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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 |