5 Written questions
5 Matching questions
- 4 ED
- Drawing Lewis Structures
- Chemical Bond
- Covalent Bond
- Lattice Energy
- a 1) Total the valence electrons of all bonded atoms. (- means you add electrons, + means you subtract electrons)
2) Use one pair of electrons to bond each outer atom to the central atom.
3) Complete the octets around all of the outer atoms.
4) Place any remaining electrons on the central atom.
5) If there are not enough electrons to give the central atom an octet, make multiple bonds.
- b A strong force of attraction that holds two atoms together. Involves the valence electrons of atoms.
- c Results from sharing electrons between two atoms, usually nonmetal atoms.
- d Orbital Hybridization sp3
- e (∆ H lattice) is the energy required to completely separate a mole of a solid ionic compound into its gaseous ions. Ionic compounds tend to have high lattice energies, which tend to make ionic compounds hard and brittle with relatively high melting points.
5 Multiple choice questions
- A molecule with one end having a slight positive charge and the other end having a slight negative charge due to differences in electronegativity. Arrow points towards the more electronegative element.
- The relative ability of an atom to attract a pair of electrons. Increases from left to right and from bottom to top. Fluorine has the highest and francium has the lowest. gas>liquid>solid Determines polarity.
- An attractive force between ions of opposite charges, often a metal cation and a nonmetal anion.
5 True/False questions
Ionization Energy → The energy required to remove an electron from an atom or ion in the gaseous state. Increases from left to right and from bottom to top on the Periodic Table.
VSEPR (Valence-shell electron-pari repulsion) → A region around an atom in which electrons will most likely be found. Produced by a nonbonding pair, a single bond, a double bond, or a triple bond.
Resonance Structures → For covalent molecules often show shared pairs of electrons (bonding pairs) as lines and unshared electron pairs (nonbonding pairs) as lines or dots.
Sextet Rule Elements → H
EDG Octahedral → MG Tetrahedral
MG Trigonal pyramidal