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Chemistry Unit 7
| Term | Definition |
|---|---|
| Valence Electrons | Outermost electrons that determine reactivity of an element |
| Bonds | Force that hold atoms together in a compound. Simultaneous attraction of valence electrons. Most atoms want a stable octet or 8 in the outer shell. Except H, H3m Li, and B3 |
| Making a Bond | Energy is released; Potential energy decrease; stability increases. Bonded atoms are more stable with less energy |
| Breaking a Bond | Energy is absorbed increasing potential energy. Stability decreases. Unbounded atoms are less stable with more energy |
| Ionic Bonds | Transfer of e- from one atom to another; results in formation ions; positive cation and negative anion. Formed between metal and nonmetals/polyatomic ions |
| Ionic Solids | High boiling and melting points. Just ions. Crystalline as solids; brittle; shatter and don't bend. Conduct electricity in liquid and aqueous phase |
| Electronegativity difference | Equal to or greater than 1.7 |
| Electronegativity | An atom's ability to attract electrons |
| Covalent Bonding | Electrons are always shared in pairs |
| Single Bond | 1 pair of electrons being shared. 2 total electrons by a single line. Represented by a single line |
| Double Bond | 2 pair of electrons being shared. 4 total electrons shared. Represented by a double line |
| Triple Bond | 3 pairs of electrons being shared. 6 total electrons shared. Represented by a triple line |
| Covalent Compounds | Molecules not composed of ions. Two nuclei share electrons to achieve stable octet. Often formed by two nonmetals, same or different. Orbitals overlap and electronegativity is less than 1.7 |
| Characteristics of Molecular Substances | Nonmetal atoms bonded to form molecules. Usually gas or liquid at room temp. Low melting points and boiling points. Poor conductors of heat and electricity. Very in all 3 phases. Water, glucose, butter, and wax |
| Polar Covalent | Unequal sharing of e- results in + and - regions, Partial Charges. EN difference 0.1-1.6. Atoms with higher EN pulls electrons closer to itself. Dipole |
| Nonpolar Covalent | Equal sharing of e- causes there not be a + and - region, No partial charges . EN difference 0. No Dipole |
| Dipole | Molecule with + and - region to uneven distribution of electrons |
| Polarity of Molecules | A molecule can contain polar bondsman but the molecule can be nonpolar. Bond type and symmetry must be considered |
| Polar Molecule | Polar Covalent bonds and is not symmetric |
| Nonpolar Molecule | Polar Covalent bonds or Nonpolar Covalent bonds and symmetric in more than 1 plane |
| Metallic Bonds | Form between two metals. Very conductive and heat and electricity, Results from the force of attraction of the mobile valence e- for a tom's positively charged nucleus. Valence e- roam from nucleus to nucleus. Described as a sea of mobile electrons . |
| Intermolecular forces of attraction (IFA) | Attractive forces between molecules |
| Dipole-Dipole Attraction | Both dipoles attract |
| Hydrogen Bonding | An intermolecular force of attraction similar to but stronger than dipole/dipole, High melting points and boiling point of compounds, Responsible for strength of water. |
| Van Der Waals | Weak force of attraction between nonpolar molecules because of brief e-shifts that make the molecule temporary polar |
| Strength of Intermolecular Forces Strongest to weakest | Hydrogen bonding > dipole-dipole> vander wools |
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