Exam 1 Content Flashcards

Acid/Base

1
Q

Avogadro’s Constant

A

6.022x10^23

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2
Q

Molar mass

A

(grams substance/moles) = molar mass

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3
Q

Molarity

A

moles of solutue/liters of solution

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4
Q

Buffers

A

resist changes in pH. Made from weak acids/bases and their salts

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5
Q

K(a)

A

represent the equilibrium constant. K<1 weak acid, K>1 strong acid.

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6
Q

Bronsted-Lowry Acids/Base

A

Acid: any substance that donates a proton (H+)
Base: any substances that accepts a proton (H+)

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7
Q

Henderson-Hasselbach Equation

A

pH = pKa + log (A-/HA) or (B/HB+)

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8
Q

pKa

A
  1. The pH at which both the acid (HA or HB+) and the conjugate (A- or B) base are maintained in equal amounts.
  2. Measure of hydrogen ion concentration required to put a H+ back on the conjugate base of the acid.
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9
Q

10^pH-pK

A

(A-/HA) or (B/HB+)

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10
Q

Arrhenius Acids/Bases

A

Acid: substance that when ADDED to WATER will increase the (H30+) concentration of the solution
Base: substance that when ADDED to WATER will increase the (OH-) concentration of the solution.

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11
Q

Lewis Acids/Bases

A

Acid: electron pair acceptor (usually metals)
Base: electron pair donor

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12
Q

7 Strong Acids

A
HCl
HBr
HI
H2SO4 (dirpotic acid)
HNO3
HClO4 (perchloric acid)
HClO3 (chloric acid)
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13
Q

Strong Bases

A

Any group 1&2 Metal Hydroxides (OH). but not Mg(OH2).

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14
Q

Neutralization Reaction

A

reaction between an acid/base that yields water and a salt. (Bronsted acid/base)

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15
Q

Ionic equation

A

written with soluble substances written as ions and only those involved in the reaction. 2H(+) + 2OH(^-1) –> 2H2O

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16
Q

(H+) =

A

10^-pH

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17
Q

(OH-) =

A

10^-pOH

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18
Q

pH + pOH =

A

14

19
Q

% ionization

A

(Memorize the formula) defines the % of HA or B in the charged form (A- or HB+), related to the value of K.

20
Q

% dissociation

A

(B)/([HB+] + [B])

Same as %ionization for HA.

21
Q

molecules

A

aggregates of atoms chemically (covalent) bonded into a discrete unit

22
Q

atoms

A

fundamental building block of all matter

23
Q

compound

A

comprised of two or more kinds of atoms (H2O, NH3)

24
Q

mixtures

A

aggregates of two or more pure substances that can be separated through physical means. hetergenous or homogenous.

25
Q

isotopes

A

same atomic number but different neutron numbers

26
Q

ion

A

a charged particle that is formed by the gain or loss of valence
electrons by an element or group of elements.

27
Q

cation

A

positively charged ions formed by losing an electron

28
Q

anion

A

negatively charged ions formed by the addition of an electron.

29
Q

valence shell

A

highest energy level of an element. in this shell are the valence electrons.

30
Q

valence electrons

A

the electrons of an element involved in chemical bonding.

31
Q

noble gas configuration

A

when an atom has all of its valence shell filled. all elements try to achieve this configuration.

32
Q

isoelectronic

A

when two ions/elements have the same electron configuration

33
Q

Homogenous mixture

A

same throughout with identical properties everywhere in the mixture (sugar dissolved in water, metal alloy in bike frames). not easily seperated.

34
Q

Hetergenous mixture

A

have different properties when sampled from different areas (Air, sand mixed with water, trail mix)

35
Q

States of Matter

A

Solids, liquids, gases, and Plasma.

36
Q

electronegativity

A

measure of the force with which an atom attracts the electron in a covalent bond. Increases up and to the right on the periodic table.

37
Q

ionization energy

A

energy required to remove an electron from a gaseous ground state atom or ion. (increases with electronegativity)

38
Q

electron affinity

A

enthalpy change accompanying the addition of an electron (correlates with electronegativity)

39
Q

atomic radius

A

half the distance between the nuclei of two identical atoms.

40
Q

Ionic Radii

A

increases when gaining electrons, decreases when losing electrons.
the radium of an atom that either gains or loses electrons.

41
Q

Octet Rule

A

Tendency for atoms to obtain or lose electrons to fulfill 8 electrons in its valence shell. C, N, O, F follow this.

(H, Li, Be, B do not follow this rule)

42
Q

VSEPR

A

Valence Shell Electron Pair Repulsion Theory predicts the shape of molecules base on the total number of bonds and lone electron pairs in the valence shell of the central atom.

43
Q

monoatomic ion

A

an ion formed from a single atom (cation/anions)

44
Q

polyatomic ion

A

formed from two or more atoms that are chemically (covalently) bonded together from having a net electronic charge. Usually from acids/bases