Final Exam (all flashcards in folder)

charles’ law equation

initial volume/initial temperature (K) \= final volume/final temperature (K)

charles’ law

according to this law, the volume of a gas increases with increasing temperature as long as the pressure on the gas remains constant

boyle’s law equation

initial pressure x initial volume \= final pressure x final volume

boyle’s law

this law states that if you decrease the volume of a container of gas and hold the temperature constant, the pressure from the gas will increase.

inverse; as temperature increases, viscosity decreases and vice-versa

viscosity and temperature have what kind of relationship?

viscosity

the resistance of a fluid to flowing

bernoulli’s principle

the principle explaining that fluid velocity increases when the flow of the fluid is restricted; states that as the velocity of a fluid increases, the pressure exerted by that fluid decreases

pascal’s principle equation

input force/output force (N) \= output force/input force (N)

pressure equation

pressure (Pa) \= force(N)/area(m^2)

pascal’s principle

the principle stating that pressure applied to a fluid is transmitted throughout the fluid

an object will float when its density is less than that of the fluid

in terms of density, when will an object float? (compare density of object and density of fluid)

the wooden block only sank until the weight of the water displaced was equal to the weight of itself

a dense wooden block is placed within a pool of water. the block then sinks beneath the surface of the water, but does not reach the bottom. how is this a demonstration of archimede's principle?

the object placed within the fluid will displace the fluid until the weight of the displaced fluid is equal to the weight of the object

apply archimedes' principle. how are the weights of the fluid and of the object placed within the fluid related?

archimedes’ principle

the principle that the buoyant force on an object is equal to the weight of the fluid displaced by the object is known as:

buoyancy

the ability of a fluid (liquid or gas) to exert an upward force on an object immersed in it; the ability of an object to float as a result of the exertion of upward forces

liquid crystals are materials that do not lose their geometric arrangement (that is present within most solids) when turning into a liquid. they are used to create liquid crystal displays (LCDs) for electronic devices. pixels are individual picture crystal elements.

what are liquid crystals? how are they used?

glass and butter

name two amorphous solids

At a certain range of temperatures, specifically that between 0 and 4 degrees Celsius, water molecules expand as their temperature decreases. This is because of water's crystal lattice structure, which forms as a result of water's highly positive and negative areas.

how and why is water an exception to thermal expansion (at a certain range of temperatures?)

thermal expansion

an increase in the size of a substance when the temperature is increased

their collisions are so forceful that electrons are stripped off of the atoms, thus breaking the attraction between atoms

explain the definition of plasma: why are they able to overcome attractions between atoms?

plasma

matter that has enough energy to overcome not just the attractive forces between its particles but also the attractive forces within its atoms; most common state of matter in the universe

speed increases with temperature, and thus the addition of thermal energy causes particles to increase in speed and eventually overcome inter-particle attractions

how do substance overcome attractions between particles, in terms of the addition of thermal energy?

heating curve

a graph that shows how temperature changes over time as thermal energy is continuously added; visually demonstrates phase changes (or when attractive forces are overcome)

sublimation

the process that causes a substance to change directly from a solid into a gas; only occurs at certain pressures

heat of vaporization

the amount of energy required for a liquid at its boiling point to become a gas; amount of energy required for a liquid to overcome attractions between particles and become a gas

boiling point

temperature at which the pressure of vapor within the liquid is equal to external pressure acting on the liquid's surface; point at which a liquid vaporizes into a gas

heat of fusion

energy required to overcome attractions between particles in the solid state, allowing for said solid to melt into a liquid

melting point

energy required to overcome attractions between particles in the solid state, allowing for said solid to melt into a liquid

1. all matter is composed of tiny particles (atoms, molecules, and ions) 2. these particles travel in constant, random movements 3. these particles collide with each other and the walls of the container in which they are held 4. the amount of energy that the particles lose from these collisions is so little that it does not matter

the assumptions of kinetic theory

temperature

the avg kinetic energy of a substance

thermal energy

the total energy of the particles that make up a material, including kinetic and potential energy

how the particles that compose gases behave

the kinetic theory is an explanation of…

solid, liquid, gas, plasma

four states of matter

element

a substance with the same kind of atoms

compound

a substance that has two or more elements combined in a fixed proportion

distillation

the process of separating substances, such as salt and water, in a mixture by evaporating a liquid and reconvening its vapor

color, state of matter, size, and shape

identify four physical properties that describe a liquid

law of conservation of mass

the law stating that the mass of all substances present before a chemical change, known as the reactants, equals the mass of all of the substances that remain after the change, which are called the products

physical (water seeps into cracks between rocks, slowly splitting them apart) chemical (limestone reacts chemically with slightly acidic water, causing new substance to form)

name the two types of weathering and give examples for each

chemical change

a change of one substance to another

chemical property

any characteristic of a material that you can observe that produces one or more new substances

physical change

a change in size, shape, or state of matter in which the identity of the substance remains the same

physical property

any characteristic of a material that you can observe without changing the identity of the substance

mixtures \= pure substance that under physical change; do not always contain same proportions of components pure substance \= can change between chemical forms (always contains same proportions of components)

c/c mixtures and substances

false

t/f: solutions and homogeneous mixtures are not the same thing

homogeneous mixture

a mixture that remains constantly and uniformly mixed and has particles that are so small that they cannot be seen with a microscope

pass a beam of light through it; light cannot pass through mixtures, but can pass through colloids

explain how you can utilize the tyndall effect to identify a colloid from a solution

tyndall effect

the scattering of a light beam as it passes through a colloid

colloid

a heterogeneous mixture with solid particles that never settle within the liquid

suspension

a heterogeneous mixture composed of a liquid and solid particles that settle within the liquid

heterogeneous and homogeneous

what are the two types of mixtures?

if an atom's outer layer is full, reactions will occur less often/not at all between that atom and other atoms.

how do the number of valence electrons determine the reactability of an element?

electron dot diagram

a diagram that uses the chemical symbol of an element surrounded by dots to represent the number of electrons in the outermost energy level

valence electrons

what kind of electrons determine the chemical properties of each individual element?

valence electrons

electrons in the outermost energy level of an atom

groups (or families)

the vertical columns in the periodic table are called

periods

the horizontal rows of elements in the periodic table

similar

elements in the same group on the periodic table have (similar/different) chemical properties

periodic table

a table that arranges elements by increasing atomic number, not atomic mass, and by periodic changes in physical and chemical properties.

most chlorine atoms contain 18 neutrons. there are 17 protons in chlorine, and because the average atomic mass is closer to 35, more chlorine atoms have a mass number of 35.

chlorine has an average atomic mass of 35.45 amu. the two naturally occurring isotopes of chlorine are chlorine-35 and chlorine-37. do most chlorine atoms contain 18 neutrons or 20 neutrons? why?

isotopes of an element are alike in the ways that they have the same number of protons, but different numbers of neutrons, causing different mass numbers between them (meaning isotopes)

explain how the isotopes of an element are alike and how they are different.

10.8 amu

calculate the average atomic mass in amu of boron-10 and boron-11: 4/5(11 amu) + 1/5(10 amu) \= ?

average atomic mass

the weighted average mass of all naturally occurring isotopes of an element, measured in atomic mass units (amu), according to their natural abundances

isotopes

atoms of the same element that have different numbers of neutrons

mass number

the sum of the number of protons and the number of neutrons in the nucleus of an atom

atomic number

the number of protons in an atom’s nucleus

1,800

protons and neutrons are over \___ times more massive than electrons

1.67 * 10^-24

the approximate size of protons and neutrons

electrons move so quickly and randomly that it is impossible to exactly pinpoint its exact location at any given moment

why is the electron cloud the most accurate to date

1. matter is composed of atoms 2. atoms are indivisible and indestructible (disproven) 3. atoms of a given element are identical in size, mass, and chemical properties 4. atoms of a specific element are different from those of another element 5. different atoms combine in simple whole-number ratios to form compounds 6. in a chemical reaction, atoms are separated, combined, or rearranged.

state the terms of dalton's atomic theory

400 B.C. \-- Democritus Model 1904 \-- Thomson Model 1911 \-- Rutherford Model 1913 \-- Bohr Model 1926 \-- Electron Cloud Model

name the five atomic models and their approximate dates

scientists accelerate charged particles and cause them to collide with protons, causing them to break apart. (this is done in particle accelerators)

how are quarks discovered

quarks

the even smaller particles that scientists suspect protons and neutrons to be composed of

electrons

particles with an electric charge of 1-

neutrons

electrically neutral particles in the nucleus; they hvae no charge

protons

particles in the nucleus with an electric charge of 1+

nucleus

the small, positively charged center of the atom

atom

the smallest particle of an element that retains the element’s properties

groups 14 and 15 contain nonmetals, metalloids, and metals, whereas groups 13 and 16 only contain two of the aforementioned

explain why groups 14 and 15 are better representations of mixed groups than groups 13 and 16

group 14: the carbon group

carbon, silicon, germanium, tin, and lead all make up what group on the periodic table?

transuranium elements

elements that have more than 92 protons, the atomic number of uranium

group 16: the oxygen group

oxygen, sulfur, selenium, tellurium, and polonium all make up what group?

the nitrogen group

nitrogen, phosphorus, arsenic, antimony, and bismuth all make up what group?

semiconductors

elements that conduct an electric current under certain conditions

allotropes

different molecular structures of the same element

metalloids

elements that have some properties of metals and some properties of nonmetals

solid nonmetals are brittle and powdery, whereas solid metals are malleable, shiny, and ductile.

explain how solid nonmetals are different from solid metals

isolated atoms

the noble gases exist as what kind of atoms?

halogens

Fluorine, chlorine, bromine, iodine, and astatine are called:

diatomic molecule

a molecule consisting of two atoms of the same element in a covalent bond

not malleable or ductile; brittle or powdery

list the properties of nonmetals

nonmetals

elements that are usually gases or solids

because metals are malleable and ductile, they can be identified through means of hammering the element into sheets or drawing it into wires

describe how to test a sample of an element to see if it is a metal

inner transition metals

the lanthanides and actinides make up which part of the periodic table?

copper, silver, and gold

the coinage metals are composed of:

iron, cobalt, and nickel

the iron triad is composed of:

transition elements; transition

elements in groups 3 through 12 in the periodic table; considered to be a \_______ between the main group elements

group 2: the alkaline earth metals

beryllium, magnesium, calcium, strontium, barium, and radium are all a part of what group on the periodic table?

radioactive element

an element in which the nucleus breaks down and gives off particles and energy

alkali metals

lithium, sodium, potassium, rubidium, cesium, and francium are all: