Question | Answer |
Are there few or many electrons in the outermost energy level of metals? | few
|
What is the difference between malleability and ductility? | bend vs. stretch
| What are the two types of covalent bonds? | pure covalent and polar covalent
| How does electronegativity change as you move from left to right across the periodic table? | increase
| What type of elements form ionic bonds? | metals and nonmetals
| Give an example of a polar covalent bond? | answers may vary
| How can we use the periodic table to help us determine the type of bonding between atoms? | Trends in electronegativity and metals vs non metals
| Why do we only consider Valence electrons in drawing Lewis structures? | they are the ones that react
| The relative ability of an atom in a molecule to attract electrons to itself is called the atoms ___________. | electronegativity
| What is a dipole moment?; draw an example. | electrical effect that occurs in molecules with separate centers of positive and negative charge.
| What does it mean when we say that in forming bonds, atoms try to achieve an electron configuration of a noble gas? | most stable configuration.
| Double point questions! Why are cations always smaller than the atoms from which they were formed? | loss of e so one valence shell is lost
| Explain the difference between the duet and the octet rule. Give an example of an atom that follows each. | H and O
| Write the Lewis structure for Sr. | see notes
| Write the Lewis structure for C2F6. | see notes
| Write the Lewis structure for N2H4. | see notes
| Write the Lewis structure for the sulfate ion. | SO4 2-
| What does it mean for a molecule to exhibit resonance? | more than one lewis structure
| Write the Lewis structure for the barium ion. | Ba2+
| What general principles determine the molecular structure (shape) of a molecule? | how many e pairs surround, which pairs used for bonding
| Come to the classroom and build a model of one of the molecules listed by the parts kit. | see models |