Study Chemistry Semester 1 Exam Review Flash Cards

 
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Chemistry Semester 1 Exam Review

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label the periodic table from left to right
non-metals, alkali metals, alkali-earth metals, transition metals, other metals, non-metals, halogens, inert elements, [in between] rare earth metals
what happens when you move down a group on the periodic table?
The atomic radius increases because protons are added, but so are new energy shells of electrons. The new energy shells provide shielding, allowing the valence electrons to experience only a minimal amount of the protons' positive charge
what happens when you move from left to right on the period of the periodic table?
the atomic radius decreases becauuse he nucleus of the atom gains protons, increasing the positive charge of the nucleus and increasing the attractive force of the nucleus upon the electrons
indicates the relative ability of an element's atoms to attract electrons in a chemical bond
electronegativity
the energy required to remove an electron from an atom or ion (endothermic - not favorable)
ionization energy
a comparison of one atom's "fuzzy edge" to another (electron cloud edge is indistinct)
atomic radius
periodic table - horizontal
row/period/series
periodic table - vertical
group/family
electrons in the outermost energy level
valence electrons
any configuration of the system that has a higher energy than the ground state (that is, more energy than the absolute minimum)
excited state
electromagnetic spectrum - put in order from least energy/frequency to most:
gamma rays, infrared, x rays, radio, microwaves, ultraviolet
radio, microwaves, infrared, ultraviolet, x rays, gamma rays
what is the main difference between the way the Bohr model and the quantum mechanical model of the atom describe electrons?
QM: electrons are thought of as waves with no distinct orbits
BM: electrons are thought of as matter (particles) with distinct orbits
(true or false) according to Bohr's atomic model, when energy is added to a hydrogen atom, its electron moves to a higher-energy orbit
true
this predicted the frequencies of the lines in hydrogen's atomic emission spectrum
Bohr's model (planetary model)
the lowest allowable energy state of an atom
ground state
(true or false) when an atom emits light, photons having certain specific energies are being emitted
true
(true or false) the neon atoms in a neon sign emit their characteristic color of light as they absorb energy
false
(true or false) atomic emission spectra can be explained by the wave model of light
false
(true or false) the fact that only certain colors appear in an element's atomic emission spectrum indicates that only certain frequencies of light are emitted
true
(true or false) a flame test can be used to identify the presence of certain elements in a compound
true
a chemistry procedure used to test for the presence of metal ions. The emission spectrum of each element produces a characteristic color
flame test
(true or false) each element has a unique atomic emission spectrum
true
(true or false) like the visible spectrum, an atomic emission spectrum is a continuous range of colors
false
minimum amount of energy that can be lost or gained by an atom
quantum
SI unit for frequency
hertz
number of waves that pass a given point in one second
frequency
height of a wave from the origin to a crest or from the origin to a trough
amplitude
the shortest distance between equivalent points on a continuous wave
wavelength
wave speed formula
speed of wave = wavelength x frequency
the magnetic behavior of an electron immersed in an external magnetic field
electron magnetic resonance (EMR)
A-X-Z notation
A = mass number
X = chemical symbol for element (if it is an ion, then charge goes next to it)
Z = atomic number
the weighted average mass of the isotopes of that element
atomic mass
the number after an element's name, representing the sum of its protons and neutrons
mass number
the number of protons in an atom
atomic number
atoms of the same element with different numbers of neutrons
isotope
gain or loss of electrons from the outer valence level of an atom so that it acquires a negative or positive charge the value of which is determined by the number of electrons gained or lost
ion formation
Dalton's atomic theory
1) atoms are invisible and indestructible
2) atoms of a given element are identical in size, mass, and chemical properties
3) atoms of a specific element are different from those of another element
4) different atoms combine in simple whole-number ratios to form compounds
5) in a chemical reaction, atoms are separated, combined, or rearranged
states that matter is composed of extremely small particles called atoms..
Dalton's atomic theory
radiation that originates from the cathode and travels to the anode of a ______ tube
cathode ray
invented first Periodic able for classifying elements. found that the elements could be classified by their reoccurring chemical and physical properties. used his periodic table to predict the existence of undiscovered elements and to determine their properties. as result, many new elements were quickly found.
mendeleev
Heisenburg's model
Charge-cloud/Quantum Mechanical model
Bohr's model
Planetary model
Rutherford's model
Nuclear model
Thomson's model
Plum-Pudding model
Dalton's model
BB model
(1754-1826) proposed the the Law of Constant Composition in 1799 ( states that the composition of a substance is always the same, regardless of how the substance was made or where the substance is found)
Proust
proposed the Combustion Theory (burning: chemical addition of oxygen to the fuel) based on sound mass measurements; named oxygen; proposed the Law of Conversation of Mass which represents the beginning of modern chemistry
Lavoisier
studied atomic structure with application of X-ray spectra; discoveries resulted in a more accurate positioning of elements in the Periodic Table by closer determination of atomic numbers; with discovery of isotopes, became apparent that atomic weight was not significant in periodic law, but rather the properties of the elements varied with atomic number
Moseley
explained that atoms exist in "stationary" states, and that when changes from one state to another, there has been an emission (or absorption) of electromagnetic radiation of frequency ν , determined by the energy difference between the two states:
Δ E = E 2 − E 1 = hν
with this theory, combined the atomic model of Rutherford with existing quantum theory
Bohr
(1834-1907) found a connection between atomic mass and elemental properties, arranged the elements in order of increasing atomic mass, and predicted the existence and properties of unobserved elements
Dmitri Mendeleev
scientists have determined that protons and neutrons are composed of subatomic particles called ______
quarks
received the Nobel Prize in 1935 for discovering the existence of neutrons, neutral particles in the nucleus which accounts for the remainder of an atom's mass
James Chadwick
in 1911, studied how positively charged alpha particles interacted with solid matter by aiming the particles at a thin sheet of gold foil. Concluded that atoms are mostly empty space; proposed existence of third atomic particle: neutron
Rutherford
used the plum pudding model of the atom and stated that the atom is a uniform, positively charged sphere containing electrons
J.J. Thomson
with the electron's charge and charge-to-mass known, he calculated the mass of a single electron
Robert Millikan
In early 1910s, used the oil-drop apparatus to determine the charge of an electron
Robert Millikan
measured the effects of both magnetic and electric fields on the cathode ray to determine the charge-to-mass ratio of a charged particle, then compared it to known values
J.J. Thomson
when an electric charge is applied, a ray of radiation travels from the cathode to the anode, called ______, which is a stream of particles carrying a negative charge
cathode ray
an instrument that allows individual atoms to be seen
scanning tunneling microscope (STM)
revived the idea of the atom in the early 1800s based on numerous chemical reactions
John Dalton
disagreed with Democritus because he did not believe empty space could exist
Aristotle
first person to propose the idea that matter was not infinitely divisible, but made up of individual particles called atomos
Democritus
the capacity to do work or produce heat
energy
density equation
D = m/v (density equals mass divided by volume)
reaction in which the products have less energy than the reactants
exothermic reaction
reaction in which the products have more energy than the reactants
endothermic reaction
states that when different compounds are formed by the combination of the same elements, different masses of one element combine with the same mass of the other element in a ratio of small whole numbers
law of multiple proportions
states that, regardless of the amount, a compound is always composed of the same elements in the same proportion by mass
law of definite proportions
a chemical combination of two or more different elements; can be broken down into simpler substances by chemical means and has properties different from those of its component elements
compound
a pure substance that cannot be broken down into simpler substances by physical or chemical means
element
a technique that is used to separate the components of a mixture based on the tendency of each component to travel or be drawn across the surface of another material
chromatography
the energy-requiring process by which a solid changes directly to a gas without first becoming a liquid
sublimation
a separation technique that produces pure solid particles of a substance from a solution that contains the dissolved substance
crystallization
a technique that can be used to physically separate most homogeneous mixtures based on the differences in the boiling points of the substances
distillation
a technique that uses a porous barrier to separate a solid from a liquid
filtration
one that has a uniform composition throughout and always has a single phase; also called a solution
homogeneous mixture
one that does not have a uniform composition and in which the individual substances remain distinct
heterogeneous mixture
a physical blend of two or more pure substances in any proportion in which each substance retains its individual properties; can be separated by physical means
mixture
states that mass is neither created nor destroyed during a chemical reaction but is conserved
law of conservation of mass
a process involving one or more substances changing into new substances; also called a chemical reaction
chemical change
a transition of matter from one state to another
phase change
a type of change that alters the physical properties of a substance but does not change its composition
physical change
a physical property that remains the same no matter how much of a substance is present
intensive property
a physical property, such as mass, length, and volume, that is dependent upon the amount of substance present
extensive property
the number of all known digits reported in measurements plus one estimated digit
significant figures
5 rules for significant figures
1) nonzero numbers are always significant
2) zeroes between nonzero numbers are always significant
3) all final zeroes to the right of the decimal are significant
4) placeholder zeros are not significant. To remove placeholder zeros, rewrite the number in scientific notation
5) counting numbers and defined constants have an infinite number of significant figures
used to express any number as a number between 1 and 10 (coefficient) multiplied by ten raised to a power (exponent)
scientific notation
refers to how close a series of measurements are to one another
precision
how close the measurement is to a true or accepted value
accuracy
a relationship in nature that is supported by many experiments
scientific law
explanation of a natural phenomenon based on many observations and investigations over time
theory
a standard for comparison
control
in an experiment, the variable whose value depends on the independent variable
dependent variable
in an experiment, the variable that the experimenter plans to change
independent variable
a set of controlled observations that test the hypothesis
experiment
a tentative explanation for what has been observed
hypothesis
numerical information
quantitative data
information that describes color, odor, shape, or some other physical characteristics
qualitative data
systematic approach used in scientific study, whether it is chemistry, biology, physics, or another science
scientific method
measure not only of matter but also of the effect of earth's gravitational pull on that matter
weight
a measure that reflects the amount of matter
mass
the study of matter and the changes that it undergoes
chemistry
scientific method
observation (qualitative & quantitative), hypothesis, experiments, conclusion
a measurement that reflects the amount of matter (standard unit is the kilogram, kg)
mass
(difference between mass and weight): _____ contributed to by protons and neutrons
mass
(difference between mass and weight): _____ is the measure of not only the amount of matter but also the effect of the earth's gravitational pull on that matter
weight
base unit of luminous intensity
candela (cd)
base unit of electric current
ampere (A)
base unit of amount of a substance
mole (mol)
base unit of temperature
kelvin (K)
base unit of mass
kilogram (kg)
base unit of length
meter (m)
base unit of time
second (s)
relative error
(absolute/true) * 100
absolute error
observed - true
1 dm^3
= 1 L (= 1 kg of water)
1 cm^3
= 1 mL (= 1 g of water)
nano (n)
10^-9
micro (fancy M)
10^-6
mili (m)
10^-3
centi (c)
10^-2
deci (d)
10^-1
BASE (no prefix)
10^0
deka (da)
10^1
hecto (h)
10^2
kilo (k)
10^3
mega (M)
10^6
giga (G)
10^9
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