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Spring 2013 / Biochemistry > Lecture 1 Inorganic Chemistry Basics > Flashcards

Lecture 1 Inorganic Chemistry Basics Flashcards

1
Q

what is INORGANIC CHEMISTRY?

A

chemistry of elements, reactivity, and atomic relationships that are based on elements and their properties

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2
Q

what is ORGANIC CHEMISTRY?

A

chemistry of CARBON, it’s reactivity and relationships with other elements and the compounds of carbon makes

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3
Q

what is the sub division of ORGANIC CHEM?

A
  1. biological

2. non-biological

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4
Q

what is HYLOZOISM?

A

doctrine that all matter has life

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5
Q

what is an ATOM?

A

single nucleus made of protons and neutrons, with a cloud of orbiting electrons

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6
Q

what determines the ELEMENT of the atom?

A

count of protons in a nucleus

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7
Q

what are the characteristics of neutrons?

A

no electrical charge
balances the instability of positively charged protons
(protons + neutrons = nucleus)

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8
Q

what is SUB-ATOMIC PARTICLES?

A

means atomic particles are divisible

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9
Q

name the smallest unit –> largest unit

A

particle –> atom –> element –> molecule –> macromolecule

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10
Q

what are the characteristics of HYDROGEN ATOM?

A
  1. 1st element
  2. only element normally w/o NEUTRON
  3. when it is UNADULTERATED, it has neutral charge [proton (+1) + electron (-1) = 0]
  4. it becomes HYDROGEN ION (or H+, or proton) when ELECTRON is stripped away
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11
Q

what determines the CHEMICAL PROPERTIES of an element?

A

of ELECTRONS orbiting nucleus

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12
Q

what is VALENCE?

A
  • the characteristic # of electrons lost or gained from the electron cloud of atom
  • valence # determines element’s chemical conduct with other elements
  • POS VAL: less electrons than protons
  • NEG VAL: more electrons than protons
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13
Q

how is a molecule formed?

A

when 2 or more atoms interact and bind together by electron behaviors

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14
Q

what gives each element’s its CHEMICAL CHARACTERISTICS?

A

the VARIABILITY of electron count (which is the valence)

[ideal atom: electron=protons, but electrons count can vary easily]

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15
Q

layers or electron shells

A

energetic states of electron cloud, which become increasingly complex as # of electrons increase with the # of protons

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16
Q

ISOTOPE

A

varying neutron count

*but never less neutrons than protons, except in hydrogen

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17
Q

periodic table

A

chart of all elements found in nature and synthetic elements created in nuclear reactors

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18
Q

periodicity

A

valence state of each element

19
Q

valence state

A

charge state
(most common loss or gain of electrons from the electron cloud by a particular element)
ex: NA +1 (it easily looses 1 electron, leaving +1 of atom)

20
Q

ELECTRONEUTRALITY

A

most important concepts in chemistry

  • atoms and molecules are powered by thermodynamic laws of physics and are driven to attain electrically neutral state
  • create cellular energy
21
Q

what re 2 STRONG BONDS?

A
  1. ionic bond

2. covalent bond

22
Q

covalent bond

A
  • freely share electrons

- most common bonds in biochemistry –> almost all CARBON compounds are covalently bonded

23
Q

ionic bonds

A
  • charge polarities in molecules create electronic attractions of +/- which link atoms by attraction to their opp charge
  • form crystalline structures (most minerals & rocks)
24
Q

hydrogen bonds

A
  • weak bonds
  • weak attraction of a covalently bonded hydrogen to any adjacent neg charged atom like oxygen
  • sub-par electrochemcial bond
  • ex: cellulouse (paper, wood), DNA, RNA
25
Q

what are the 2 weak bonds

A
  1. hydrogen bonds

2. Van der Waals forces

26
Q

polarity

A
  • having a pos and neg-charged side
  • asymmetric imbalance of electronic charge
    [ex: H2O is stable, but has a net off-balanced charge –> H +1, H+1, O-2]
27
Q

non-polarity

A

symmetrical distribution of its atoms (neutral balanced charge due to the balance of its structure)

28
Q

ion

A

an atom that is dissolved in water and has either a pos or neg charge

29
Q

molecule

A

2 or more atoms that are bounded together creating complexity

30
Q

macromolecule

A

huge # of molecules bonded together to form giant molecules

31
Q

characteristics of WATER

A
  • polarized molecule (has pos & neg region), which make it a powerful dissolving agent
32
Q

dissolution

A

when ionic compound, like NaCl dissolves in water, the sodium (+1) and chlorine (-1) go into solution, and salt crystals is broken up, the atoms distributed throughout the water, but still electrically neutral

33
Q

dissolution potential

A

determines how easily or how much of compound will dissolve in water

34
Q

Do covalent molecules dissolve in water?

A

yes, but they do not dissociate –> their asymmetrical charge distribution, as in glucose, allows the polarity of water to put the molecule into solution

35
Q

solubility

A
  • polar substance dissolve in polar fluids like water

- non-polar substances will dissolve in non-polar fluids like carbon tetrachloride or oils

36
Q

cations

A

pos charge

ex: Na+, Ca+2

37
Q

anions

A

neg charged

ex: Cl-, PO4-

38
Q

salt

A
  • ionic compounds, when anions and cations crystalize together
  • water-based environment of body fluids are salty due to ionizing nature of water creating cations and anions (body needs 2g of sodium per day)
39
Q

pH

pH 7

A

percent hydrogen ions

percent of hydrogen where acid and base (alkaline) properties are equal on a scale of 1-14

40
Q

acid

A

simple acid compound is sulfuric acid (H2SO4) -> has 2 hydrogen cations compound with 1 sulfate anion
- acid usually has hydrogen as cation
readily reacts with other substances in corrosive way, bc their power to ionize can be very strong
- DNA & citric acid are examples of an acid

41
Q

hydronium

A

H3O+

H+

42
Q

what is the most common anion that produces BASIC solution?

A

hydroxide ion OH-

the more OH- dissociates into water, the more powerful the base

43
Q

what is a simple base (alkaline)?

A

sodium hydroxide (or lye - ex: draino), an ionic compound
NaOH
the “basic” part of this compound as it dissolves is the OH- moiety, like H+, OH- is corrosive

Spring 2013 / Biochemistry (13 decks)

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