bonding + structure

Question 1

What is Ionic Bonding?

Answer 1

Ionic Bond: Electrostatic attraction between oppositely charged ions.

Question 2

How do metals behave in Ionic Bonding?

Answer 2

Metals lose outer electrons to achieve noble gas structure and form positive ions (cations).

Group 1: 1+ ions, Group 2: 2+ ions, Group 3: 3+ ions. Exceptions: Transition metals may form variable charges.

Question 3

How do non-metals behave in Ionic Bonding?

Answer 3

Non-metals gain electrons to achieve noble gas structure and form negative ions (anions).

Group 7: 1- ions, Group 6: 2- ions, Group 5: 3- ions. Non-metal ions end in -ide (e.g., oxide, chloride).

Question 4

What is required for Ionic Compound Formation?

Answer 4

Charges on ions must cancel out for overall neutrality.

• only show outer shells unless told otherwise

Question 5

What is Covalent Bonding?

Answer 5

Covalent Bond: Attraction between a nucleus and a shared pair of electrons.

Question 6

What are exceptions to the Octet Rule?

Answer 6

• BF3: Boron stable with 6 electrons; group 3 elements can make only 3 bonds.
• Expanding the octet- atoms in period 3 or higher (eg. PCl5) can hold more than 8 electrons due to 3rd shell

Question 7

What are multiple covalent bonds?

Answer 7

Single bond: One pair of electrons shared.
Double bond: Two pairs shared (e.g., O2).
Triple bond: Three pairs shared (e.g., N2).

Question 8

What are the key properties of Ionic Compounds?

Answer 8

• High melting and boiling points due to strong ionic bonds.
• Solid does not conduct electricity; molten/aqueous conducts as ions are free to move
• Water solubility as polar water molecules surround and seperate ions in the lattice

Question 9

What is a Dative Covalent Bond?

Answer 9

Dative Covalent Bond: Shared pair of electrons provided by one atom, represented with an arrow from donor to acceptor atom.

Question 10

What is VSEPR?

Answer 10

Valence Shell Electron Pair Repulsion: Electron pairs repel to maximize distance.

Question 11

How do lone pairs affect bond angles?

Answer 11

Lone pairs reduce bond angles by 2.5° per pair due to greater repulsion.

Question 12

What is Electronegativity?

Answer 12

Electronegativity: Ability of an atom to attract a pair of electrons in a covalent bond.

Question 13

What are the trends in Electronegativity?

Answer 13

Increases across a period and up a group.
- Most electronegative elements: Fluorine > Oxygen > Nitrogen.

Question 14

What is polarity in bonds and molecules?

Answer 14

• Nonpolar bond: Equal electronegativity- electrons shared equally
• Polar bond: Unequal electronegativity. dipole forms

Question 15

How do you determine the polarity of a molecule?

Answer 15

• Symmetrical molecules are nonpolar;dipoles cancel
• asymmetrical molecules are polar.

Question 16

What are the anomalous properties of water due to hydrogen bonding?

Answer 16

High boiling point, less dense ice structure ( due to open lattice) , and surface tension due to strong intermolecular hydrogen bonding , require more energy to break.