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CHEM 120 SUMR'DONE > Final Vocabulary > Flashcards

Final Vocabulary Flashcards

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1
Q

High specific gravity

A

large quantities of proteins in solutes-salts/sugar/proteins than solvent-water

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2
Q

Low specific gravity

A

much more solvent-water than solutes-salts/sugar/proteins (close to waters density)

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3
Q

Elements

A

pure substances

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4
Q

Compounds

A

pure substances

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5
Q

Mixtures

A

physical combination (NOT a pure substance)

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6
Q

Homogeneous mixture

A

mixed so well you CANNOT distinguish the different components visually

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7
Q

Heterogeneous mixture

A

you CAN distinguish the components but may need a microscope (e.g. blood, milk, etc.)

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8
Q

Physical property

A

properties that can be observed WITHOUT changing the identity of the substance under observation

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9
Q

Examples of physical properties

A

E.g. temp at which a substance changes state (boiled water is still water), size, malleability, conductivity, density, etc.
[Solid→Gas = sublimation] [Gas→Solid = deposition]

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10
Q

Chemical property

A

can only be observed DURING a change in the identity of the substance under observation

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11
Q

Examples of chemical properties

A

E.g. a chemical might be corrosive, combustible, explosive, etc.

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12
Q

Physical change

A

a process that does NOT change the identity of the substance under observation (just a change in physical state)

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13
Q

Examples of physical change

A

E.g. melting, boiling, grinding, etc.

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14
Q

Chemical change

*Results in a formation of __ __ also called __.

A

a process that DOES change the identity of the substance under observation (formation of a new compound) → also called REACTIONS

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15
Q

Examples of chemical change

A

E.g. rusting, tarnishing, burning, etc.

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16
Q

Specific Heat

A

amount of heat required to raise the temperature of 1 gram of a substance 1℃

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17
Q

Conductors

A

have LOW specific heat, metals

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18
Q

Insulators

A

have HIGH specific heat, nonmetals

19
Q

“Burning calories”

A

food is burned in a calorimeter to determine their energy values

20
Q

Atomic radius

A

a length equal to half the distance between the nuclei of two covalently bonded atoms

21
Q

Ionic radius

A

the distance from the nucleus to the outermost e- of an ion

22
Q

Cation

*Size?

A

a positively charged ion of a metal

*Cations are much smaller

23
Q

Anion

*Size?

A

a negatively charged ion

*Anions are somewhat larger

24
Q

Ionic bonding

A

the attraction between positive and negative ions in an ionic compound

25
Q

Covalent bonding

A

holds the shared atoms together and forms a molecule

26
Q

Ionic Formulas

A

Ionic compounds are composed of ions. If you know the ions that make up the compound, you can write the formula (formula unit). DROP, SWAP, REDUCE

27
Q

Molecular Formulas

A

Covalent molecules are composed of neutral atoms, not ions. To write the molecular formula you need to know the name of the molecule

28
Q 
Oxidizing agent (oxidant)
*The species that’s being oxidized/reduced
A

The species in a reaction that causes another one to be oxidized
*The species that’s being reduced

29
Q 
Reducing agent (reductant)
*The species that’s being oxidized/reduced
A

The species in a reaction that causes another one to be reduced
*The species that’s being oxidized

30
Q

Typically an individual element is __

An individual species (reactant) is the __

A

Typically an individual element is oxidized/reduced

An individual species (reactant) is the oxidant/reductant

31
Q

Intramolecular interactions

A

inside molecules

32
Q

Intermolecular interactions

A

between molecules

33
Q

Electronegativity

A

the ability of an atom to attract electrons to itself

34
Q

Transfer of electrons: __ interaction

A

ionic interaction

35
Q

Unequal-sharing of electrons: __ bond

A

polar covalent bond

36
Q

Equal-sharing of electrons: __

A

nonpolar covalent bond

37
Q

Nonpolar Molecules have a __ shape with __ exterior atoms

A

Symmetrical shape (generally no lone pairs on central atom) with exterior atoms all the same

38
Q

Polar Molecules have a __ shape with __ exterior atoms

*It can be __ combination of atoms with a ___ geometry

A 
Symmetrical geometry (no lone pairs) with different exterior atoms
*ANY combination of atoms with a nonsymmetrical geometry (lone pairs)
39
Q

Dipole-dipole Forces are present in __ molecules

  • The larger the difference in electronegativity within a molecule, the greater/smaller the dipole-dipole interaction.
  • X and Y =
A

Present in polar molecules

  • The larger the difference in electronegativity within a molecule, the greater the dipole-dipole interaction
  • X and Y = nonmetals
40
Q

Hydrogen Bonding

  • Strength
  • Special type of __ bonding
  • Strength is limited by:
  • Present ONLY between molecules with:
A
  • VERY STRONG
  • Special type of dipole-dipole bonding
  • Limited by the number of lone pairs on the central atom
  • Present ONLY between molecules with: N-H, O-H, and H-F bonds
41
Q

London Forces
A.k.a.
-The __ the mass of the molecules, the __ the London forces
-The __ the surface-to-surface contact between molecules, the __ the London forces
-Due to __ electron movement (Swishing)

A

A.k.a. van der Waals force and dispersion force

  • The larger the mass of the molecules, the stronger the London forces
  • The larger the surface-to-surface contact between molecules, the stronger the London forces
  • Due to transient electron movement (Swishing)
42
Q

Strength of bonds and attractive forces:

  • Ionic bond
  • Covalent bond
  • Hydrogen bond
  • Dipole-dipole attractions
  • Dispersion forces
A

Strong:

  • Ionic bond
  • Covalent bond

Somewhat strong:

  • Hydrogen bond
  • Dipole-dipole attractions

Weak:
-Dispersion forces

43
Q

Dispersion forces are

A

Temporary shift of electrons in nonpolar bonds

CHEM 120 SUMR'DONE (9 decks)

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