Chapter 1 Flashcards
what comprises most of the atom’s volume?
empty space containing electrons
equation to determine the maximum number of electrons in the energy shell of the elements in each row
two raised to the n-squared, where n represents the period
properties of s-orbital
- spherical - contains two electrons
properties of p-orbitals
- px, py, and pz: exist along axes of Cartesian coordinate system - each p-orbital contains two electrons, allowing six electrons total - orthogonal: form at ninety-degree angles; never intersect one another - look like infinity symbols
electronegativity (including trends)
attractiveness for electrons - increases across a period (closer to stability) - decreases down a group (further away from nucleus)
electron affinity
energy released from gaining an electron
ionic bonds (in terms of electronegativity)
difference in electronegativity between elements > 1.9
polar covalent bonds (in terms of electronegativity)
1.9 > difference in electronegativity in elements > 0.5
nonpolar covalent bonds (in terms of electronegativity)
difference in electronegativity between elements < 0.5
relationship between size and first ionization energy
size of atoms decrease across a period, due to the stronger attraction between additional protons in the nucleus and additional electrons orbiting it. with size decreases energy; therefore, more input energy required to break the bond
formal charge
charge on an atom in a molecule or polyatomic ion formal charge = (number of electrons in neutral, unbonded atom) - (all unshared electrons + one-half of shared electrons)
functional groups
1.) organize compounds into classes 2.) exhibit characteristic reactions 3.) serve as basis for naming compounds
alcohols
(-OH) hydroxyl group bound to tetrahedral carbon
primary alcohol
bonded to a carbon bound to one other carbon and two hydrogens
secondary alcohol
bonded to a carbon bound to two other carbons and one hydrogen
tertiary alcohol
bonded to a carbon bound to three other carbons
amine
nitrogen-containing amino group
primary amine
nitrogen bound to carbon and two hydrogens
secondary amine
nitrogen bound to two carbons and a hydrogen
tertiary amine
nitrogen bound to three carbons
aldehyde
(C=O): carbon with double-bond bound to one hydrogen and one carbon (ie, at end of carbon chain)
ketone
(C=O): carbon with double-bond bound to two carbons (ie, in middle of carbon chain)
carboxylic acids
(-COOH)
carboxylic esters (esters)
derivative of carboxylic acid; hydrogen of carboxyl group replaced by another carbon-containing group
carboxylic amides (amides)
- derivative of carboxylic acid; -OH (hydroxyl) group replaced by an amine. - group exhibits planar structure
shapes of hybrid orbitals in three-dimensions
