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AP Chemistry Unit 1 Study Guide

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Section 1

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paramagnetic vs diamagnetic

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Chemistry Science

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Mar 14, 2020

Cards (75)

Section 1

(50 cards)

paramagnetic vs diamagnetic

Front

Diamagnetic atoms have only paired electrons, whereas paramagnetic atoms, which can be made magnetic, have at least one unpaired electron.

Back

arrangement of periodic table

Front

periods, groups/families, metals/nonmetals/metalloids, atomic mass, atomic number

Back

Dimitri Mendeleev

Front

predicted the existence and properties of new chemical elements

Back

quantum

Front

smallest amount of energy that can be lost or gained by an atom

Back

molar mass

Front

the sum of the total mass in grams of all the atoms that make up a molecule per mole unit: grams/mol

Back

sheilding

Front

describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell

Back

quantitative

Front

data that can be expressed as a number (age, weight)

Back

Ernest Rutherford

Front

gold foil experiment- shot alpha particles and proposed nuclear theory: 1) most of atoms mass and all of its positive charge contained in nucleus 2) most of volume is empty space 3) there are negatively charged electrons outside nucleus and neutral charged protons inside, making the overall atom neutrally charged

Back

kinetic molecular theory (KMT)

Front

PV = nRT (ideal gas law) P = pressure (atm) V = volume (L) n = number of moles R = 0.0821 atmL / molK T = temperature (K) Pressure = force / area Why does gas exert pressure? gas particles in constant, rapid, random motion particles collide w/ surface of container & w/ each other Gases have kinetic energy because always in motion KE = ½ mv^2 (v = velocity) Temperature- average kinetic energy of particles in sample temp & kinetic energy directly proportional

Back

metric conversions

Front

Back

plum pudding model

Front

JJ Thompson

Back

quantum numbers

Front

branch of physics relating to the very small particles

Back

pauli exclusion principle

Front

no 2 electrons in the same atom will have same set of quantum numbers

Back

Werner Heisenberg

Front

uncertainty principle- can not know simultaneously exact location and velocity of an electron

Back

frequency

Front

waves/sec., hertz (hz)

Back

hund's rule

Front

an electron must fill each orbital of equal energy before 2 electrons fill any orbital

Back

probability density

Front

the probability (per unit volume) of finding the electron at a point in space as expressed by the three dimensional plot of the wave function squared

Back

empirical formula vs. molecular formula

Front

empirical is simplest or most reduced ratio of elements in a compound while molecular is how many atoms of each element are in a compound (C6H12O6 is molecular and CH2O is empirical)

Back

aufbau principle

Front

an electron must fill the lowest energy orbital that can receive it

Back

combustion reaction

Front

CxHy + O2 ---> CO2 + H2O

Back

rounding

Front

0.0000987 rounds to 0.00001 or 10.560 rounds to 10.6

Back

electromagnetic spectrum

Front

Back

qualitative

Front

information that is not numerical (feelings, how it looks)

Back

periodic law

Front

the law that the properties of the elements are periodic functions of their atomic numbers. Also called Mendeleev's law.

Back

Max Planck

Front

discovered that energy, which appears to be emitted in wavelengths, is actually discharged in small packets (quanta), Planck's constant is 6.626 × 10^-34 J (s)

Back

balancing equations

Front

unbalanced: H2 + O2 ---> H2O balanced: 2H2 + O2 ---> 2H2O

Back

photoelectron effect

Front

the observation that many metals emit electrons when light falls upon them

Back

orbitals - s,p,d,f

Front

Back

temperature conversions

Front

°F=1.8°C+32 °C=(°F-32)/1.8 K=°C+273

Back

photon (quantum)

Front

particle of EM radiation having 0 mass and carries a quantum of energy

Back

quantum mechanical

Front

Back

significant figures

Front

in any reported measurement, the non-place-holding digits that indicate the precision of the measured quantity (4 sigfigs = 0.01000 or 3 sigfigs = 100.)

Back

accuracy vs precision

Front

accuracy- how close a measured value is to the actual value precision- how close a series of of measurements are to one another or how reproducible they are

Back

constructive vs destructive interference

Front

-Constructive interference is a type of interference that occurs at any location along the medium where the two interfering waves have a displacement in the same direction -Destructive interference is a type of interference that occurs at any location along the medium where the two interfering waves have a displacement in the opposite direction

Back

Louis de Broglie

Front

discovery of wave nature of electrons

Back

percent compostition

Front

mass of element/total mass of compound X 100

Back

scientific notation

Front

18,750,000 = 1.875 X 10^7 or 0.000018750 = 1.875 X10^-6

Back

diffraction

Front

the phenomena by which a wave emerging from an aperture spreads out to form a new wave front

Back

dimensional analysis

Front

is a problem-solving method that uses the fact that any number or expression can be multiplied by one without changing its value

Back

wavelength

Front

meters, "lambda" λ

Back

electron configurations, orbital notation, noble gas notation

Front

orbital notation- arrows noble gas notation- for chlorine: [Ne]-3s2-3p5

Back

effective nuclear charge (Z eff)

Front

net positive charge experienced by valence electrons

Back

Antoine Lavoisier

Front

law of conservation of mass: matter is neither created nor destroyed

Back

Albert Einstein

Front

attempted to disprove quantum mechanics, and failed until he died

Back

Henry Mosely

Front

created periodic table that organized by increasing atomic number, elements classified by proton, and with similar properties

Back

JJ Thompson

Front

cathode ray experiment- applied magnetic fields across tube, produced negative charge, discovered electron, Plum Pudding model

Back

John Dalton

Front

experimented with mixtures of gases to determine effect of properties of mixtures as a whole concluded: 1) all matter made of atoms 2) atoms of a given element have identical properties (FALSE: isotopes) 3) atoms of different elements combine in ratios to form chemical compounds 4) atoms can not be subdivided, created, or destroyed (FALSE) 5) atoms can be combined, separated, or rearranged

Back

Erwin Schrodinger

Front

combined the equations for the behavior of waves with the de Broglie equation to generate a mathematical model for the distribution of electrons in an atom, Schrodinger's cat- claims that if you don't know what the state of any object is, then - as long as you don't look to check - it is actually in all possible states simultaneously

Back

Niels Bohr

Front

tried to prove hydrogen levels, concluded electrons only occupy certain energy levels

Back

coulombs' law

Front

As distance increases, the forces and electric fields decrease

Back

Section 2

(25 cards)

metallic character

Front

level of reactivity of a metal

Back

particle view - states of matter

Front

1) Solid- definite shape, definite volume molecules tightly packed 2) Liquid- no definite shape molecules slide past one another 3) Gas- no definite shape, no definite volume molecules move very rapidly 4) Plasma- very high temps, atoms lose their electrons example: fluorescent bulbs, stars

Back

ionization energy

Front

the amount of energy required to remove an electron from an atom to form a cation

Back

chromatography

Front

the separation of a mixture by passing it in solution or suspension or as a vapor (as in gas chromatography) through a medium in which the components move at different rates

Back

distillation

Front

A process in which the mixture is heated to boil off the more volatile (easily vaporizable) liquid.

Back

photoelectron spectroscopy

Front

utilizes photo-ionization and analysis of the kinetic energy distribution of the emitted photoelectrons to study the composition and electronic state of the surface region of a sample -It refers to energy measurement of electrons emitted from solids, gases or liquids by the photoelectric effect, in order to determine the binding energies of electrons in a substance (Coulomb's Law) -Measures electrons emitted from solids, gases, or liquids by photoelectron effect in order to determine binding energies of electrons.

Back

elements vs compounds pure substance vs mixture

Front

1) Pure substance- made up of only one component and its composition is invariant (does not vary from one sample to another) components can be individual atoms or groups of atoms joined together broken down to either element or compound 2) element- a substance that cannot be chemically broken down into simpler substances example: helium compound- substance composed of 2 or more elements in a fixed proportion example: water 3) Mixture- composed of two or more components in proportions that can vary from one sample to another broken down to either heterogeneous and homogeneous heterogenous- the composition varies from one region of the mixture to another example: wet sand homogenous- composition throughout example: kool-aid

Back

atomic radius

Front

Back

spectrophotometry

Front

(Beers Law) Method used to measure how much a chemical substance absorbs light by measuring the intensity of light as a beam of light passes through sample solution -The basic principle is that each compound absorbs or transmits light over a certain range of wavelength Measures amount of light of a specified wavelength which passes through a medium

Back

law of definite proportions

Front

Joseph Proust all samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements -ratio of masses is also same -hints that matter is composed of atoms

Back

physical properties and changes

Front

1) property- a characteristic that can be observed or measured w/out changing the identity of the substance color, state, melting point, boiling point, density 2) change- change in a substance that doesn't involve a change in the identity of the substance change in shape or size (tearing a piece of paper, hammering a sheet of metal)

Back

ionic radius

Front

Back

flame tests

Front

An analytic procedure used in chemistry to detect the presence of certain elements, primarily metal ions, based on each element's characteristic emission spectrum Lithium-red Sodium-strong orange Potassium- pink (lilac) Strontium- red Barium- Pale green Copper- blue-green

Back

filtration

Front

The mixture is poured through filter paper in a funnel.

Back

decanting

Front

Carefully pouring off one substance into a different container

Back

chemical properties and changes

Front

1) property- substance's ability to undergo changes that transform it into a different substance charcoal = combustible 2) change- when substance is converted into a new substance example: nuclear bomb, baking bubbling (gas formed) vapor (smoke) color change odor precipitation (solid formed) change temp (hotter or colder) light production

Back

density

Front

D = m/v 1) intensive property (density)- one that is independent of the amount of substance often used to identify substances bc these properties depend only on the type of substance and not on the amount of it 2) extensive property (mass)- one that depends on the amount of the substance if you know only the mass of a sample, that info alone will not allow you to identify it as gold units- kg/m^3 Liquids and solids = g/cm^3 or g/mL Aluminum = least dense metals, platinum = most dense

Back

emission spectroscopy

Front

Method of chemical analysis that uses the intensity of light emitted from a flame, plasma, arc or spark at a particular wavelength to determine the quantity of an element in a sample -The wavelength of the atomic spectral line gives the identity of the element while the intensity of the emitted light is proportional to the number of atoms of the element

Back

law of multiple proportions

Front

John Dalton When 2 elements (call them A & B) form 2 different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers

Back

electron affinity

Front

a neutral atom's likelihood of gaining an electron

Back

mass spectrometry

Front

Technique that helps identify the amount and type of chemicals present in a sample by measuring the mass-to-charge ratio and abundance of gas-phase ions. A mass spectrum (plural spectra) is a plot of the ion signal as a function of the mass-to-charge ratio -Measures the masses of atoms and the percent abundances of isotopes of elements and separates particles according to their mass

Back

isotopes

Front

same number protons, diff number neutrons 3 isotopes of hydrogen protium- 1 proton, 0 neutrons deutrium- 1 proton, 1 neutron tritum- 1 proton, 2 neutrons (most abundant)

Back

electronegativity

Front

measure of the tendency of an atom to attract a bonding pair of electrons

Back

evaporation

Front

the process by which a substance is turned from a liquid to a gas

Back

law of conservation of mass

Front

created by Lavoisier and says in a chemical reaction, matter is neither created nor destroyed

Back