Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

10. Periodic Properties of the Elements

Periodic Trend: Atomic Radius

General Chemistry

10. Periodic Properties of the Elements

Periodic Trend: Atomic Radius

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following is true?

Be is smaller than Mg due mainly to differences in Z_eff.

Na is larger than Mg due mainly to differences in the principal quantum number.

C is smaller than F due to an increase in the outermost energy levels of electrons.

P is larger than N due primarily to stronger attractions between electrons in the outermost orbitals.

Ca is larger than Mg due to larger orbitals.

Previous problemNext problem

Verified step by step guidance

Step 1: Understand the concept of atomic size and how it is influenced by factors such as effective nuclear charge (Zeff), principal quantum number, and electron shielding.

Step 2: Analyze the statement 'Be is smaller than Mg due mainly to differences in Zeff.' Beryllium (Be) and Magnesium (Mg) are in the same group, and atomic size increases down a group due to additional electron shells, not primarily due to Zeff.

Step 3: Evaluate the statement 'Na is larger than Mg due mainly to differences in the principal quantum number.' Sodium (Na) and Magnesium (Mg) are in the same period, and atomic size decreases across a period due to increased Zeff, not primarily due to principal quantum number.

Step 4: Consider the statement 'C is smaller than F due to an increase in the outermost energy levels of electrons.' Carbon (C) and Fluorine (F) are in the same period, and atomic size decreases across a period due to increased Zeff, not due to changes in energy levels.

Step 5: Assess the statement 'Ca is larger than Mg due to larger orbitals.' Calcium (Ca) and Magnesium (Mg) are in the same group, and atomic size increases down a group due to additional electron shells, which means larger orbitals.