Ch. 1-2 Essential Ideas and Atoms, Molecules, and Ions

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123 Terms

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chemistry

the study of matter, its properties, the changes that matter undergoes, and the energy associated with these changes

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matter

anything with both mass and volume

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composition

the types and amounts of simpler substances that make up matter

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physical property

properties a substance shows itself without interacting with another substance

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color

physical property

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melting and boiling point

physical property

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density

physical property

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chemical property

properties a substance shows as it interacts with other substances

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flammability

chemical property

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corrosiveness

chemical property

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physical change

produces a recognizable difference in the appearance without changing the composition (state change)

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chemical change

transformation of a substance by rearranging, removing, replacing, or adding atoms

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solid

state of matter with a fixed shape and volume, may be hard or soft, rigid or flexible

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liquid

state of matter with varying shape but a fixed volume, shapes conforms to the shape of the container it is in

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a liquid has an _________

upper surface

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gas

state of matter with no fixed shape or volume and no surface

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plasma

gaseous state of matter with an appreciable amount of electrically charge particles

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where is plasma found?

certain high temperature environments (stars and lightning)

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solid state to liquid state

melting

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solid state to gaseous state

deposition

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liquid state to solid state

freezing

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liquid state to gaseous state

evaporation

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gaseous state to liquid state

condensation

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gaseous state to solid state

sublimation

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true or false: physical changes are reversible

true

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energy

the ability to do work

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potential energy

energy due to object’s position

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kinetic energy

energy due to object’s movement

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______ energy states are more stable than _______ energy states

lower; higher

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specific heat

the amount of heat needed to raise temperature of 1g of substance 1 degree C

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true or false: nonmetals generally have low specific heats

false: they usually have high specific heats

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true or false: metals generally have low specific heats

true

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if you sleep outside in the winter, would sleeping in a tent or a car be safer?

the tent because nonmetals have higher specific heats

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gravitational system

the potential energy gained when a lifted weight is converted to kinetic energy as the weight falls

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conversion factor

ratio of equivalent quantities used to express a quantity in different units

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If you need 325 cm of wire and the wire sells for $0.15/ft, how much will the wire cost?

$1.60

325 cm x 1in/2.54cm x 1ft/12in x $0.15/1ft = 1.60 dollars

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density

mass divided by volume

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Celsius degrees

scale based on the freezing and boiling points of water; most common around the world

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Kelvin

the “absolute temperature scale”, begins at absolute zero

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true or false: the Kelvin scale only has positive numbers

true

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Fahrenheit degrees

this scale has a different size and different zero points than other scales

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true or false: Celsius and Fahrenheit use the same size degree

false: Celsius and Kelvin share the same size degree

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Celsius temperature to Kelvin

C temp + 273.15

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Kelvin temperature to Celsius

K temp - 27.15

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Celsius temperature to Fahrenheit

9/5(C temp) + 32

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Fahrenheit temperature to Celsius

5/9(F temp - 32)

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A child has a body temperature of 38.7 degrees Celsius. If the normal body temperature is 98.6 degrees Fahrenheit, do they have a fever? What is their temperature in Kelvin?

yes and 311.8 K

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true or false: the rightmost digit of a measurement is always certain

false: it is always estimated

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zeros to the ______ of digits are not significant

left

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_______ zeros in ________ are significant

trailing; decimal places

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true or false: all nonzero digits are significant

true

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the significant figures for a multiplication/division answer should have the _____________ as the measurement with the fewest sig. figs.

same number of significant figures

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the answer to an addition/subtraction problem should have the ____________ as the measurement with the fewest decimal places

same number of decimal places

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exact numbers have _______________ associated with them

no uncertainty

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precision

how close measurements in a series are to each other

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accuracy

how close each measurement is to the actual value

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systematic error

produces values that are either all higher or all lower than the actual value

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random error

produces values that are both higher and lower than the actual value

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true or false: some results can be precise while also being inaccurate

true

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_______ connect the dots on a graph

NEVER

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R² value

indicates how close measurements are to a straight line

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standard deviaiton

measure used to quantify the amount of variation in a set of data

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small standard deviation has _____ precision and is ______ to mean value

high; close

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large standard deviation has _____ precision and _______ variation

low; random

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atom

basic structural unit of an element that retains its chemical properties

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a neutral atom has the same number of what?

protons and electrons

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atomic mass

sum of number of protons and neutrons

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true or false: the atomic number of an atom is equal to its number of electrons

false: equal to number of protons

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If Boron’s (B) atomic mass is equal to 11 and its atomic number is 5, calculate its numbers of protons, electrons, and neutrons.

protons = 5

electrons = 5

neutrons = 6

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isotopes

atoms of the same element having different masses (different numbers of neutrons)

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excited electron state

promotion of electrons occurs as it absorbs energy

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electrons absorb energy when they move to _______ energy levels

higher

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relaxation state

electrons release energy as they travel to lower energy states

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ground state

the lowest possible energy level

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Bohr failed to explain what?

line spectra of atoms with more than one electron

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what is a major change from Bohr’s Theory to the Modern Atomic Theory?

electrons do NOT move in orbits

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atomic orbitals

regions in space with a high probability of electrons

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Dmitri Mendeleev and Lothar Meyer did what?

independently

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periodic law

the physical and chemical properties of the elements are periodic functions of their atomic number

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period

horizontal row of elements on periodic table

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group

(aka “families”) column of elements on periodic table

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metals

substances whose atoms tend to lose electrons (positive charge) and mainly found in the left 2/3 of periodic table

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high thermal/electrical conductivity

metallic property

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high malleability/ductility

metallic property

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solid at room temperature

metals

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nonmetals

substances whose atoms tend to gain electrons (negative charge) and mainly found on the right 1/3 of the periodic table

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brittle and powdery solids/gases

nonmetals

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true or false: nonmetals’ properties are the opposite of metallic properties

true

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electron configuration

describes the arrangement of electrons in atoms

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principle energy levels

regions where electrons may be found (values like n=1,2,3. . . )

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sublevel

set of energy-equal orbits within a principle energy level

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true or false: s orbitals are spherically symmetrical in shape

true

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true or false: p orbitals are shaped like dumbbells

true

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how many electrons can a s orbital hold?

2

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how many electrons can a p orbital hold?

6

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how many electrons can a d orbital hold?

10

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Aufbau Principle

electrons will fill the lowest available orbitals first

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Pauli Exclusion Principle

each orbital can hold up to two electrons with their spins in the opposite directions

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Hund’s Rule

each orbital in a subshell is half-filled before any becomes paired

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valence electrons

outermost electrons in an atoms