Bonding Flashcards
(36 cards)
Why do atoms bond together?
To become more stable; a molecule has less energy than isolated atoms.
What are the two major types of bonding?
Intramolecular bonding (within molecules) and intermolecular bonding (between molecules).
What are the four main types of chemical bonds?
Network covalent, metallic, ionic, and covalent (molecular).
What is an ionic bond?
The force of attraction between a cation and an anion.
What is a covalent bond?
The simultaneous attraction of two nuclei for a shared pair of electrons.
What is a metallic bond?
The attraction between positive metal nuclei and mobile valence electrons.
What is a network covalent bond?
A 3D structure where atoms are continuously linked by strong covalent bonds.
What are the properties of ionic compounds?
High melting/boiling points, brittle, conduct electricity when molten or dissolved.
What are the properties of molecular (covalent) compounds?
Can be solids, liquids, or gases; do not conduct electricity; low melting/boiling points.
What are the properties of metallic bonds?
Malleable, ductile, conduct electricity and heat, high melting/boiling points.
What are the properties of network covalent solids?
Very hard, high melting points, non-conductive.
What happens to atomic radius across a period?
Decreases from left to right due to increasing nuclear attraction.
What happens to atomic radius down a group?
Increases due to the addition of electron shells.
What is ionization energy?
The energy required to remove an electron to form a cation.
What is electronegativity?
An atom’s tendency to attract electrons in a bond.
Which element has the highest electronegativity?
Fluorine (4.0).
What type of bond forms if the electronegativity difference is between 1.7 and 3.3?
Ionic bond.
What type of bond forms if the electronegativity difference is less than 1.7?
Polar covalent bond.
What type of bond forms if the electronegativity difference is zero?
Nonpolar covalent bond.
What does a Lewis dot diagram represent?
Valence electrons and bonding possibilities of an atom.
What is the octet rule?
Atoms tend to form bonds to achieve eight valence electrons.
What are lone pairs in a Lewis structure?
Non-bonding valence electrons.
What does VSEPR stand for?
Valence Shell Electron Pair Repulsion Theory.
What is the molecular shape of CH4 (Methane)?
Tetrahedral.
