The Periodic Table
Chemical Bonding
Lewis Structures & Bonding Formulas
Polarity & Metallic Bonds
Bohr's Model and Electron Configuration
100

Very reactive group 1 metals with only one valence electron in their outer shell

What are alkali metals?

100

A chemical bond that occurs when one atom "steals" electrons from another atom, causing the charged atoms to then stick together

What is an ionic bond?

100

When drawing Lewis structures, most atoms need ____ electrons to be stable (unless they are hydrogen, boron, or another exception!)

What is 8 electrons?

100

Which atom would have a partial negative charge in an HF molecule?

What is fluorine?

100

Draw the Bohr's model for Hydrogen

200

Nonreactive elements that have a stable octet of eight electrons in their valence shell

What are noble gases?

200

Which kind of bond is formed by atoms that share electrons unequally and create partial negative and positive charges that cause it to be attracted to other molecules?

What is polar covalent bond?

200

Draw the Lewis Dot Structure for PCl3

200

C-H bonds are always considered ___________

What is nonpolar?

200

Draw this bohr's model as a LDS

300

The side on the periodic table that contains most of the nonmetals

What is right side?

300

Which compound usually has a higher boiling point - ionic or covalent? Explain why.

What is ionic compounds - because they have a crystal lattice made of oppositely-charged ions that stick together strongly; in contrast, covalent molecules are held together by weak intermolecular forces

300

The formula for a compound formed from Oxygen and Aluminum

What is Al2O3?

300

This image represents a _____________ bond

What is a metallic bond?

300

The element represented by the electron configuration: 1s22s22p63s1

What is sodium?

400

How does electronegativity change as you go across a period from left to right. Explain why.

What is electronegativity increases because the positive charge of the nucleus increases (more protons) and pulls electrons in closer?

400

Why do most atoms want to bond?

What is atoms want to decrease their potential energy and become stable?

400

The charge on tin in SnCl4 (write in roman numerals)


What is Tin (IV)?

400

This range of electronegative difference typically represents a polar covalent bond

What is 0.4-1.7?
400

The abbreviated electron configuration for silver

What is [Kr]5s24d9?

500

How does atomic radius change as you go down a group. Explain why.

What is the atomic radius increases because more energy levels are added, and the electrons get farther away from the nucleus - causing the atom to get bigger?

500

A bond formed between 2 non-metals

What is a covalent bond?

500

Draw the Lewis structure for C2H6.

500

CO is a polar/nonpolar bond (show your work)

What is polar?
500

The full electron configuration for rubidium 

What is 1s22s22p63s23p64s23d104p65s1