Module 3 ( Chemical Bonding, Reaction Types, Balancing, Stoichiometry) Flashcards
What is chemical bonding?
The force of attraction between atoms
True or False. Atoms need 8 electrons for them to be stable.
True
Differentiate anion from cation.
Anion has negative charge from gaining electrons while cation has a positive charge from losing electrons.
Enumerate the two types of chemical bonds.
Ionic and Covalent Bond
Bonding between a metal and a nonmetal
Ionic Bonding
What is ionization?
When atoms gain or lose electrons.
Bonding between nonmetals, or nonmetal with itself.
Covalent bonds.
Differentiate the two types of covalent bonds.
Nonpolar are when electrons are equally shared and between 2 unlike atoms. Polar are when electrons are unequally shared with atoms of the same kind.
What is the electronegativity difference between the types of bonds?
Nonpolar : 0 - 0.5
Polar: 0.5 - 1.6
Ionic - 1.7 and up
What naming system should be used when a compound consists of a metal?
The naming system for ionic compounds
True or False. The group number is the number of neutrons in the outermost shell.
(If false, correct the statement)
False.
The group number is the number of electrons in the outermost shell.
The electron dot structures for molecules
Lewis structure
What do the unshared electrons in a compound call?
Lone pairs
What is a polyatomic ion?
It contains both ionic and covalent bond.
A compound consisting of two different elements.
Binary compounds
A hydrogen atom bonded with another atom as an anion.
Binary acids
Differentiate the naming for liquid and gaseous acids.
Liquids: hydro + nonmetal + ic + acid
Gaseous: hydrogen + nonmetal + ide
Naming for binary ionic compounds.
Metal + nonmetal “ide”
Which type of binary compounds uses prefixes in naming?
BInary covalent compounds
True or False. In binary covalent, anions should be first in naming.
(If false, correct the statement)
False.
In binary ionic, cations are the first in names. The second element ends with “ide” and includes a prefix based on how many atoms.
Used by Dalton as a shorthand notation.
Symbols of elements
When writing a chemical formula, what should one know first?
Know the charges of ions first.
2 general rules in writing a chemical formula.
- No subscript if it has the same amount of charges
2. Swap subscripts with different amounts of charges.
True or False. All polyatomic ions end with “-ate” or “-ite” except cyanide, hydroxide, peroxide.
(If false, correct the statement.)
True
What is Slivka’s square used for?
It’s used for naming polyatomic ions that contains oxygen.
What is Slivka’s square?
An imaginary box in the periodic table with corner Si, S, Te, Sn.
The general rules for Slivka’s square.
- Any polyatomic ions outside the square has 3 oxygens
2. Polyatomic ions inside the square has 4 oxygens.
Enumerate the Big 5.
- Carbonate → CO3^2-
- Chlorate → ClO3^1-
- Nitrate → NO3^2-
- Sulfate → SO4^2-
- Phosphate → PO4^3-
General rules for naming ions by extensions in ternary compounds.
- “Hypo- is one less oxygen than “-ite”
- “-ite” is one less oxygen than “-“ate”
- “per-“ is over “-ate”
Naming acids without oxygen
hydro + negative ion + ic + acid
Naming acids with oxygen
- remove “-ate” + “-ic” acid
2. remove “-ite” + “-ous” acid
An ionic compound that has a specific number of water molecules.
Hydrates
Anhydrates
Hydrates that has their water removed
In a chemical formula, which is on the left and right sides?
Reactants on the left and products on the right
It indicates the number of moles produces.
Coefficients
True or False. The reaction should contain information about state properties.
(If false, correct the statement.)
True
What is a chemical reaction?
A process that transforms substance into another substances.
Two or more reactants with one product.
Synthesis Reaction
Decomposition Reaction
breaks apart, one reactant with two or more products
AB + CD → AD + BC
Double Replacement Reaction
A reaction that produces water + carbon dioxide
Combustion
The study involving chemical formulas and equations, molecular and formula mass, percent composition.
Stoichiometry
The calculation of reactants and products in chemical reactions.
Stoichiometry
Mass of an atom of an element
Atomic Mass
The total mass of all atoms in a molecule
Molecular Mass
Mass of a unit cell in an ionic compound
Formula Mass
The sum of the atomic weights for the atoms in a chemical formula
Formula Weight
The lowest whole number ratio of atoms in a compound
Empirical formula
Molecular formula
The true number of atoms of each elements in the formula of compounds
True or False. Stoichiometry is based on the law of conservation of mass.
(If false, correct the statement.)
True
Molarity (M)
moles of solute/ Liter of solution
Molality (m)
moles of solute/kg of solvent
Normality (N)
Number of gram equivalent * (volume of soln in liters)
How to get the moles of solute?
weight in grams/ gram molecular weight
The formula in getting the weight of solute
(L of solute)(gmw)(M)
How to solve for weight of solvent.
Weight of solution - Weight of solute
The formula in getting the number of gram equivalent
weight of solute/ (equivalent weight)(vol g solution)
Used for quantitative reactions in solution and titration
Molarity
Used in determining how colligative properties vary with solute concentration
Molality
Used for trace quantities
Percent mass
Used in measuring the gram equivalent
Normality
