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H Chem > Unit 6 (chapters 5 & 6) > Flashcards

Unit 6 (chapters 5 & 6) Flashcards

1
Q

acid

A

Substances that produce hydrogen ions in aqueous solution; proton donor

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2
Q

activity series

A

lists the elements from most reactive to least reactive
ex: Halogens activity series is F>Cl>Br>I

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3
Q

aqueous

A

dissolved in water

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4
Q

balancing

A

Making sure that all atoms present in the reactants are accounted for among the products

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5
Q

binary compound

A

A two-element compound

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6
Q

coefficient

A

Large number before particles, affects all atoms in particle

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7
Q

combustion

A
  • Burning
  • One of the reactants is always O2 (because O2 is necessary to support combustion)
  • The other reactant is the thing being combusted- all atoms in that reactant are separated from each other and combined with oxygen
  • Every product is a binary compound with oxygen in it
  • The most common combustion reactions involve hydrocarbons (compounds of C & H)
    Ex: 2C8H18 (g) + 25O2 (g) -> 16CO2 (g) + 18H2O
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8
Q

decomposition

A
  • AB -> A + B
  • a compound breaks down into two or more simpler compounds or elements
  • Only ONE reactant and it is always a compound (elements cannot decompose)
    Ex: 2H2O2 (aq) -> 2H2O2 (l) + O2 (g)
    Ex: 2NaCl (s) -> 2Na (s) + Cl2 (g) (this requires electrolysis)
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9
Q

dissociation

A
  • NOT a reaction type- only physical change (though similar to decomposition)
  • ionic compound dissolves (physical change)
  • starts with single compound and ends with multiple separated parts, but they aren’t neutral elements and compounds, but instead aqueous ions
    Ex: NaCl (s) -> Na+ (aq) + Cl- (aq)
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10
Q

double replacement

A
  • AB + CD -> AD + CB
  • A reaction between two ionic compounds
  • The cation and anion in each switch places (or trade partners)
    Ex: AlCl3 (aq) + 3AgNO3 (aq) -> 3AgCl (s) + Al(NO3)3 (aq)
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11
Q

endothermic

A

heat taken out, feels cold

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12
Q

exothermic

A

exo=exit, thermic=thermomator
heat given out, will be felt- feels warm

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13
Q

formula

A

chemical equation of an element or compound

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14
Q

formula unit

A

the chemical formula of an ionic compound that lists the ions in the lowest ratio that equals a neutral electrical charge

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15
Q

ion

A

An atom or a group of atoms that has a net positive or negative charge

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16
Q

ionic compound

A

A compound that results when a metal reacts with a nonmetal to form cations and anions

17
Q

metal

A

Elements that give up electrons relatively easily and are typically lustrous, malleable, and good conductors of heat and electricity

18
Q

molecular compound

A

compound with 2 or more nonmetals

19
Q

molecule

A

a group of atoms bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction

20
Q

monoatomic ion

A

ion consisting of only one atom

21
Q

nonmental

A

Elements that do not exhibit metallic characteristics. Chemically, a typical nonmetal accepts electrons from a metal

22
Q

polyatomic ion

A

An ion containing a number of atoms

23
Q

precipitate

A

production of insoluble solid from liquids

24
Q

product

A

end result of reactant, right side of the equation

25
Q

reactant

A

materials on the left side of the equation, what you start with

26
Q

reaction

A

a process in which one or more substances, also called reactants, are converted to one or more different substances, known as products

27
Q

single replacement

A
  • A + BC -> AC + B
  • A + BC -> BA + C
  • Reactants are always a lone element and a compound
  • The lone element in the reactants replaces one of the elements in the compound
  • A nonmetal can only replace another nonmetal (taking the anion role in the compound)
  • A metal can only replace another metal (taking the cation role in the compound)
    -exception to this is metals can also replace H+ in acids
    Ex: Zn (s) + 2HCl (aq) -> ZnCl2 (aq) + H2 (g)
    Ex: Cl2 (g) + 2KBr (aq) -> 2KCl (aq) + Br2 (l)
    Note: not all single replacement reactions can occur
    An element can only replace another element that is below it in an activity series (more reactive elements can replace less reactive elements)
28
Q

subscript

A

lower than an atom, shows the number of only that specific atom

29
Q

symbol

A

a notation of one or two letters representing a chemical element

30
Q

synthesis

A
  • A + B -> AB
  • Combination of two or more elements or compounds to make a larger compound
  • only ONE product and it is ALWAYS a compound
    Ex: N2 (g) + 3H2 (g) -> 2NH3 (g)
    Ex: 2Mg (s) + O2 (g) -> 2MgO (s)
    Note: the second example can be classified as a combustion reaction. Combustion and Synthesis are the only reaction overlaps
31
Q

transition metal

A

metallic elements in the middle block of periodic table, variable valence. Valence electrons in 2 shells instead of 1

32
Q

chemical reactions

A

aka chemical changes, most often referred to as “reactions”
there’s no such thing as physical reactions
no new matter

33
Q

Signs of chemical reactions

A

Color change (does not count if it’s expected, such as with food dye)
Enegry released or absorbed (endothermic, exothermic, light)
Precipitate formed (freezing doesn’t count, usually 2 clear solutions results in nonclear solution)
Gas given off

34
Q

Energy

A

the ability to do work or cause change in matter

35
Q

Potential energy

A

energy of position or arrangement of particles

36
Q

Kinetic energy

A

energy of motion

37
Q

triangle above arrow in equation

A

indicates reactants are heated

38
Q

Balancing equations rules

A
  • Use pencil
  • Write the reactants on the left and the products on the right, separated by a right-pointing arrow ->
  • Double-check formulas and leave them alone, no changes!
  • Start with elements other than hydrogen and oxygen (because they’re so common)
  • Make the number of each kind of atom equal by adding coefficients
  • Coefficient * subscript = # of that atom
39
Q

Balancing equation tips

A
  • When balancing an equation with polyatomic ions in the formula, you can treat the polyatomic ion as one big particle and not balance the elements individually
  • If it doesn’t work at first, add 1 to the coefficient before the first particle on the reactant side, the solve. Continue as needed

H Chem (9 decks)

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