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chemistry > GIANT FINALS STUDY SESH > Flashcards

GIANT FINALS STUDY SESH Flashcards

1
Q

science

A

the knowledge obtained by observing natural events and conditions in order to discover facts and formulate laws or principles that can be verified or tested

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2
Q

chemistry

A

the study of the composition, structure, and properties of matter and the changes that matter undergoes

composition: what a molecule is made up of (i.e. matter, atoms)
structure: the shape that gives a molecule it’s properties

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3
Q

chemical

A

any substance that has a definite composition or is used or produced in a chemical process

definite composition: ethanol

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4
Q

basic vs applied research

A

basic: carried out to increase general knowledge
applied: carried out to solve practical problems

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5
Q

matter vs mass

A

matter: has mass and takes up space
mass: a measure of the amount of matter

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6
Q

chemical properties

A

a substance’s ability to undergo changes (a reaction) that alter its composition and identity

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7
Q

element vs compound

A

element: composed of one kind of atom
compound: made from two or more elements in fixed proportions

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8
Q

physical vs chemical changes

A

physical: the identity of a substance IS NOT changed
(i. e. change of state, crumbling)

chemical: the identity of a substance CHANGES
(i. e. combustion, oxidation)

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9
Q

what are the three major states of matter?

A

solid, liquid, gas

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10
Q

anything that happens with matter requires…

A

energy!!!

  • energy accompanies both physical and chemical changes
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11
Q

energy, mass, and matter are neither…

A

created nor destroyed

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12
Q

mixtures vs pure substances

A

mixtures: two or more different substances joined together (not chemically)

pure substances: consisting of one element or compound

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13
Q

periodic table

A

an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column

  • elements organized by chemical properties
  • columns = groups
  • rows = periods
  • same periods = same outer valence shell configuration
  • same groups = similar properties

s-block, p-block, d-block, and f-block

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14
Q

what are the different classifications?

A
  • metals: shiny, malleable, ductile, good conductors
  • nonmetals: brittle, poor conductors
  • metalloids: intermediate in properties between metals and nonmetals
  • noble gases: unreactive
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15
Q

scientific method

A

a logical approach to solving problems that lend themselves to investigation

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16
Q

hypothesis vs theory

A

hypothesis: a TESTABLE statement that serves as the basis for predictions and further experiments
(if. .. then…)

theory: a broad generalization that explains a body of known facts or phenomena
- can change over time

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17
Q

what is the result of nearly every measurement?

A

a number and a unit

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18
Q

SI system

A

a system of measurement used in science consisting of…

  • meters (length)
  • kilograms (mass)
  • seconds (time)
  • kelvin (temperature)
  • mole (amount of substance)
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19
Q

weight

A

a measure of the gravitational pull on matter

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20
Q

derived SI units

A
  • square meter (area)

- cubic meter (volume)

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21
Q

density

A
  • the level of compactness of a substance
  • the ration of mass to volume
  • density = mass/volume
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22
Q

conversion factors

A

used to convert from one unit to another

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23
Q

accuracy vs precision

A

accuracy: the closeness of a measurement to the correct or accepted value
precision: the closeness of values for a set of measurements

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24
Q

significant figures

A

consist of all digits known with certainty plus one final digit, which is uncertain

  • answer should have the same amt of sigfigs as the number that has the fewest sigfigs
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25
Q

exact conversion factors

A

completely certain and do not limit the number of digits in a calculation
i.e. avogadro’s number

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26
Q

directly vs inversely proportional

A

directly proportional: dividing one by the other yields a constant value

  • increase in a = increase in b
  • a/b = c

inversely proportional: their product has a constant value

  • ab = c
  • increase in a = decrease in b
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27
Q

history of atoms

A
  • atoms have been around since ancient Greece
  • in the 19th century, John Dalton proposed a scientific theory of atoms than can still be used to explain properties of most chemicals today
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28
Q

mass ratios

A
  • always the same, regardless of how much of the compound there is or how it was formed
  • if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element can be expressed as a ration of small whole numbers
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29
Q

cathode-ray tubes

A

supply evidence of the existence of electrons, which are negatively charged subatomic particles that have relatively little mass

  • measured the charge-to-mass ratio of an electron
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30
Q

properties of the nucleus

A
  • positive
  • small
  • dense
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31
Q

atomic nuclei

A
  • Rutherford found evidence for the existence of the atomic nucleus by bombarding gold foil with a beam of positively charged particles
  • atomic nuclei are composed of protons and electrons
  • atomic nuclei have a radii of about 0.001 pm and atoms have a radii of about 40-270 pm
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32
Q

protons vs neutrons vs electrons

A

protons: electric charge of +1
electrons: electric charge of -1
neutrons: no electric charge

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33
Q

atomic number vs mass number

A

atomic number: equal to the number of protons of an atom

mass number: equal to the total number of protons and neutrons that make up the nucleus of an atom

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34
Q

unified atomic mass unit

A

based on the carbon-12 atom and is a unit for measuring the mass of atoms
- equals 1.660 540 x10^23

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35
Q

average atomic mass

A

formed by calculating the weighted average of the atomic masses of the naturally occuring isotopes of the element

36
Q

isotopes

A

two of the same elements with different # of neutrons

37
Q

avogradro’s number

A

approx 6.022 x10^23

  • a sample that countains a number of particles equal to avo’s number contains a mole of those particles
38
Q

what nature does light have?

A

dual wave-particle nature

39
Q

quantum theory

A

electrons can exist only at specific atomic energy levels

  • developed to explain observations such as photoelectric effect and the line-emission spectrum of hydrogen
  • when an electron moves from one main energy level to a main energy level of lower energy, a photon is emitted. the photon’s energy equals the energy difference between two levels
  • when an electron moves from one main energy level to a higher main energy level, a an amount of energy is absorbed, accounting for the difference between the two levels
40
Q

photoelectric effect

A

the emission of electrons from a metal when light shines on it

  • proposed by my boi Albert #HeARealOne
41
Q

hydrogen’s line-emission spectrum

A
  • investigators passed an electric current through a tube containing hydrogen gas at low pressure, producing a pink glow
  • this light was shined through a prism, separating it into four colors of the visible spectrum (known as hydrogen’s line-emission spectrum)
42
Q

what nature do electrons have?

A

dual wave-particle nature

43
Q

Heisenberg uncertainty principle

A

it is impossible to determine simultaneously the position and velocity of an electron or any other particle

44
Q

orbital

A

a three-dimensional region around the nucleus that shows the region in space where an electron is most likely to be found

45
Q

quantization of electron energies

A

a natural outcome of the Schrodinger wave equation, which describes the properties of an atom’s electrons

46
Q

four quantum numbers

A

properties of electrons in atomic orbitals

principal quantum number (n): indicates the main energy level occupied by the electrons
- n = 1, 2, 3…

angular momentum quantum number (l): indicates the shape of the orbital
- l = 0, 1, 2… (n-1)

magnetic quantum number (m sub l): indicates the orientation of an orbital around the nucleus
- ml = -1, 0, +1

spin quantum number (m sub s): has only two possible values, +1/2 or -1/2, which indicates states of an electron in an orbital

  • spin/arrow going up = +1/2
  • spin/arrow going down = -1/2
47
Q

what are the three principals in which the ground-state electron configuration of an atom can be written?

A

Aufbau principle: an electron occupies the lowest energy orbital that can receive it
(orbitals most be filled lowest to highest)

Hund’s rule: orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state
(one orbital must be added to each section before pairing)

Pauli exclusion principle: no two electrons in the same atom can have the same set of four quantum numbers
(no two electrons can be facing up or facing down)

48
Q

what are the three different types of notation that electron configurations can be depicted by?

A

orbital notation: notation with lines and arrows representing electron configurations

electron-configuration notation: spaces with a lower energy level are filled first until desired element is reached
- 1s2 2p2 2p6 3p2

noble-gas notation: an outer main energy level occupied by eight electrons and abbreviated using the symbol for the noble gas in brackets
- [He] 2s2 2p4

49
Q

periodic law

A

the physical and chemical properties of the elements are period functions of their atomic numbers

50
Q

ionic vs covalent vs metallic compounds

A

ionic: metal & nonmetal
covalent: nonmetal & nonmetal
metallic: metal & metal

51
Q

cations vs anions

A

cation: lose one electron to form positive ion
anion: gain one electron to form negative ion

52
Q

molecular vs ionic bonds

A

molecular bonds: SHARE electrons

ionic bonds: transfer electrons

53
Q

noble gases

A
  • unique chemical stability
  • highest occupied levels have an octet of electrons (ns2 np6)
  • generally unreactive
54
Q

valence electrons

A

electrons in an atom that are available to be lost, gained, or shared in the formation of chemical compounds

55
Q

electron affinity, electronegativity, and ionization energy

A

electron affinity: the energy change that occurs when an electron is acquired by a neutral atom (energy it takes to ADD an electron)
-increases to the right and up

electronegativity: the measure of the ability of an atom in a chemical compound to attract electrons from another atom in a compound
- increases to the right and up

ionization energy: the energy required to remove one electron from a neutral atom of an element
- increases going to the right and up

56
Q

atomic radius vs ionic radius

A

atomic radius: one-half of the distance between the nuclei of identical atoms that are bonded together
- decreases going to the right and up

ionic radius: the radius of a monoatomic ion in an ion crystal structure
- decreases going to the right and up

57
Q

octet rule

A

many chemical compounds tend to form bonds so that each atom shares or has eight electrons in its highest occupied energy level

58
Q

Lewis structures vs resonance structures

A

Lewis structures: dot notations and lone pairs surrounding the letter of an element
**between covalent bonds

resonance structures: bonding in molecules or ions that cannot be correctly represent by a single Lewis structure
(portrays both of the Lewis structures that a compound can have)

59
Q

ionic compound

A

a three-dimensional network of positive and negative ions mutually attracted to one another
-harder and more brittle and have higher boiling points than materials containing only covalently bonded atoms

60
Q

electron sea

A
  • formed in metallic bonding
  • delocalized electrons that don’t belong to any one atom, move freely about a metal’s network of empty atomic orbitals. these electrons form a sea of electrons around metal atoms
  • gives metals their properties of high electrical and thermal conductivity, malleability, ductility, and luster
61
Q

VESPR theory

A

used to predict the shapes of molecules based on the fact that electron pairs strongly repel each other

62
Q

hybridization theory

A

used to predict the shapes of molecules, based on the fact that orbitals within an atom can mix to form orbitals of equal energy

63
Q

three types of intermolecular forces

A

dipole-dipole: interactions between POLAR molecules; molecules attract each other from opposite sides acting at short range

London dispersion: the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
- these forces are on every type of element/compound

hydrogen bonding: intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule

  • bonds ONLY between H-F, H-O, and H-N
  • i.e. water
64
Q

polar vs nonpolar molecules

A

polar: molecules with uneven Lewis structures and uneven dipoles
nonpolar: molecules with an even Lewis structure and dipoles that balance each other out

65
Q

positive vs negative monatomic ions

A

positive: identified by the name of the appropriate element
negative: named by dropping parts of the ending of the element’s name and adding -ide to the root

66
Q

binary compounds

A
  • composed of two elements

- binary ionic compounds are named by combining the names of the positive and negative ions

67
Q

formula mass, molar mass, and percentage composition

A

formula mass: sum of average atomic masses of all atoms present in the formula

molar mass: used as a conversion factor between amount in moles and mass in grams of a given compound or element

percentage composition: the percentage by mass of each element in the compound

68
Q

empirical formula vs molecular formula

A

empirical: shows the SMALLEST whole-number ratio of atoms in a given compound
- indicates how many atoms of each element are combined in the simplest unit of a chemical compound

molecular: the actual formula of a molecular compound
- can be found from the empirical formula if the molar mass is measured

69
Q

what are observations that suggest a chemical reaction is taking place?

A
  • evolution of energy as heat and light
  • production of gas
  • change in color
  • formation of a precipitate
70
Q

balanced chemical equation

A

represents, with symbols and formulas, the identities and relative amounts of reactants and products in a chemical reaction

71
Q

what are the four types of reactions?

A

synthesis: A + X –> AX
decomposition: AX –> A + X

single-displacement: A + BX –> AX + B

double displacement: AX + BY –> AY + BX

combustion: a substance combines with oxygen, releasing energy in the form of light and heat
- a hydrocarbon and oxygen yielding CO2 and H2O

72
Q

activity series

A
  • a list of the elements in order of their chemical reactivity
  • useful in predicting whether a chemical reaction will occur
  • determined through experiments
73
Q

reaction vs composition stoichiometry

A

stoichiometry: element measurement

composition stoichiometry: deals with the mass relationships of elements in a compound

reaction stoichiometry: involves the mass relationship between reactants and products in a chemical reaction

74
Q

mole ratio

A

the conversion factor that relates the amount in moles of any two substances in a chemical reaction

  • derived from a balanced equation
75
Q

how are the amounts vs the masses of a substance expressed?

A

amount of a substance: expressed in moles

mass of a substance: expressed by using mass units such as grams, kilograms, or milligrams

76
Q

what is necessary to solve any stoichiometric problem?

A
  • A BALANCED CHEMICAL EQUATION!!

- the mass or amount of the reactants and products

77
Q

limiting vs excess reactant

A

limiting: reactant that limits the amount of the other reactant that can combine and the amount of product that can form in a chemical reaction
- controls the maximum possible amount of product formed

excess reactant: substance that is not used up completely in a reaction

78
Q

theoretical, actual, and percentage yields

A

theoretical yield: the maximum amount of product that can be produced from a given amount of reactant

actual yield: the measured amount of that product obtained from a reaction

percentage yield: the ratio of the actual yield to the theoretical yield, multiplied by 100
- actual yield/theoretical yield x 100

79
Q

kinetic-molecular theory

A
  • explains properties of gases, liquids, and solids
80
Q

properties of gases, liquids, and solids relating to the kinetic-molecular theory

A

gases

  • consisting of many tiny, fast-moving particles that are far apart relative to their size
  • fluid
  • high level of expansion
  • low density,
  • compressible
  • diffuse and effuse

liquids

  • particles are closer together and more ordered than those of a gas and are less ordered than those of a solid
  • fairly high density
  • relatively incompressible
  • fluids: can flow
  • can diffuse (although slower than gases)

solids

  • definite volume and definite shape
  • may be crystalline or amorphous
  • nonfluid
  • definite melting point
  • very dense
  • incompressible
  • low rate of diffusion
81
Q

ideal vs real gas

A

ideal gas: a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory

real gas: a gas that does not behave completely according to the assumptions of the kinetic-molecular theory

82
Q

crystalline vs amorphous solids

A

crystalline solids: consisting of crystals
- exist as either a single crystal or a group of crystals

amorphous solids: atoms/particles are arranged randomly

83
Q

crystals & crystal structures

A

crystal: a substance in which the particles are arranged in an orderly, geometric, repeating pattern

crystal structure: the total three-dimensional array of points that describes the arrangement of the particles of a crystal

84
Q

surface tension vs capillary action

A

surface tension: a force that tends to pull adjacent parts of a liquid’s surface together, thereby decreasing the surface area to the smallest possible size

capillary action: the attraction of the surface of a liquid to the surface of a solid
- happens when adhesion (water sticking to other things) is stronger than cohesion (water sticking to itself)

85
Q

liquid-vapor equilibrium

A

when the molecules of a liquid in a closed system condense at the same rate at which they evaporate

86
Q

dynamic equilibrium

A

when two opposing changes occur at equal rates in a closed system

87
Q

formula unit

A

the simplest ratio of the compound’s cations and anions

- ionic compounds

chemistry (9 decks)

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