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is a positively charged subatomic particle that is found in the nucleus of an atom

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proton

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is a negatively charged subatomic particle that is found in the space outside the nucleus

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electron

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is a neutral subatomic particle that is found in the nucleus of an atom.

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neutron

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equals the number of protons in an atom of that element.

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atomic number

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The sum of the protons and neutrons in the nucleus of an atom. We get this number by rounding the atomic mass. It must be a whole number with no decimals because we cannot have less than one subatomic particle. (for example we cannot have 1/2 or 3/10 of a proton!)

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mass number

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Atoms of the same element that have different numbers of neutrons and different mass numbers. Because they are the same element they will have the same atomic number. The difference in the number of neutrons is related to the difference in the mass number!

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isotope

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The weighted average of the masses of the isotopes of an element. (will typically be a decimal number and does not generally represent the mass of a particular atom of an element but will be closest to the isotope which is more commonly found)

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atomic mass

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a region of an atom in which electrons of the same energy are likely to be found

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energy level

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a visual model of the most likely locations for electrons in an atom (we cannot identify a specific location but use probability to determine roughly where the electrons will most likely be)

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electron cloud

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a region in an atom where there is a high probability of finding electrons (we have used this term interchangeably with electron cloud and energy level)

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orbital

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The arrangement of electrons in the orbitals of an atom. The most stable of these is the one in which the electrons are in orbitals with the lowest possible energies. (in other words if we were filling a Bohr model we would place the electrons in the first energy level and would not go to the second until the first level was full, then electrons in the second level and fill this before going to the third...). This arrangement is also responsible for the chemical properties of the element.

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electron configuration

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When all the electrons in an atom have the lowest possible energies, the atom is said to be in its ground state. Electrons can be excited and removed from this state by going to a higher energy level but they won't stay there indefinitely.

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ground state

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the positively charged dense center of an atom where the protons and neutrons are found

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nucleus

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Having no net electric charge. An atom with the same number of protons and electrons.

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neutral

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the force between electrically charged objects (like charges repel and opposite charges attract each other)

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electrostatic force

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a particle smaller than an atom, such as a proton, neutron, or electron

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subatomic particle

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a tiny particle or packet of light energy (this is emitted when an electron returns from an excited state to its ground state)

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photon

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an electron that is found in the outermost shell of an atom and that determines the atom's chemical properties

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valence electron

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the average when the numbers have different weights. We use this to find the atomic mass for the periodic table. However, you can use this to calculate your grades also since each category tests, quizzes, labs, and homework make up a different portion of your grade. For example Homework is only 12% of your final grade but you have several homework assignments so you take the average of all of your homework assignments and then multiply by .12. This will tell you the amount that this type of assignment contributes to your weighted grade.

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weighted average

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A horizontal row of elements in the periodic table.

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period

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Vertical columns of the periodic table. The elements within a group have similar properties. This is because the elements have the same number of valence electrons.

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group

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The pattern of repeating properties on the periodic table. Properties of elements repeat in a predictable way when atomic numbers are used to arrange elements into groups. The elements in a group have similar electron configurations. An element's electron configuration determines its chemical properties. Therefore, members of a group in the periodic table have similar chemical properties.

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periodic law

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A table that shows all of the known elements, their atomic number, symbol, and weighted average atomic mass. Elements with similar properties are grouped together. Dimitri Mendellev first grouped and organized the elements into what is now known as the periodic table. He used the atomic mass as the primary characteristic to decide where each element belonged in his table. He even left spaces for elements to be discovered because of the pattern he saw once he started organizing those elements known at that that time. Henry Moseley organized the modern periodic table according to atomic number, rather than atomic mass.

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periodic table

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Groups 3-12 of the periodic table. Many of the elements in this group have more than one possible charge.

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transition metals

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This category of elements are usually gases at room temperature. However, they can be found in other states and will be dull in appearance, poor conductors of heat and electricity (poor conductivity). All of these are found above and to the right of the metalloids on the periodic table except Hydrogen.

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nonmetals

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This category of elements are generally solids at room temperature, are shinny (or have metallic luster), are good conductors of heat and electricity (good conductivity). All of these can be found below and to the left of the metalloids on the periodic table. (note that Hydrogen does not fall into this category despite that it is located on the same side of the periodic table)

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metals

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This category of elements have characteristics of metals and nonmetals. They form a sort of staircase of elements, including B, Si, Ge, As, Sb, Te.

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metalloids

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The ease and speed with which an element combines, or reacts, with other elements and compounds. This is determined by the electron configuration of the element.

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reactivity

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First to theorize the concept of the atom in 5th century BC. The word atom is derived from the Greek word "atomos", meaning indivisible.

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Democritus

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1. All matter is made up of individual indivisible particles called atoms (this is the solid sphere model). 2. All atoms of a given element are identical in properties. Atoms of different elements have different properties. 3. Compounds are formed by a combination of 2 or more atoms 4. Atoms cannot be created, destroyed, or converted into other kinds of atoms during chemical reaction

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Dalton's model of atom

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This model gave evidence that the atom was made up of smaller particles. Called the plum pudding model, this model has negatively charged particles mixed throughout a positive "soup". We have also called it the chocolate chip cookie dough or muffin with chunks model.

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Thomson Model of atom

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This scientist conducted an experiment with gold foil and discovered that the atom was made up of mostly empty space with a dense positively charged nucleus. His model shows this positive nucleus with negatively charged particles somewhere outside the nucleus but not in specific locations.

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Rutherford model of atom

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This model of the atom is also called the planetary model of the atom because it shows electrons orbiting the nucleus in distinct energy levels. This model is great for showing how the electrons are placed outside of the nucleus but is not the most recent model of the atom. The light specra of atoms is evidence of Bohr's atomic model-because light gets emitted from an atom in quantized (fixed) amounts.

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Bohr model of atom

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An atom model wherein electrons are no longer depicted as particles moving around the nucleus in a fixed orbit. Instead, as a quantum mechanically-influenced model, we shouldn't know exactly where they are, and hence describe their probable location around the nucleus only as an arbitrary 'cloud'.

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Wave Mechanical/ Quantum, Electron cloud model of atom

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2

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max # of electrons in first energy level of Bohr model

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8

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max # of electrons in second energy level of Bohr model

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For all elements but Hydrogen and Helium 8 is the max number of valence electrons to be stable or non-reactive Hydrogen and helium only need 2 since this is the maximum in the first energy level.

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# of valence electrons to be stable

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farthest right in the periodic table. Group 18 all of these have a full valence shell with 8 electrons except Helium which has a full valence shell with 2 electrons.

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noble gasses

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farthest left in the periodic table in Group 1 all of these have 1 valence electron and are metals except Hydrogen which is a non-metal but is located above this group because it has 1 valence electron. They are the most reactive of the metals

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alkali metals

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group 2 elements

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alkaline earth metals

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group 17 elements - most reactive of the non-metals

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halogens

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the number of valence electrons

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Looking at the group number of the element will tell us what?

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the number of energy levels the element has.

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The period of an element gives us what information?

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reactivity of the element (how it will bond with other elements to form molecules and compounds).

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the number of valence electrons gives us a clue about what?

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These are all electrons being placed in the Bohr model of an atom. They are found orbiting the nucleus in distinct energy levels.

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Where are electrons on the Bohr model of the atom?

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The protons and neutrons are in the nucleus and it is represented by #5 in the diagram.

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What subatomic particles are in the nucleus of an atom? And where is the nucleus of an atom located?

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This image represents Dalton's model of the atom. According to Dalton, the atom was a hard sphere.

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Dalton model (Image)

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They are located in the outermost shell.

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Where are valence electrons of an atom located?

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This image represents JJ Thompson's "plum pudding" model of the atom.

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Thomson model of atom (picture)

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This image represents Rutherford's "nuclear" model of the atom. Small dense positively charged nucleus surrounded by negative electrons.

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Rutherford model (picture)

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Bohr's model built on the Rutherford model, because Bohr theorized that the locations of the electrons outside the nucleus weren't random, but that they were located in well-defined orbits. Don't get orbits confused with orbitals.

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Bohr model (picture)

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Our currently accepted theory of the atom. Electrons exist in orbitals, which are mathematically predicted, most probable regions of finding electrons. Heisenberg and schrodinger are credited most with this theory.

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Wave mechanical/ quantum/ electron cloud model of the atom (picture)

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The bright line spectrum of an element can be explained with the Bohr model of the atom, which shows that electrons in an atom are in discrete energy states and emit distinct amounts of light when going from higher energy states to lower ones. Since the emission spectrum is different for every element, it acts as an atomic fingerprint by which elements can be identified. Some elements were discovered by the analysis of their atomic spectrum. Helium, for example, was discovered while scientists were analyzing the absorption spectrum of the sun.

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Bright Line Spectra (Picture)

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