Question | Answer |
The scientific system of writing numbers | scientific notation |
Give the scientific Notation of
1,000,000,000 | 10^9 |
Give the scientific notation of'
1,000,000 | 10^6 |
Give the scientific notation of
1,000 | 10^3 |
Give the scientific notation of
100 | 10^2 |
Give the scientific notation of
1 | 10^0 |
Give the scientific notation of
0.01 | 10^-2 |
Give the scientific notation of
0.000001 | 10^-6 |
Give the scientific notation of
0.000000001 | 10^-9 |
method to measure weight, length, and volume | metric system |
simple, logical, and efficient measurement system | metric system |
basic units of measurements of the metric system | grams, liters, and meters |
Basic measurement of weight | grams (g) |
Basic measure of weight | liter (L) |
Basic measure of distance | meter (m) |
Tera-
abbreviation
means?
numerically | T-
10^12
1 quadrillion times |
Giga-
abbreviation?
means?
numerically? | G-
10^9
1 billion times |
Mega-
abbreviation?
means?
numerically | M-
10^6
1 million times |
kilo-
abbreviation?
means?
numerically? | k-
10^3
1 thousand times |
hecto-
abbreviation?
means?
nummerically? | h-
10^2
1 hundred times |
deka-
abbreviation?
means?
numerically? | D-
10^1 times |
deci-
abbreviation?
means?
numerically? | d-
10^-1
1 tenth of |
centi-
abbreviation?
means?
numerically? | c-
10^-2
1 hundredth of |
milli-
abbreviation?
means?
numerically? | m-
10^-3
1 thousandth of |
micro-
abbreviation?
means?
numerically? | u(backwards)
10^-6
1 millionth of |
nano-
abbreviation?
means?
numerically? | n-
10^-9
1 billionth of |
pico-
abbreviation?
means?
numerically? | p-
10^-12
1 trillionth of |
femto-
abbreviation?
means?
numerically? | f-
10^-15
1 quadrillionth of |
3 most common temperature systems | Fahrenheit, Celsius, nad Kelvin |
temperature measuring system used only in the United States, its territories,Belize, and Jamaica. | Fahrenheit |
Rarely used for any scientific measurements except body temperature. | Fahrenheit |
Zero degrees is the freezing point of sea water or heavy brine at sea level. | Fahrenheit |
32 degrees is the freezing point of pure water at sea level. | Fahrenheit |
212 degrees is the boiling point of pure water at sea level. | Fahrenheit |
Most people have a body temperature of 98.6 degrees | Fahrenheit |
temperature system used in the rest of the world and by the scientific community. | Celsius/Centigrade |
zero degrees is the freezing point of pure water at sea level. | Celsius |
100 degrees is the boiling point of pure water a sea level. | Celsius |
Most people have a body temperature of 37 degrees | Celsius |
Used only in the scientific community | Kelvin |
zero degrees is -273 degrees Celsius and is thought to be the lowest temperature achievable or absolute zero | Kelvin |
The freezing point of water is 273 | Kelvin |
The boiling point of water is 373 | Kelvin |
Basic building block of all molecules | Atom |
Atom's physical structure | Nucleus |
At the center of the atom and is composed of protons and neutrons | Nucleus |
When are atoms most stable? | When an orbital is full |
positive electrical charge | protons |
negative charge | electrons |
no charge | neutrons |
an atom that is electrically charged | ion |
an atom that has a positive charge | cation |
an atom that has a negative charge | anion |
defined by its properties | matter |
rows of the periodic table | periods |
columns of the periodic table | groups |
energy required to remove the outermost electron from the atom. | ionization energy |
ability to attract electrons | electronegativity |
what location is the alkali metals in the periodic table? What are the properties? | Group 1
metals with one outermost electron. form 1+ ions |
what location are the alkaline earth metals in the periodic table? what are the properties? | Group 2
metals with two outermost electrons. Form 2+ ions |
where are the transition metals located in the periodic table? | Groups 3-10
Metals that usually form colored ions and solutions. Have multiple oxidation states. |
Where are the Halogens located in the periodic table? | Group 17
Nonmetals with seven outermost electrons.
Form 1- ions |
Where are the noble gases located in the periodic table? | Group 18
Nonmetal gases that do not react because they have full outermost PELs |
Two important numbers or properties of atoms that can be obtained from the periodic table are? | atomic number & mass |
number of protons in the nucleus, and it defines an atom of a particular element. | atomic number |
what is the atomic mass of an atom? | average mass of each of that element's isotopes. |
different kinds of the same atom that vary in weight | Isotopes |
What is it called when a an element or atom exists in combination with other elements? | compound |
How is an equation written> | Reactants ----> Products |
In any chemical reaction, an arrow between the reactants and the products is drawn out. What does the arrow symbolize? | the direction of the reaction |
what does the law of conservation of mass state? | Mass cannot be created or destroyed during a chemical reaction. Therefore, once the reactants have been written and the products predicted, the equation must be balanced. |
A state in which reactants are forming products at the same rate that products are forming reactants. | Equilibrium |
Name 4 ways to increase the reaction rate | increase the temperature in the reaction, increase the surface area of the reactants, add a catalyst, or increase the concentrations of reactants. |
If you increase the temperature in the reaction what happens? | causes the particles to have a greater kinetic energy causing them to move faster. Contact is when the chemical reactions will occur. |
What happens when you increase the surface area of the particles in the reaction? | Gives the particles more opportunity to come into contact with one another. |
accelerates a reaction by reducing the activation energy or the amount of energy necessary for a reaction to occur. | catalyst |
what happens when you increase the concentration of the reactants? | It will cause more chance collisions between the reactants and produce more products. |
Homogeneous mixture of two or more substances | solution |
can be a liquid in a liquid, a solid in a liquid, or a solid in a solid. | solutions |
name the four types of solutions | compounds, alloys, amalgams, emulsions |
Mixtures of different elements to create a single matter | compound |
solid solutions of metals to make a new one such as bronze, which is copper and tin, or steel, which is iron and carbon, tungsten, chromium, and manganese | alloys |
a specific type of alloy in which another metal is dissolved in mercury | amalgams |
mixtures of matter that readily separate such as water and oil. | emulsions |
How is percent concentration expressed? | weight/weight; grams/grams
weight/volume; grams/liters
volume/volume; milliliters/liter
**mg/100mL |
How is Molar concentration expressed? | a mole=6.02x10^23
mol/L |
Name the five main types of chemical reactions | synthesis
decomposition
combustion
single replacement
double replacement |
two elements combine to form a product.
2K(+) + 2Cl(-) ---> 2KCL | Synthesis |
opposite of synthesis because it is the breaking of a compound into its component parts. | NaCl ---> Na(+) + Cl(-)
decoposition |
self-sustaining, exothermic chemical reaction usually initiated by heat acting on oxygen and a fuel compound such as hydrocarbon. | combustion |
replacement reactions involve ionic compounds; consist of a more active metal reacting with an ionic compound containing a less active metal to produce a new compound | single replacement |
joining of one atom | chemical bonding |
electrostatic attraction between two oppositely charged ions, or a cation and an anion. | ionic bond |
generally formed between a metal and a nonmetal | ionic |
formed when two atoms share electrons, generally in pairs, one from each atom. | covalent bond |
in a covalently bonded compound, if the electrons in the bond are shared equally, then the bond is termed ____. | nonpolar |
___ is based on the difference in eletronegativity values for the elements involved in the bond. | polarity |
NOT BONDING INTERACTIONS; Weaker forces of attraction between whole mlecules | intermolecular forces |
attraction for a hydrogen atom by a highly electronegative element. | hydrogen bond |
attraction of one dipole on one molecule for the dipole of another molecule | dipole-dipole interactions |
how is a dipole created? | when an electron pair is shared unequally in a covalent bond between two atoms or elements |