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CHEM 155: Gen Chem 1 > CH. 3 > Flashcards

CH. 3 Flashcards

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1
Q

metal atom

A

becomes a cation (a positively charged ion)

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2
Q

nonmetal atom

A

becomes an anion (a negatively charged ion )

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3
Q

formation of ionic compound

A

a metal loses an electron (Na+), a nonmetal gains electron, (Cl-)

  • oppositely charged ions are held together by ionic bonds,
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4
Q

covalent bond // ( molecular compounds)

A
  • when nonmetal bonds with another nonmetal, electrons are not transfered but rather shared
  • there are NO ions!! No charges!!
  • electrically neutral
  • gives accurate representation of the compound
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5
Q

Chemical formulas

A

empirical (relative): CH

molecular (actual): C2H2

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6
Q

Diatomic molecules (molecular elements)

A

H2(hydrogen), N2 Nitrogen), O2 (oxygen), F2 (fluoride), Cl2 (chlorine), Br2 (bromine), I2 (iodine)

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7
Q

polyatomic ions

A

ion composed of two or more atoms

- a compound composed of a metal and a polyatomic ion; therefore, is an ionic compound

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8
Q

atomic element

A
  • single atoms as their basic unit

Ex: Xenon

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9
Q

Difference between ionic and molecular compounds

A
  • Molecular compounds contain highly directional covalent bonds, which result in the formation of molecules.
  • Ionic compounds contain nondirectional ionic bonds, which result (in the solid state) in the formation of ionic lattices
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10
Q

Naming molecular compounds (two or more nonmetals)

A

(prefix)(name of first element)(prefix)(base name of 2nd element + -ide)

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11
Q

Prefixes for molecular compounds (two or more nonmetals!!)

A
  • mono = 1 (ommitted for the first element in the formula)
  • di = 2
  • tri = 3
  • tetra = 4
  • penta = 5
  • hexa = 6
  • hepta = 7
  • octa = 8
  • nona = 9
  • deca = 10
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12
Q

acids

A
  • molecular compounds that release hydrogen ions when dissolved in water
  • usually written first in their formula, and one or more nonmetals, written second
  • sour taste
  • ability to dissolve many metals
  • 2 types: binary acids and oxyacids
  • formula has H as first element
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13
Q

aqeous

A
  • dissolved in water
  • Ex: HCl (aq): hydrochloric acid (an acid when dissolved in water)
    • differs from HCl (g) - hydrogen monochloride
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14
Q

Naming Binary Acids

A
  • Hydrogen and a nonmetal
  • (hydro)(base name of nonmetal + -ic)(acid)

ex: HCl (aq): hydrochloric acid
HBr (aq): hydrobromic acid
HI (aq): hydroiodic acid

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15
Q

Naming OxyACIDS

A
  • contain hydrogen and an oxyanion (an anion containing a nonmetal and oxygen)
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16
Q

How do chemical bonds form?

A
  • chemical bonds form because of the attractions between charged particles (the electrons and protons) that compose atoms
  • like charges repel, opposite charges attract
17
Q

empirical formula vs. molecular formula

A
  • empirical: gives the relative number of atoms of each element in a compound – communicates least information
    (H2O2 –> HO)
  • molecular: gives the actual number of atoms of each element in a molecule of a compound ; indicates the number and type of each atom in the molecule
    (H2O2)
18
Q

structural formula

A
  • a molecular formula that uses lines to represent covalent bonds and shows how atoms in a molecule are connected or bonded to each other, communicates most information about a compound
  • indicates how atoms connect
  • can also depict the different types of bonds that occur within molecules
  • H20: H – O – O – H
  • CO2: O = C = O (double bonds)
19
Q

Ball - and - stick molecular model

A
  • represents atoms as balls and chemical bonds as sticks; how the two connect reflects a molecular shape
  • portrays geometry of molecule
  • balls are typically color coded:
    • carbon = black
    • hydrogen = white
    • nitrogen = blue
    • oxygen = red
20
Q

Space-filling molecular model

A
  • atoms fill up the space between each other to more closely represent our best estimates for how a molecule might appear if scaled to visible size
  • gives the best sense of the relative sizes of the atoms and how they merge together in bonding
21
Q

Based on what you learned in Chapter 2 about atoms, what part of the atom do you think the spheres in the molecular space-filling models shown in the table below represent? If you were to superimpose a nucleus on one of these spheres, how big would you draw it?

A
  • Each sphere represents the electron cloud of the atom. The nucleus would be too small to see on the same scale.
22
Q

Ionic compound formulas

A
  • always contain positive and negative ions
  • In a chemical formula, the sum of the charges of the positive ions (cations) must equal the sum of the charges of the negative ions (anions)
  • the formula of an ionic compound reflects the smallest whole-number ratio of ions
23
Q

Which metal has the same charge in all of its compounds?

A

Ans: “Sr”

  • Most transition metals can form more than one kind of cation and its charge must then be specified for a given compound
24
Q

Naming Binary Ionic Compounds Containing a Metal that Forms ONLY ONE type of Cation

A
  • contain only two different elements
  • (name of metal cation)(base name of nonmetal anion + -ide)

Ex: KCl: Potassium Chloride
CaO: Calcium Oxide

25
Q

Naming Binary Ionic Compounds Containing a Metal That Forms More Than One Kind of Cation

A

Fe 2+: Iron (II)
Fe 3+: Iron (III)

  • (name of metal cation) (charge of metal cation in Roman numerals in parentheses) (base name of nonmetal anion + -ide)
  • PbCl4: lead(IV) chloride
26
Q

Hydrated Ionic Compounds

A
  • ionic compounds containing a specific number of water molecules associated with each formula unit
  • waters of hydration can usually be removed by heating the compound
  • “prefixhydrate”
27
Q

Common Hydrate prefixes

A
  • hemi = 1/2
  • mono = 1
  • di = 2
  • tri = 3
  • tetra = 4
  • penta = 5
  • hexa = 6
  • hepta - 7
  • octa = 8
28
Q

Formula Mass

A
  • Formula Mass = [(# of atoms of 1st element in chemical formula) x Atomic Mass of element] + [(# of atoms of 2nd element in chemical formula) x (Atomic mass of 2nd element)]
  • Ex: Formula mass of CO2:
    (1)(12.01 amu) + (2)(16.00amu)
    = 440.1 amu
29
Q

Molar Mass

A
  • mass in grams of 1 mol of its molecules or formula units
  • numerically equivalent to its formula mass
  • Ex) CO2:
    • Formula mass = 44.01 amu
    • Molar Mass = 44.01 g/mol
30
Q

Mass percent composition (aka mass percent)

A
  • an element’s percentage of the compounds total mass

- Mass percent of element X = (mass element C in q1 mol of compound / mass of 1 mol of the compound) x 100%

31
Q

Without doing any calculations, list the elements in C6H6O in order of decreasing mass percent composition.

A
  • C > O > H
  • Since carbon and oxygen differ in atomic mass by only 4 amu, and since there are six carbon atoms in the formula, we can conclude that carbon constitutes the greatest fraction of the mass. Oxygen is next because its mass is 16 times that of hydrogen and there are only six hydrogen atoms to every one oxygen atom.

CHEM 155: Gen Chem 1 (5 decks)

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