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Chem Fall 101 > Chapter 3 > Flashcards

Chapter 3 Flashcards

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1
Q

covalent bonds

A

sharing electrons

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2
Q

ionic bonds

A

transferring electrons

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3
Q

molecular compound

A

nonmetal atoms with covalent bonds

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4
Q

empirical formula

A

shows types of atoms present in the simplest whole-number ration ex// P2O5; not P4O10

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5
Q

molecular formula

A

based on the actual molecule ex// P4O10; not P2O5

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6
Q

structural formula

A

-order in which atoms are bonded together -what types of bonds ex// O=C=O

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7
Q

organic compounds

A

made up of C and H -may contain O or N

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8
Q

line angle formula/line structure

A

hexagon shaped things

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9
Q

ionic compound

A

made of positive and negative ions joined together by electrostatic forces of attraction

-metal atoms lose electrons, nonmetals gain

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10
Q

cation

A

positive ion

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11
Q

anion

A

negative ion

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12
Q

formula unit

A

smallest electrically neutral collection of ions

(ratio of atoms is the same as in the chem formula)

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13
Q

monatomic

A

a single ionized atom

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14
Q

polyatomic

A

2+ atoms

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15
Q

formula mass

A

mass of a forumla unit in atomic mass units

ex// Mg(NO3)2 = 24.3050 u + 2[14.0067 u + 3)15.9994 u)]

= 148.3148 u

(also known as molecular mass and atomic mass)

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16
Q

molar mass

A

mass of 1 mole of compound

ex// 1 mol H2O = 18.0153 g H2O = 6.022 x 10^23 molecules

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17
Q

allotropy

A

element exists in 1+ molecular forms

ex// oxygen exists in O2 and O3

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18
Q

determining percent composition

A
  1. determine the molar mass of the compound (denominator)
  2. determine the contribution of the given element to the molar mass (numerator)
  3. formulate the ratio of the mass of the given element to the mass of the compound as a whole
  4. multiply the ratio by 100% to obtain mass percent

mass % = [(# of atoms of element per formula unit) x molar mass of element]/molar mass of compound x 100%

19
Q

determining formula of an unknown compound

A
  1. take 100 g of the masses; given mass percent
  2. convert masses of the elements in the 100 g sample to amounts in moles
  3. write tentative formula
  4. attempt to convert subscripts to smalles whole number by dividing each of the subscripts by smallest one
  5. then multiply if still not whole number

*gives empirical formula*

20
Q

combustion analysis

A

sample of a compound is burned in a stream of oxygen gas

To Determine Empirical Formula

  1. determine mass of carbon in x g CO2 by first convert to mol, then g.
  2. do same for H2O for hydrogen
  3. take total mass of sample and subract mass of H and C
  4. convert grams of O to mols
  5. plug into CHO formula
  6. divide and multiply subscripts for formula
21
Q

oxidation state

A

number of an element that corresponds with how many electrons gained/lost

eg. NaCl

Na has a +1 oxidation state

Cl has a -1 oxidation state

eg. MgCl2

Mg: +2 state

Cl: -1 state (b/c 2 of them)

22
Q

rules for applying oxidation states

A

*rules to be applied in numerical order and whenever two rules contradict, go by the lower numbered rule*

  1. OS of an individual atom in a free element is 0.
  2. total of the OS of all atoms in the
    a. neutral species, like isolated atoms, molecules, and formula units, is 0
    b. an ion is equal to the charge on the ion
  3. in their compounds, the group 1 metals have an OS of +1 and group 2 metals have an OS of +2 (eg. OS of K in KCl is +1, OS of Mg is +2 in MgBr2
  4. in its compounds, OS of fluorine is -1
  5. in its compounds, OS of hydrogen is usually +1
  6. in its compounds, OS of oxygen is usually -2
  7. in binary (2-element) compounds w/ metals, group 17 elements have an OS of -1; group 16, -2, group 15, -3
23
Q

organic compound

A

compound formed by carbon and hydrogen

(orgo)

-mostly molecular; few are ionic

24
Q

binary compounds

A

formed by 2 elements

25
Q

naming ionic compounds

A

metal + nonmetal = ionic compound

  1. write unmodified name of metal
  2. modfy end of nonmetal to -ide
    eg. NaCl = sodium chloride
    eg. MgI2 = magnesium iodine = magnesium iodide
    - must be electrically neutral
26
Q

-ous and -ic

A
  • ous = for the lower oxidation state
  • ic = high oxidation state
27
Q

molecular compound

A

nonmetal + nonmetal

  • naming is similar to ionic compound
  • write the eleemnt with the positive oxiation state first
    eg. HCl not ClH
  • indicate relative number of atoms through prefixes

(mono = 1, di = 2 , tri = 3, tetra = 4, penta = 5, hexa = 6, hepta = 7, octa = 8, nona = 9, deca = 10)

eg. B2Br4 = diboron tetrabromide

*do not use mono for first named element

eg. NO = nitrogen monoxide, not mononitrogen monoxide

28
Q

acid

A

substance that ionizes/breaks down in water to produce H+ anions

-molecular compound

29
Q

binary acid

A

2 lement compound of H and a nonmetal

eg. HCl

30
Q

bases

A

yield OH- in aqueous solutions

31
Q

naming binary acids

A

use prefix hydro- and other nonmetal modified w/ -ic

eg. HF = hydrofluoric acid

32
Q

polyatomic ions

A
  1. anions more common than cations
  2. very few polyatomic anions carry the -de ending in their names (exceptions = OH- (hydroxide ion) and CN- (cyanide ion); common endings are -ite/-ate and some w/ prefixes (hypo-, per-)
  3. oxygen is common to many polyatomic anions, called oxoanions
  4. certain nonmetals form a series of oxoanions containing different numbers of oxygen atoms; names are related to oxidation state of the nonmetal atom to which the O atoms are bonded

(low to high)

hypo__ite, __ite, __ate, per__ate

  1. all common oxoanions of Cl, Br, I carry a charge of 1-
  2. some series of oxoanions also contain various numbers of H atoms and are named accordingly
    eg. HPO4(2-) is the hydrogen phosphate ion, and H2PO4(-) is the dihydrogen phosphate ion
  3. prefix thio- means sulfur has been substituted for an oxygen
33
Q

ternary compounds

A
  • majority of acids are ternary compounds
  • contain 3 diffeernt elements; H and 2 other nonmetals
  • if one of the nonmetals is oxygen, the acid is called an oxoacid
  • naming oxoacids is ame as for oxoanions, but ending -ous is used instead of ite, and -ic instead of -ate
34
Q

salts

A

hydrogen of the oxoacid has been replaced w/ a metal

-ionic compounds

35
Q

hydrate

A

each formula unit of the compound has associated w/ it a certain # of water molecules

eg. CoCl2 x 6 H2O
- if water is removed by heating, compound is called anhydrous

36
Q

hydrocarbons

A

only C and H

37
Q

alkanes

A

hydrocarbons w/ only single bonds

  • name by using a word stem + ending -ane
    eg. C5H12 = pentane; C7H16 = heptane
38
Q

alkenes

A

hydrocarbons w/ 1+ double bonds

39
Q

methyl group

A

CH3 group

40
Q

isomers

A

molecules w/ same molecular formula but different arrangement of atoms

41
Q

alcohols

A

-presence of one -OH (replaces an H atom)

42
Q

functional group

A

individual atoms or groups of atoms that are attached to the carbon chains/rings of organic moecules and give the molecules their characteristic properies

-increases possibility of isomers

43
Q

-OH group

A

hydroxyl

44
Q

-COOH

A

carboxyl group

  • aka CO2H
  • acidic properties
  • H attached to one of the O atoms is ioniziable/acidic
  • carboxylic acid

*methanoic acid/formic acid = HCOOH

*ethanoic acid/acetic acid = CH3COOH

-when a halogen is substituted for 1+ H atoms, named: fluoro-, chloro-, bromo-, iodo-

Chem Fall 101 (3 decks)

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