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