Final Vocabulary Flashcards
High specific gravity
large quantities of proteins in solutes-salts/sugar/proteins than solvent-water
Low specific gravity
much more solvent-water than solutes-salts/sugar/proteins (close to waters density)
Elements
pure substances
Compounds
pure substances
Mixtures
physical combination (NOT a pure substance)
Homogeneous mixture
mixed so well you CANNOT distinguish the different components visually
Heterogeneous mixture
you CAN distinguish the components but may need a microscope (e.g. blood, milk, etc.)
Physical property
properties that can be observed WITHOUT changing the identity of the substance under observation
Examples of physical properties
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]
Chemical property
can only be observed DURING a change in the identity of the substance under observation
Examples of chemical properties
E.g. a chemical might be corrosive, combustible, explosive, etc.
Physical change
a process that does NOT change the identity of the substance under observation (just a change in physical state)
Examples of physical change
E.g. melting, boiling, grinding, etc.
Chemical change
*Results in a formation of __ __ also called __.
a process that DOES change the identity of the substance under observation (formation of a new compound) → also called REACTIONS
Examples of chemical change
E.g. rusting, tarnishing, burning, etc.
Specific Heat
amount of heat required to raise the temperature of 1 gram of a substance 1℃
Conductors
have LOW specific heat, metals
Insulators
have HIGH specific heat, nonmetals
“Burning calories”
food is burned in a calorimeter to determine their energy values
Atomic radius
a length equal to half the distance between the nuclei of two covalently bonded atoms
Ionic radius
the distance from the nucleus to the outermost e- of an ion
Cation
*Size?
a positively charged ion of a metal
*Cations are much smaller
Anion
*Size?
a negatively charged ion
*Anions are somewhat larger
Ionic bonding
the attraction between positive and negative ions in an ionic compound
Covalent bonding
holds the shared atoms together and forms a molecule
Ionic Formulas
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
Molecular Formulas
Covalent molecules are composed of neutral atoms, not ions. To write the molecular formula you need to know the name of the molecule
Oxidizing agent (oxidant) *The species that’s being oxidized/reduced
The species in a reaction that causes another one to be oxidized
*The species that’s being reduced
Reducing agent (reductant) *The species that’s being oxidized/reduced
The species in a reaction that causes another one to be reduced
*The species that’s being oxidized
Typically an individual element is __
An individual species (reactant) is the __
Typically an individual element is oxidized/reduced
An individual species (reactant) is the oxidant/reductant
Intramolecular interactions
inside molecules
Intermolecular interactions
between molecules
Electronegativity
the ability of an atom to attract electrons to itself
Transfer of electrons: __ interaction
ionic interaction
Unequal-sharing of electrons: __ bond
polar covalent bond
Equal-sharing of electrons: __
nonpolar covalent bond
Nonpolar Molecules have a __ shape with __ exterior atoms
Symmetrical shape (generally no lone pairs on central atom) with exterior atoms all the same
Polar Molecules have a __ shape with __ exterior atoms
*It can be __ combination of atoms with a ___ geometry
Symmetrical geometry (no lone pairs) with different exterior atoms *ANY combination of atoms with a nonsymmetrical geometry (lone pairs)
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 =
Present in polar molecules
- The larger the difference in electronegativity within a molecule, the greater the dipole-dipole interaction
- X and Y = nonmetals
Hydrogen Bonding
- Strength
- Special type of __ bonding
- Strength is limited by:
- Present ONLY between molecules with:
- 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
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.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)
Strength of bonds and attractive forces:
- Ionic bond
- Covalent bond
- Hydrogen bond
- Dipole-dipole attractions
- Dispersion forces
Strong:
- Ionic bond
- Covalent bond
Somewhat strong:
- Hydrogen bond
- Dipole-dipole attractions
Weak:
-Dispersion forces
Dispersion forces are
Temporary shift of electrons in nonpolar bonds
