Chemistry Brooks

Today we worked on Chapter 7 Questions. Finish them for HOMEWORK!!
7.1 Worksheet  Ionic Compounds and Metals
7.2 Worksheet Ionic Bonds and Ionic Compounds


THINGS TO REMEMBER
1. BRING BOOK EVERYDAY
2. PICK up your make up assignment after school today, Due before school tomorrow
3. Make up Quiz (for anyone who missed or needs to redo a quiz) WHEN: After school Monday 12/12/2011
4. Graphs DUE (You should have 3) Ionic, Electronegativity, and Radius. Each graph comes with questions.

Notes from Today

CHAPTER SEVEN NOTES

+ Ions: Cations (Cat ions: Think cats good, positive)

 - Ions: Anions (An ions: Think onions, bad… negative)

Sodium     Na                    LOW ionization: Means 1 little energy in the electron… leaves quickly.

11 p

10 e

net 1+

Fluorine      F                    HIGH electronegativity: Pulls electrons in easily.

  9 p

10 e

net 1-

CHARGE has to do with gaining and losing electrons

IONIC BOND

·       An ionic bond is a force that holds together atoms that are oppositely charged.

·       Ionic bonds generally occur between a metal and a nonmetal.

·       Ionic bond: giving and taking

IONIC COMPOUNDS

·       Ionic compounds are strong bonds, held together by every side

·       The formula unit of an ionic compound shows the simplest ratio of the ions.

·       The overall charge of a formula unit for an ionic compound is always zero.

·       The formation of a stable ionic compound from ions may be either exothermic or endothermic.

·       Ionic compounds…

o    Have high melting points

o    Have high boiling points

o    Are very hard and brittle

o    Conduct electricity poorly in a solid state

o    Conduct electricity well in a liquid state

o    Conduct electricity well when dissolved in water

·       EXAMPLES: Salts are examples of ionic compounds.

LATTICE & IONS:

·       A three-dimensional arrangement of particles in an ionic solid is called a crystal lattice.

·       In a crystal lattice of an ionic compound, ions are surrounded by ions of the opposite charge.

·       The more negative the lattice energy is, the greater the strength of the attractive force holding ions in place.

·       The crystal lattice of ionic compounds affects their melting and boiling points.

·       The lattice energy is the energy required to separate the ions of an ionic compound.

·       Ions that have larger charges tend to produce more negative lattice energy than ions with smaller charges do.

GAINING/LOOSING ELECTRONS

·       In electron transfer involving a metallic atom and a nonmetallic atom during ion formation, the nonmetallic atom gains electrons from the metallic atom.

·       Elements in GROUP 1 lose their one valence electron, forming an ion with a 1+ charge.

·       A sodium atom tends to lose one electron when it reacts.

·       The electron structure of a zinc ion (Zn²⁺) is an example of a pseudo-noble gas formation.

·       The ending –ide is used to designate an anion.

CHEMICAL BOND

·       The force that holds two atoms together is called a chemical bond. Such an attachment may form by attraction of the positively charged nucleus of one atom for the negatively charged electrons of another atom, or by the attraction of charged atoms, which are called ions. The attraction may also involve valence electrons, which are electrons in the outermost energy level.

NOBLE GASES

·       The noble gases are a family of elements that have very little tendency to react. Most of these elements have a set of eight outermost electrons, which is called a stable octet. The relatively stable electron structures developed by loss of electrons in certain elements of groups 3, 4, 13, and 14 are called pseudo-noble gas formations.