Quarerly exam 1 | Dive education

Data,

A collection of facts and information, which you may have recorded during an experiment, from which conclusions and decisions can be made.

deductive reasoning,

Starts with general statements and leads towards specifics ("logic leads to truth").

inductive reasoning,

Starts with facts and works towards general conclusions (science).

observation,

The act of receiving information through the senses, and recording it.

science,

A systematic study through careful observation, collection of data, and experimental investigation; observations of the physical universe.

truth,

Anything that is not false.

pure science,

t is based on deductions from demonstrated facts and truths, but is not focused on practical applications, "the quest for knowledge".

applied science,

Solving practical problems by the application of one or more fields of pure science.

faith,

Confidence or trust in something, that is not based on actual proof.

bias,

An inclination or predisposition in a certain direction that prevents an unprejudiced consideration of a question.

fact

Something that actually exists, that has been observed or experienced.

metal

The group of elements that are characterized as being good conductors, and the tendency to give up electrons in a reaction.

metalloid

Elements that exhibit metallic and nonmetallic qualities.

nonmetal

The group of elements that are characterized as being poor conductors, and the tendency to gain electrons in a reaction.

metallic hydride

Compounds formed by the reaction of hydrogen with an active metal.

alkali metal

Highly reactive chemical elements that form group 1 (IA); each have one valance electron.

alkaline earth metal

A series of elements that forms group 2 (IIA); each have two valence electrons.

transition metal

A group of strong metals that exhibit similar characteristics, and can be found in groups 3-12 (IB-VIIIB) of the period table.

inner transition metal

A group made up of the lanthanide and actinicide series.

post-transition metal

A group of metals found in groups IIIA, IVA, and VA.

actinide series

A series of inner transitional metals with atomic numbers from 90 to 103. It is one of the series placed under the table, for a more convenient shape.

lanthanide series

A series of inner transitional metals with atomic numbers from 58 to 71. It is one of the series placed under the table, for a more convenient shape.

semiconductor

A material that allows for partial conductivity. It conducts better than an insulator, but not as well as a conductor.

oxide

Binary compounds formed by reactions between oxygen, and any element beside the noble gasses.

sulfide

A compound formed with sulfur that has its lowest oxidation number of -2.

halogen

A reactive group of elements that all have seven valence electrons, and are located in group 17 (VIIA).

noble gas

The elements from group 18 (VIIIA) that all have 8 valence electrons (except helium, which has two) and are characterized as being very stable.

atomic radius

A trend that decreases as you move from left to right across a period in a periodic table, and that increases as you move down a group.

electrostatic attraction

Forces causes by opposite charges between two particles.

ionization energy

The minimum energy required to remove an atom's outermost electron. This trend increases as you move from left to right across a period in a periodic table, and decreases as you move down a group.

electron affinity

The amount of energy released when an electron joins an atom to form a negative ion. This trend increases as you move from left to right across a period in a periodic table, and decreases as you move down a group.

electronegativity

The degree of attraction an atom has for additional electrons. This trend increases as you move from left to right across a period in a periodic table, and decreases as you move down a group.

periodic table

A chart containing all of the elements arranged into rows and columns, based on recurring trends of their properties.

periodic law

The physical and chemical properties of elements occur in a systematic manner that correlates with their atomic number.

group or family

Sometimes referred to as a group, it is a vertical column in the periodic table.

period or series

Horizontal rows of the periodic table, sometimes referred to as series.

North American Convention Periodic Table

The most common form of the periodic table in the US, that uses A and B designations for main groups or transitions metals. For families, Arabic numerals are sometimes substituted for Roman numerals.

European Convention Periodic Table

A form of the periodic table that uses different A and B designations, and different family labels than the North American Convention.

IUPAC Periodic Table

A form of the periodic table that does not use A and B designations, and labels the families 1-18 in Arabic numerals.

atomic mass unit

The unit of measure used to express the mass of an atom, defined as one-twelfth the mass of an atom of carbon-12.

mass number

The total number of protons plus neutrons of an atom.

atomic number

The number of protons in an atom. It is always constant, and can be used to identify an atom.

isotope

Elements whose atoms have the same number of protons, but a different numbers of neutrons.

atomic mass

The mass of an atom, including its protons, neutrons, and electrons. It is usually expressed in atomic mass units (amu).

valence electron

The electrons that make up the outermost energy level, and that play a key role in determining how atoms react with each other.

electron-dot structure

Also known as Lewis dot structures, they are diagrams that show the valence electrons of an element. They are made up of the element's symbol surrounded by dots representing its electrons, and can be used to show bonds between atoms.

ion

An atom or molecule that carries a charge due to the gain or loss of an electron.

cation

An ion that carries a positive charge.

anion

An ion that has a negative charge.

principal energy level

The area occupied by a specific group of electrons orbiting the nucleus.

orbital

A section of a sublevel that shows the specific area that an electron is most likely to be in, given its amount of energy.

sublevel

A division of a principal energy level that contains one or more orbitals.

Pauli exclusion principle

A maximum of two electrons, with opposing spin, can occupy an orbital.

diagonal rule

A diagram that can be used to remember the order that energy levels and sublevels are filled.

Aufbau principle

The arrangement of electrons in a small atom have the same configuration as the lower levels of a larger atom. Adding electrons to the smaller atom will give the configuration of larger atoms.

electron configuration

The arrangement of electrons given by principal energy level, sublevel, and electrons per sublevel.

orbital notation

A section of a sublevel that shows the specific area that an electron is most likely to be in, given its amount of energy.

photon

The basic unit of light, or any other form of electromagnetic radiation.

Hund's rule

As sublevels are being filled, each orbital receives one electron, before the first is filled with two.

quantum number

A series of numbers that give the location of an electron by size of principal energy level, type of sublevel, direction of orbital, and spin.

atom

The smallest unit of elements, made up of electrons surrounding the nucleus of protons and neutrons.

model

A schematic description of a complex system, process, or theory based on experimental data.

Law of Definite Composition

A compound is always composed of the same distinct proportion of elements by mass.

quantum

The discrete, minimum amount of energy involved in an interaction.

electron

Particles that are smaller than protons or neutrons, they have a negative charge

neutron

Particles that have a neutral charge.

proton

Particles that carry a positive charge, and the number of protons distinguishes one element from another.

continuous spectrum

Contains all colors, with no distinct boundaries between them.

line spectrum

Diagrams the distinct frequencies for all the light waves from a given source.

quantized

A set values that are separate and discrete, as opposed to being continuous.

principal energy level

The area occupied by a specific group of electrons orbiting the nucleus.

Heisenberg uncertainty principle

It is not possible to know the exact velocity and position of an electron at the same time.

mass

Usually used interchangeably with weight, because an object's mass and weight are proportional to each other. The quantity of inertia possessed by an object that can be multiplied by the acceleration due to gravity to determine its weight.

weight

The force that gravity exerts on an object. It is the mass of an object multiplied by acceleration due to gravity.

density

The mass per unit volume of a substance.

accuracy

The degree of closeness between a measured value, and its actual value.

precision

The degree of closeness of repeated measurements. How close the results of multiple trials of something are to each other.

significant digit

The number of digits known for certain, plus one estimated digit.

scientific notation

A method of expressing extremely large or extremely small numbers, using powers of ten.

SI system

System international, it is an internationally agreed upon system of measurement for mass, distance, and volume based on the metric system.

unit analysis

A method of converting between various units of measure.

unit multiplier (conversion factor)

A fraction made up of equivalent measures, that is equal to one. It is used to convert from one unit to another.

energy

The ability of an abject to move something, or be moved. The ability to do work, by a force.

endothermic

A reaction that absorbs energy, in the form of heat.

exothermic

A reaction that releases energy, in the form of heat.

kinetic theory

Particles are in constant motion. In a solid they may just vibrate next to each other, but in a liquid or gas they travel much faster.

kinetic energy

The energy of an object caused by its motion.

temperature

A measure of the average kinetic energy of the particles in a substance.

heat

The transfer of kinetic energy from one substance to another.

1st Law of Thermodynamics

Energy cannot be created or destroyed, it just changes form.

2nd Law of Thermodynamics

In an energy conversion, some energy goes to an unusable form.

solid

A state of matter in which the object has a definite shape and volume.

liquid

A state of matter which is characterized as having definite volume, but no definite shape.

gas

A state of matter in which the particles move about freely, with no structure. It will always fill the container it is in, assuming its size and shape.

plasma

A state of matter similar to gas, but in which the particles are moving at much greater speeds, and are electrically charged.

condensation

A phase change in which a substance transitions from the gas phase, to the liquid phase.

evaporation

The physical change of a liquid changing states into a gas.

freezing

The process in which a liquid undergoes a phase change to become a solid.

melting

The process in which a solid changes phases into a liquid.

sublimation

The process in which a solid transitions directly into a gas, without becoming a liquid.