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Chem Praxis Notes > Ch 11- 17 > Flashcards

Ch 11- 17 Flashcards

(76 cards)

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1
Q

Periodic table

A

Alkali metals
Alkali earth metals
Transition metals
Metalloids
Nonmetals
Halogens
Noble gases

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2
Q

Atomic radius trends

A

Atomic radius increases down a group

Radius decreases across a period because more protons

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3
Q

Ionization energy

A

Amount of energy required to remove an electron from an atom

Move down a group easier to ionize because further away from nucleus

Ionization energy increase across a period because more protons

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4
Q

Electronegetivity

A

Ability to attract other electrons

Electronegativity decreases down a group
Shells further out from nucleus

Electronegativity increases across period because more protons ie smaller radius therefore more attraction

Noble gases have no electronegativity

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5
Q

Metallic character

A

Decreases across the period

Increase as u move down a group

Dense, shiny, good conductor of heat/electricity, easily loose e-

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6
Q

Paramagnetism

A

Partially filled d orbitals can be induced to magnetic field - weak and temporary

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7
Q

Nonmetals

A

Not dense
Not dull
Do not conduct heat electricity

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8
Q

Metalloids

A

Properties of metals and nonmetals
Dull or shiny
Partially conduct heat/electricity

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9
Q

Molar mass /atomic mass

A

G/mol

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10
Q

Mole to mass

A

Moles A x mole ration B/A x molar mass B = mass of B

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11
Q

Molar volume

A

At ideal conditions PV=nRT
0 degree C =32 Fahrenheit 273 K 1 atm

Mv = 22.4 L / mol

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12
Q

Percent yield

A

= Actual yield / theoretical yield x 100%

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13
Q

Dehydration reaction

A

Loss of H2O molecules from reactant

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14
Q

Condensation

A

Loss of h20 and forming new molecule together

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15
Q

Decomposition

A

Remove water from hydrates

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16
Q

Common strong acids

A

HCl
HI
HBr
HClO4 perchloric acid
H2SO4 sulfuric acid

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17
Q

Common strong bases

A

NaOH sodium hydroxide
KOH potassium hydroxide
LiOH lithium hydroxide
CsOH Caesium hydroxide
Ba(OH)2 Barium Hydroxide

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18
Q

Weak acids

A

HC2H3COOH ACETIC ACID
HF HYDROFLUORIC ACID
H3PO4 phosphoric acid
H2SO4 sulfurous acid
HClO hypochlorous acid

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19
Q

Weak bases

A

NH3 ammonia
NH4OH Ammonium hydroxide
CH3NH2 methyl amine
C6H5NH2 phenyl amine
C5H5N pyridine

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20
Q

Ligand

A

Neutral
Molecule or ion that has a lone pair e- to act as a Lewis base

Ex: h2O, ammonia, cyanide

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21
Q

Coordinated compounds

A

Transition metals with attached ligands

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22
Q

Complex ion

A

Ion made of transition metals with attached Ligands

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23
Q

Oxidation number

A

Primary valance electrons invoked in ionic binding

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24
Q

Coordination number

A

Secondary valance electrons involved in bonding to ligands

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25
Coordinate covalent bond
Ligands that bind to transition metals by donating both pairs of electrons
26
Common coordination numbers
Ag 2+ Cu 2,4+ Fe 6+ Ni 4,6 Cr 6+ Co 6+
27
Coordination numbers shape
2 linear 4 square planar 4 tetrahedral 6 octahedral
28
Enthalpy of bond energy
Delta H reaction = Delta H broken + delta H form Break bonds = + need energy Form bond = - release energy
29
Oxidation Reduction
Electrons are lost Electrons gained
30
Oxidizing agent. Reducing agent
Electrons gained. Electrons lost
31
Combustion reaction
Element or compound reacts with oxygen Producing energy as heat or light
32
Energy of cell =
Energy of cathode - energy of anode
33
Corrosion
Iron -anode looses electrons and cathode is h20 to alcohol which leads to iron oxide
34
Rate =
k [A]^m [B]^n
35
Arrhenius equation
k = A e^( -Ea/ RT) A frequency factor T kelvin R= 8.314 j/mol K
36
Equilibrium constant K
K = products / reactants In []
37
Le chateliers principle
Equilibrium shift to oppose change until new eq is reached Increase one side -> other side Exothermic shift left as new bonds release energy Endothermic shifts right ie energy in to break bonds Increase pressure with gases means less gases favored
38
Keq and Q
Q = Keq Q > Keq more p than r, shift to r till eq Q < Keq more r than p, shift to p till eq
39
Solubility product constant Ksp
Eq constant for solid substances dissolving in aq soln
40
Carbohydrates
Glucose Fructose Ribose Help hold together DNA Deoxyribose Lacks O or COOH group Helps bind DNA
41
Sugars
Monosaccharides Glucose Disaccharides Sucrose Formed by dehydration Trisaccharides Polysaccharides
42
Glycosidic bonds
Covalent bond between 2 monosaccharides May constrain N or S Generally more stable 1.4 or 1,6 binding
43
Cellulose
Fiber Thousands of glucose molecules together
44
Starch
Complex sugars amylopectin and amylose Mammals store as glycogen ie identical
45
Proteins
21 amino acids C H O N and S Se
46
Nucleic acids
DNA rna Deoxyribose and ribose plus phosphate
47
Carbohydrates
Carbons that are hydrated
48
Lipids
Fatty acids Hydrophobic and hydrophilic C O H
49
Peptide bind
Covalent bond holds amino acids together
50
Proteins
Large biological molecules Amino acids with peptide bonds Keratin- hair skin nails Enzymes ie decrease activation E Movements Actin - cell mobility Myosin - muscle contraction Transport fat Insulin control blood sugar Antibodies Transcription
51
Amino acids
Polar Non polar Proline - amine Cysteine- sulfur Glycine - no side chain
52
Four structures of proteins
Primary - order of Aminos Secondary - repetitive 3D structure Alpha, beta, random Tertiary - complete 3D structure of protein Quaternary - 3D structure of multiple proteins
53
Lipids
Biological dietary fats Insoluble in water Soluble in nonpolar solvents
54
Glycerol
Triglycerides Saturated fats No double binds Unsaturated fats Double bonds Trans fats Synthetic trans double bonds
55
Phospholipids
Glycerol attached to Phosphate - polar COOH - non polar Creates lipid bilayers
56
DNA rna
Deoxyribonucleic acid Ribonucleic acid
57
Nucleotide
Basic subunit of nuclein acid Phosphate group Nitrogenous base Suagr
58
Polynucleotide
Held together by Phosphodiester bond
59
Polynucleotide
Held together by Phosphodiester bond
60
Four nitrogenous bases in DNA
GATC GUANINE ADENINE THYMINE CYTOSINE
61
DNA strands are
Anti parallel but orientated opposite directions giving HELIX SHAPE
62
Watson crick Franklin
1953 paper deoxyribose High res images of dna fibers
63
DNA to rna to protein
Messenger rna Ribosomal rna Transfer rna
64
Isomer
Molecules has same chemical formula but different structures
65
Solubility rules
Group 1 elements Ammonium NH4+ Nitrates NO3- Chlorides Cl- except ag, hg, cl2, pb Sulfates SO4 2-
66
In solubility rules
Carbonates CO3 2- Hydroxides OH- Sulfides S 2-
67
Salt
2 ions Metal and non metal Electric charge 0 Strong ionic bond Crystalline structure Conduct electricity - electrolytes Hard and brittle
68
Acidity constant Ka Ph = PKa = Water pKa =
[H+][A-]/[HA] -log [H+] -log [Ka] 14
69
Dihydrogen phosphate Carbonic acid
H2PO4 H2CO3
70
Arrhenius acid Arrhenius base
Produce h+ Smell sour Produce OH- Soapy In solution
71
Bronsted- Lowry acid Bronsted-Lowry base
Proton donor Proton acceptor Does not have to be dissolved in water Conjugate acid: acid that form with proton Conjugate base: base that for with loss of proton
72
Lewis acid Lewis base
Accepts electron pair covalent bond Donates electron pair covalent bond
73
Amphoteric
Proton acceptor and donor H20
74
Self ionization constant of water Kw =
1.0x10^-14 = [h30+][Oh-]
75
Molar solubility
Ksp = [] [] Of what compound dissociates to Just like rate laws Ksp largest is most soluble
76
Titration Equivalence point
When H+ = OH- ie ph 7 Where [H+] (V of H+) = [Oh-] (v of oh-) Mol/L and L

Chem Praxis Notes (6 decks)

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