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Chemistry 11 > Chemical Reactions > Flashcards

Chemical Reactions Flashcards

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1
Q

Monoatomic ion

A

an ion consisting of only one ion (Na or Cl)

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2
Q

Cation

A

Positive ion

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3
Q

Anion

A

Negative Ion

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4
Q

Univalent Metal

A

A metal with only one stable ionic form; for example, the only stable ionic form of sodium is Na+. All the metals of groups 1A, 2A and Al3+ , Zn2+ and Ag+ are univalent.

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5
Q

Multivalent Metal

A

A metal with more than one stable ionic form. Many transition metals, as well as Pb and Sn are multivalent.

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6
Q

Polyatomic ion

A

A group of atoms covalently bonded together with an overall positive or negative charge, such as NH4+ and NO3 – .

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7
Q

Binary acid

A

An acid consisting of hydrogen and another nonmetal

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8
Q

Oxyacid

A

An acid consisting of hydrogen, oxygen and another nonmetal

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9
Q

Binary Ionic Compound

A

Ionic compound made of TWO elements.

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10
Q

Polyatomic anion that ends in -ite

A

has a lower oxygen number

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11
Q

Polyatomic anion that ends in -ate

A

has a higher number of oxygen

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12
Q

Greek Prefixes

A

Mono- 1 di- 2 tri- 3 tetra 4 penta 5 hexa 6 hepta 7 octa 8 nona 9 deca 10

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13
Q

Binary Molecular Compound

A

a covalent bond between TWO non metals, they share electrons

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14
Q

Acids

A

compound in which one or more H+ ions are bonded to an anion

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15
Q

Binary Acid

A

When the anion is monoatomic, the acid is a binary acid (it consists of just two elements)

In gas state you name it like a regular binary ionic compound.

When these compounds are in their acidic form (aqueous state), the name begins with the prefix hydro- followed by the full name of the second nonmetal, and the suffix –ic, followed by the word “acid”.

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16
Q

Oxyacid

A

When the anion is an oxyanion (a polyatomic anion containing oxygen), then the acid is an oxyacid.

To name these acids, if the polyatomic anion ends with –ite, the suffix –ous is added to the root name, and if the polyatomic anion ends with –ate, the suffix –ic is added to the root name.

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17
Q

HCN

A

Although HCN is not a binary compound (It consists of three elements), it is named in the same way as the others since it has no oxygen and can exist in both the gaseous and aqueous states.

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18
Q

Synthesis

A

A chemical reaction in which two or more reactants (elements and/or compounds) combine to produce a single product

Sometimes a synthesis reaction is also a combustion reaction.

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19
Q

Combustion

A

Combustion is defined as rapid reaction of a substance with oxygen, resulting in the formation of oxides and release of energy as heat and light.

a highly exothermic rapid reaction of a substance with oxygen which results in the production of oxide(s)

20
Q

Decomposition

A

A chemical reaction in which a compound breaks down into two or more elements and/or simpler compounds

21
Q

Single Displacement

A

A chemical reaction in which one element in a compound is replaced (displaced) by another element

22
Q

Double Displacement

A

A double displacement reaction is one the three possible types:

Precipitation (determined by solubility chart)

Gas Formation (unstable compound decomposes into water and gas)

Neutralization (acid+base –> salt +water)

AKA (exchange reaction and metathesis reactions)

23
Q

Salt

A

An ionic compound that is neither an acid nor a base nor a metal oxide

24
Q

Hydrocarbon

A

Hydrocarbon is a compound consisting of carbon and hydrogen alone. Methane, CH4 (the main component of natural gas) and propane, C3H8 (fuel for gas barbecue) are examples of hydrocarbons.

25
Q

Complete Combustion

A

When a hydrocarbon or a hydrocarbon derivative combusts, the products are carbon dioxide and water provided that sufficient oxygen is available.

26
Q

Incomplete Combustion

A

If, on the other hand, the amount of oxygen available is insufficient, the reaction can produce elemental carbon, or soot C(s), and carbon monoxide, CO(g), as well as, carbon dioxide, and water, in which case the reaction is called “incomplete combustion”.

27
Q

Bunsen Burner Combustion

A

A blue flame, such as a Bunsen burner flame is an indication of complete combustion resulted from sufficient oxygen. A yellow flame, such as that of a candle is an indication of incomplete combustion.

28
Q

Organic Molecules

A

must have hydrogen and carbon

29
Q

Inorganic Molecules

A

most inorganic compounds do not contain carbon

30
Q

Hydrates

A

Hydrates contain one or more water molecules in their crystal structure. The number of water molecules vary from one hydrate to another. These water molecules are loosely bonded to the metal ions and can be broken upon heating. The metals (with complex electronic arrangement), allow for molecules like water that have lone pairs to bond loosely. The number of water molecules in the formula of the hydrate is called the “number of hydration water.”

31
Q

Anhydrous salt

A

A dry salt that does not contain water

32
Q

Unstable Compounds

A

H2CO3

H2SO3

NH4OH

33
Q

Complete Ionic Equation

A

you separate all the ions, indicate the charges, add coefficients

34
Q

Spectator Ions

A

Ions that appear in identical forms on both sides of a complete ionic equation

35
Q

Net ionic equation

A

ions and compound directly involved in the reaction

36
Q

Any compund containing these are water soluble

A
  • alkalai metal ions
  • hydrogen ions, H+
  • ammonium ion, NH4+
  • nitrate ion, NO3-
37
Q

Synthesis Reactions

A
  1. Formation of binary compound from 2 elements
    a) univalent metal + non metal -> ionic
    b) multivalent metal + non metal -> ionic
    c) non-metal + non-metal -> molecular
  2. Element reacts with compound to form new compound
  3. Two compounds combine to form new compound
    a) metal oxide + water -> metal hydroxide (base)
    b) non-metal + water -> acid
38
Q

Decomposition Reactions

A
  1. Binary compound decomposing into elements
  2. Metal Nitrate -> metal nitrite + oxygen gas
  3. Metal Carbonate -> metal oxide + carbon dioxide
  4. Metal Hydroxide -> metal oxide + water
39
Q

Single Displacement (Metal displacing Hydrogen in acid or water)

A

Metal + Water -> Metal Hydroxide (base) + Hydrogen gas

40
Q

Neutralization Reaction

A

DD, if insoluble salt is formed it can be neutralization and precipitation

acid + base -> salt + water

41
Q

How Soap is made in the industry

A

The soap industry does not use carboxylic acid to produce soap because it is expensive to create. They use natural fatty acids like animal fat or vegetable oil to produce soap in the most cost effective way. So intead of water being produced, glycerin is produced.

42
Q

Chemistry of Soap

A

Soaps are made by reacting alkali metals with fatty acids. The reaction produces salts of the fatty acids making things easier to clean. This is an example of a neutralization reaction. The salt cation is Na or K and the anion is a long chain of carboxylic acid. The ionic compound has a hydrophobic hydrocarbon tail and a hydrophylic anionic head.

43
Q

When Soap is Used

A

Something that is hydrophilic is a polar molecule because it attracted to water. Something that is hydrophobic is non polar. When you look at soap, the nonpolar sides make LDF as the Hydrogen and Carbon have a low electronegativity difference. Certain parts of the soap are polar because there is oxygen presents and there is a large electronegativity difference between oxygen and carbon. When we put soap in water, the head is the part that is attracted to water. The Na and carboxylic ions separate from each other as it is an ionic solutions that dissolves in water. The nonpolar molecules are attracted to the grease. Water is polar and it cannot dissolve grease. This is how soap acts as a mediator

44
Q

Hard and Soft Water

A

The presence of Ca and Mg ions in water make it hard. These ions come from water passing through limestone. It is hard for soap to lather necause soap makes a ppt with Calcium and Mg because they are insoluble. Soap bonds Ca and Mg. They use sulfur instead in detergent because it doesn’t form ppt, it is soluble with Ca and Mg. Soft water does not have Ca or Mg so it can lather easily. Detergents are synthetic.

45
Q

Micelles

A

The soap particle tails that are hydrophobic surround the grease and form a micelle as they isolate little partivles of the grease and suspend them in H2O long enough that they can be washed away.

46
Q

Lipophilic

A

nonpolar hydrophobic tails of soap are lipophilic (“oil-loving”)

Chemistry 11 (3 decks)

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