R8 helpful chemistry, Cheat Sheet of Chemistry

This is the r8 for exam 3 that

Typology: Cheat Sheet

2025/2026

Uploaded on 02/22/2026

arlethatilano16
arlethatilano16 🇺🇸

1 document

1 / 8

Toggle sidebar

This page cannot be seen from the preview

Don't miss anything!

bg1
Recitation 8
Last Name: _____________________________
First Name: _____________________________
1. What is the octet rule? What three categories summarize exceptions to the octet
rule?
2. Draw a Lewis structure for the phosphate ion where the central atom satisfies
the octet and label the formal charges on each atom in the structure.
Draw a better structure for phosphate that minimizes formal charges. Include
the resonance structures.
3. There are 5 electron-domain classifications. Identify each and give the ideal bond
angle between the central atom and the outer atoms or electron-pairs.
Number of electron
domains
Name Ideal Bond Angle
2
3
4
5
6
4. How do lone pairs and double bonds change the bond angels in a structure?
1
pf3
pf4
pf5
pf8

Partial preview of the text

Download R8 helpful chemistry and more Cheat Sheet Chemistry in PDF only on Docsity!

Last Name: _____________________________ First Name: _____________________________

  1. What is the octet rule? What three categories summarize exceptions to the octet rule?
  2. Draw a Lewis structure for the phosphate ion where the central atom satisfies the octet and label the formal charges on each atom in the structure. Draw a better structure for phosphate that minimizes formal charges. Include the resonance structures.
  3. There are 5 electron-domain classifications. Identify each and give the ideal bond angle between the central atom and the outer atoms or electron-pairs. Number of electron domains Name Ideal Bond Angle 2 3 4 5 6
  4. How do lone pairs and double bonds change the bond angels in a structure?
  1. Fill in the following Table, including the correct ABmEn designation. Number of electron domains Electron Domain Number of Bonds & Electron-Pairs Molecular Geometry Name 2 Linear 2 bonds or a bond and 1 lone pair of electrons Linear 3 Trigonal Planar 3 bonds AB 3 2 bonds & 1 lone pair AB 2 E 1 4 Tetrahedral Trigonal pyramidal Bent 5 5 bonds AB 5 Seesaw 3 bonds & 2 lone pairs AB 3 E 2 Linear 6 6 bonds Square pyramidal 4 bonds & 2 lone pairs AB 4 E 2
  1. How many and what types of bonds form a double bond?
  2. How many and what types of bonds form a triple bond?
  3. What is the approximate bond angle of the carbons labeled below? Carbon 1: Carbon 2:
  4. How many sigma and pi bonds are in the structure shown below? Sigma: Pi:
  5. What is the difference between the following: Polar Covalent bond and Nonpolar covalent bonds Polar Covalent bonds and Ionic bonds
  6. Use both types of notations (+ and - or arrows) to indicate the polarity of the bonds below. 1 2

Atoms in bond Arrow notation + and - notation O and C N and F

  1. When atoms can share two pairs of electrons, the bond between the atoms will be _______________ (weaker/stronger) and ________________ (longer/shorter) than when only one pair of electrons are shared.
  2. The two main factors that relate to the strength of an ionic compound’s lattice energy are ___________________________ and ___________________________. Explain why these two factors influence the lattice energy of an ionic compound.
  3. Which of the two ionic compounds compared below has the larger lattice energy? Why (charge or size)? Compound Explain why Compound Explain why SrO or MgO K 2 S or Li 2 S CsI or BaI 2 KF or CaF 2
  4. Fill in the blanks with one of these choices: Solid Liquid Aqueous Ionic substances never conduct in the ___________________ phase but will conduct in either the ___________________ phase or the __________________ phase.
  5. Which tend, on average, to have higher melting points: covalent molecules or ionic substances? Why?
  1. Fill in the blanks in the table below: Formula Name Formula Name NF 3 I 2 O 5 Nitrogen monoxide Iodine heptafluoride P 2 O 5 P 4 S 10 Silicon tetrachloride Dinitrogen pentoxide SO 2 CS 2 Selenium hexabromide Dinitrogen monoxide CBr 4 PBr 5 Disulfur dichloride Carbon monoxide
  2. Fill in the blanks in the table below: Ion Name Anion/ Polyatomic Ion Formula Acid Formula Acid Name Acetate HNO 3 Cl- Phosphate Sulfurous Acid
  1. Calculate the following molar masses: Name Formula Molar Mass (g/mol) Magnesium Nitride Calcium Acetate Sodium Hypochlorite Carbon Tetrabromide
  2. Calculate and fill in the missing parts of the table below, using the units in the column headers as a guide. Mass in grams = Mol = Grams or Atoms 14.6 g Sodium sulfite

____________ mol Sodium sulfite

____________ atoms Na ____________ g Zinc phosphide

5.02 mol Zinc phosphide

____________ grams Zn ____________ g Lead (II) Nitrate

____________ mol Lead (II) Nitrate

1.74 x 10^24 atoms O ____________ g Potassium chlorate ____________ mol Potassium chlorate 5.71 grams Cl