Podcast Beta
Questions and Answers
The Octet Rule states that atoms avoid sharing electron pairs to complete their valence shells.
False
Nitrogen typically has 5 valence electrons and requires 3 additional electrons to complete its octet.
True
PCl5 can accommodate more than 8 electrons around the phosphorus atom due to its larger size.
True
Resonance involves a molecule rapidly shifting between different Lewis structures.
Signup and view all the answers
The 3d orbitals are significantly lower in energy than the 3s and 3p orbitals.
Signup and view all the answers
Boron can form stable compounds with only 6 valence electrons, such as BF3.
Signup and view all the answers
Hydrogen cyanide (HCN) is an example of a compound that exhibits resonance forms.
Signup and view all the answers
The term 'resonance hybrid' refers to a structure that results from the combination of multiple equivalent Lewis structures.
Signup and view all the answers
Sodium chloride (NaCl) is classified as a covalent compound.
Signup and view all the answers
Odd electron molecules can have a total of 11 valence electrons like nitric oxide (NO).
Signup and view all the answers
Resonance hybrids are structures that have multiple resonance forms.
Signup and view all the answers
The bond enthalpy of H2 is measured at + 436 kJ/mol, which indicates an exothermic reaction.
Signup and view all the answers
Multiple bonds are longer than single bonds between the same pair of elements.
Signup and view all the answers
A curly arrow in chemical diagrams represents the movement of a single electron.
Signup and view all the answers
The bond enthalpy of C-O is greater than that of H-O.
Signup and view all the answers
The bond length is influenced by the number of bonds and the atomic radii of the heavy atoms involved.
Signup and view all the answers
Nitrate is represented by the chemical formula SO2.
Signup and view all the answers
The bond enthalpy of F-F is significantly higher than that of Cl-Cl.
Signup and view all the answers
C≡C has a bond strength of 837 kJ/mol, making it one of the strongest bonds listed.
Signup and view all the answers
In covalent bonding, covalent radii increase as you move up a group in the periodic table.
Signup and view all the answers
Study Notes
Lewis Diagrams
- Lewis diagrams illustrate valence electrons of an atom.
- They are used in covalent compounds such as H2O, NH3, CH4, and ionic compounds such as NaCl, MgO, CaCl2.
Covalent Bonds – The Octet Rule
- Atoms share electron pairs to complete their octet.
- Elements in period 2, like C, N, O, and F, have no d-orbitals and cannot have more than 8 electrons around them.
- Elements in period 3 and beyond have empty d-orbitals which can be used for expanded octets, allowing atoms to have more than 8 electrons.
Resonance
- Multiple bonds can be shown in different equivalent locations in a molecule.
- The actual structure is a blend of all resonance forms called a resonance hybrid.
- Examples include nitrate (NO3-) and sulfur dioxide (SO2).
Bond Strength
- Bond strength is measured by bond enthalpy (ΔHB).
- Bond enthalpy is the energy required to break a bond.
- The strength of a bond depends on the adjacent atoms.
Bond Length
- Heavier atoms have larger atomic radii due to more electrons.
- Multiple bonds are shorter than single bonds between the same elements due to increased electron density.
- Covalent radii increase down a group.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
Explore the fundamentals of chemistry with our quiz on Lewis diagrams, covalent bonds, resonance, bond strength, and bond length. This quiz covers essential concepts such as the octet rule and bond enthalpy, providing insights into how atoms interact to form compounds. Test your knowledge and deepen your understanding of molecular structures!
