study guide - unit 6 Flashcards
(17 cards)
what is a bond?
when all atoms achieve a stable outer shell configuration similar to the noble gas
what is an ionic bond?
complete transfer of VE
what is a covalent bond?
ions with shared electrons
what are polar covalent bonds?
bonding electrons shared unequally between two atoms
what are non-polar covalent bonds?
bonding electrons shared equally between two atoms
what are polyatomic atoms?
ions made of more than 1 atom
what is ionic radius and its effect on size and its trend?
distance between ion’s nucleus and outermost shell
loses electrons - decreases in size
gains electrons - increases in size
(P) decrease
(G) increase
what are isoelectric series?
why?
ions with same number of electrons, but different overall charges due to differing atomic number
what is ionization energy and its trend?
energy required to remove an electron from an atom
(P) - increases
(G) - decreases
what is lattice energy?
energy required to separate ionic bonds
what is electronegativity?
measure of an atom’s ability to attract shared electrons to itself
what is the reactivity trends for metals verus non-metals?
metals: (P) decreases & (G) increases
non-metals: (P) increases & (G) decreases
explain the size order of an isoelectric series according to coulombic attractions
greater positive charge = greater coulombic attraction and a decrease in size
lesser negative charge = lesser coulombic attraction and an increase in size
what are the five properties of ionic compounds?
- high bp/mp
- crystal structure
- usually soluble in water
- conducts electricity when dissolved in water
- insoluble when melted
what are the three properties of acids?
- pH less than 7
- sour taste
- name from anion
what are the two factors that effect lattice energy?
smaller size & higher energy = stronger lattice energy
how do you predict the solubility and melting point based on lattice energy being greater or smaller?
greater = lower solubility & higher melting point
smaller = higher solubility & lower melting point
