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Inorganic and Organic Chemistry (Lecture) > Module 3 ( Chemical Bonding, Reaction Types, Balancing, Stoichiometry) > Flashcards

Module 3 ( Chemical Bonding, Reaction Types, Balancing, Stoichiometry) Flashcards

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1
Q

What is chemical bonding?

A

The force of attraction between atoms

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2
Q

True or False. Atoms need 8 electrons for them to be stable.

A

True

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3
Q

Differentiate anion from cation.

A

Anion has negative charge from gaining electrons while cation has a positive charge from losing electrons.

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4
Q

Enumerate the two types of chemical bonds.

A

Ionic and Covalent Bond

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5
Q

Bonding between a metal and a nonmetal

A

Ionic Bonding

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6
Q

What is ionization?

A

When atoms gain or lose electrons.

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7
Q

Bonding between nonmetals, or nonmetal with itself.

A

Covalent bonds.

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8
Q

Differentiate the two types of covalent bonds.

A

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.

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9
Q

What is the electronegativity difference between the types of bonds?

A

Nonpolar : 0 - 0.5
Polar: 0.5 - 1.6
Ionic - 1.7 and up

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10
Q

What naming system should be used when a compound consists of a metal?

A

The naming system for ionic compounds

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11
Q

True or False. The group number is the number of neutrons in the outermost shell.

(If false, correct the statement)

A

False.

The group number is the number of electrons in the outermost shell.

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12
Q

The electron dot structures for molecules

A

Lewis structure

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13
Q

What do the unshared electrons in a compound call?

A

Lone pairs

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14
Q

What is a polyatomic ion?

A

It contains both ionic and covalent bond.

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15
Q

A compound consisting of two different elements.

A

Binary compounds

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16
Q

A hydrogen atom bonded with another atom as an anion.

A

Binary acids

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17
Q

Differentiate the naming for liquid and gaseous acids.

A

Liquids: hydro + nonmetal + ic + acid
Gaseous: hydrogen + nonmetal + ide

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18
Q

Naming for binary ionic compounds.

A

Metal + nonmetal “ide”

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19
Q

Which type of binary compounds uses prefixes in naming?

A

BInary covalent compounds

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20
Q

True or False. In binary covalent, anions should be first in naming.

(If false, correct the statement)

A

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.

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21
Q

Used by Dalton as a shorthand notation.

A

Symbols of elements

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22
Q

When writing a chemical formula, what should one know first?

A

Know the charges of ions first.

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23
Q

2 general rules in writing a chemical formula.

A
  1. No subscript if it has the same amount of charges

2. Swap subscripts with different amounts of charges.

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24
Q

True or False. All polyatomic ions end with “-ate” or “-ite” except cyanide, hydroxide, peroxide.

(If false, correct the statement.)

A

True

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25
Q

What is Slivka’s square used for?

A

It’s used for naming polyatomic ions that contains oxygen.

26
Q

What is Slivka’s square?

A

An imaginary box in the periodic table with corner Si, S, Te, Sn.

27
Q

The general rules for Slivka’s square.

A
  1. Any polyatomic ions outside the square has 3 oxygens

2. Polyatomic ions inside the square has 4 oxygens.

28
Q

Enumerate the Big 5.

A
  1. Carbonate → CO3^2-
  2. Chlorate → ClO3^1-
  3. Nitrate → NO3^2-
  4. Sulfate → SO4^2-
  5. Phosphate → PO4^3-
29
Q

General rules for naming ions by extensions in ternary compounds.

A
  1. “Hypo- is one less oxygen than “-ite”
  2. “-ite” is one less oxygen than “-“ate”
  3. “per-“ is over “-ate”
30
Q

Naming acids without oxygen

A

hydro + negative ion + ic + acid

31
Q

Naming acids with oxygen

A
  1. remove “-ate” + “-ic” acid

2. remove “-ite” + “-ous” acid

32
Q

An ionic compound that has a specific number of water molecules.

A

Hydrates

33
Q

Anhydrates

A

Hydrates that has their water removed

34
Q

In a chemical formula, which is on the left and right sides?

A

Reactants on the left and products on the right

35
Q

It indicates the number of moles produces.

A

Coefficients

36
Q

True or False. The reaction should contain information about state properties.

(If false, correct the statement.)

A

True

37
Q

What is a chemical reaction?

A

A process that transforms substance into another substances.

38
Q

Two or more reactants with one product.

A

Synthesis Reaction

39
Q

Decomposition Reaction

A

breaks apart, one reactant with two or more products

40
Q

AB + CD → AD + BC

A

Double Replacement Reaction

41
Q

A reaction that produces water + carbon dioxide

A

Combustion

42
Q

The study involving chemical formulas and equations, molecular and formula mass, percent composition.

A

Stoichiometry

43
Q

The calculation of reactants and products in chemical reactions.

A

Stoichiometry

44
Q

Mass of an atom of an element

A

Atomic Mass

45
Q

The total mass of all atoms in a molecule

A

Molecular Mass

46
Q

Mass of a unit cell in an ionic compound

A

Formula Mass

47
Q

The sum of the atomic weights for the atoms in a chemical formula

A

Formula Weight

48
Q

The lowest whole number ratio of atoms in a compound

A

Empirical formula

49
Q

Molecular formula

A

The true number of atoms of each elements in the formula of compounds

50
Q

True or False. Stoichiometry is based on the law of conservation of mass.
(If false, correct the statement.)

A

True

51
Q

Molarity (M)

A

moles of solute/ Liter of solution

52
Q

Molality (m)

A

moles of solute/kg of solvent

53
Q

Normality (N)

A

Number of gram equivalent * (volume of soln in liters)

54
Q

How to get the moles of solute?

A

weight in grams/ gram molecular weight

55
Q

The formula in getting the weight of solute

A

(L of solute)(gmw)(M)

56
Q

How to solve for weight of solvent.

A

Weight of solution - Weight of solute

57
Q

The formula in getting the number of gram equivalent

A

weight of solute/ (equivalent weight)(vol g solution)

58
Q

Used for quantitative reactions in solution and titration

A

Molarity

59
Q

Used in determining how colligative properties vary with solute concentration

A

Molality

60
Q

Used for trace quantities

A

Percent mass

61
Q

Used in measuring the gram equivalent

A

Normality

Inorganic and Organic Chemistry (Lecture) (6 decks)

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