, aging, medical therapy, nutrient metabolism, pregnancy energy cost, growth faltering, childhood and adult obesity.
Isotopes utilized for metabolic studies, body composition assessment, and protein turnover.

Periodicity

Elements arranged in periodic table by increasing atomic number, similar properties grouped together.
Major classifications of elements: Main group (representative), transition metals, metalloids.

Major Classifications of Elements

Main group elements: alkali metals, alkaline earth metals, halogens, noble gases.
Transition metals.
Metalloids.

Trends in the Periodic Table

Trends of atomic radius, electron affinity, ionization energy, electronegativity.
Trends across periods and groups.

Relative Abundance of Elements in the Human Body

Human body comprised of ~ 99% of 6 elements (O, C, H, N, Ca, P) and a further 5 elements (S, K, Na, Cl, Mg), with ~0.15% of the rest being trace elements.

The Electronic Configuration of Atoms

Aufbau Principle: electrons fill orbitals of lowest energy levels first.
Pauli Exclusion Principle: an orbital can hold a maximum of 2 electrons with opposite spins.
Hund's Rule: orbitals with the same energy are singly occupied before pairing occurs.

Shapes and Symmetry of Atomic Orbitals

Atomic orbitals have specific shapes and symmetry.
S orbital: spherical symmetry.
P orbital: dumbbell shape, with two lobes.
D orbital: more complex shapes.

Chemical Bonds

Bond: force of attraction between oppositely charged particles.
Covalent Bond: sharing of valence electrons between atoms.
Ionic Bond: complete transfer of electrons from one atom to another.
Metallic Bond: overlap of orbitals extending over three dimensions (3D) with delocalized electrons.

Covalent Bonding

Sharing of valence electrons between atoms.
Resulting molecules are product of covalent bonds, typically occurring between nonmetals.
Different types of covalent bonds: single, double, triple bonds.

Properties of Covalent Compounds

Low melting and boiling points.
Poor conductors of electricity.
Generally not soluble in water.

Ionic Bonding

Complete transfer of electrons between a metal and a nonmetal.
Formation of ions (cations (+) and anions (-) )
Electrostatic force of attraction between oppositely charged ions.

Properties of Ionic Bonding

High melting points.
Poor electrical conductivity in solid state.
Conduct electricity in molten or aqueous solution.

Metallic Bonding

Overlapping of atomic orbitals in three dimensions.
Delocalized electrons throughout the structure.
Metals generally lose electrons to become positively charged cations.
Tend to form ionic compounds with nonmetals.

Octet Rule

Main group elements tend to form compounds by either gaining or losing electrons to achieve 8 valence electrons.

Exceptions to the Octet Rule

Electron-deficient molecules: central atom has fewer electrons than normal.
Hypervalent molecules: central atom has more electrons than normal.
Odd-electron molecules: odd number of valence electrons, so electron is unpaired.

Ionic Bonding & Covalent Bonding

Few compounds are 100% ionic or covalent.
Ionic character depends on electronegativity difference.
Covalent character in ionic compounds influenced by cation/anion size and charge.

Review Topics

Atomic Structure & Composition, Periodic Table and its classifications.
Characteristics of Metals, Non-metals, and Metalloids, Chemical Formulas, Chemical Nomenclature.
Common Monoatomic Ions, Common Polyatomic Ions, Formula of Compounds.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Description

This quiz focuses on key concepts from Chapter 2 of chemistry, including hypervalent compounds, ionic bonds, and the octet rule. Test your understanding of these fundamental principles and how they relate to ionic character and electronegativity. Perfect for students looking to reinforce their chemistry knowledge!