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105 Cards in this Set
- Front
- Back
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Atomic Structure |
Protons and Neutrons in Nucleus Electrons outside
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Nucleus |
dense Positively charged center of Atom containing Protons and neutrons |
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What determines the atomic # of an element? |
# of Protons
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What is the element #on the Periodic table called? |
Atomic Number |
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You cannot change _________ in regular chemistry? |
Protons |
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Are atoms of an elements of the periodic table charged? |
No unless you are told, They are neutral because the # of Protons = # of electrons |
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You can change the # of__________ in an atom without changing what element it is. |
Electrons |
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Atomic Theory |
1. All matter is composed of atoms. 2. Atoms of a given element differ than all other elements. 3. Chemical compounds have a defined ratio. 4. Chemical Reactions only change the way atoms are combined in compounds, the elements are unchanged. |
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Atomic masses are expressed in _________? |
Atomic Mass Unit (amu) |
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Subatomic Particle |
very small particle that is a building block for an atom |
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What are the 3 types of subatomic particles? |
Protons Neutrons Electrons
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Electron |
smallest subatomic particle and has negative charge |
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Proton |
Subatomic particle with + charge
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The charge of ______ and __________ are equal but opposing. |
Protons and Electrons |
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Charge of Proton |
+1` |
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Charge of Electron |
-1 |
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Neutron |
subatomic particle with no charge |
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Nucleon |
Any subatomic particle in nucleus; thus protons and neutrons |
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A mass # = |
Number of protons and Neutrons |
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Element |
Pure substance in which all atoms have same atomic # |
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Isotope |
atoms of an element that have same number of protons and electrons but different neutrons |
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19 A F F 9 Z |
Mass # (A) Symbol Atomic # (z) |
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Atomic Mass |
Calculated average mass of isotopes of a given element and takes in to account abundant of each isotopes |
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Why do some elements have similar characteristics? |
Similar number of electrons and their arrangement |
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Shells Characteristics |
Principle energy Levels 1st shell is n=1 Each shell has subshells The further away the higher the energy
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S shell has how many subshells? |
1orbital
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P shell has how many subshells? |
3 orbital |
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d shell has how many subshells? |
5 Orbital |
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How many electrons can be in each orbital? |
2 |
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Electron Shell |
a region of space about a nucleus that contains electrons that have approx. the same energy and that spend most of their time approx. the same distance form the nucleus |
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Electron Subshell |
region of space within a shell that contains electrons with about same energy
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# of Subshells = # of ___________ |
Shells |
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Electron orbital |
region of space within a subshell in which the electrons are most likely to be |
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Describe two electrons in an orbital |
they always spin in opposite directions |
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Rules for electrons
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1. Subshells are filled in order of increasing energy
2. Each orbital gets one before a second adds to any orbital 3. only 2 and they have opposing spin |
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Electron Configuration |
statement of how many electrons are in each subshell |
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Example of Electron Configuration |
# Lower case letter (s,p,d,f) followed by superscripts of the # of electrons in that subshell |
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Orbital Diagram |
Uses same 1s Followed by arrows noting electrons in orbital and direction of spin; 1st is always upward followed by downward |
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Why does the d row of the periodic table drop? |
Some overlap of energy levels occur beginning in shell 3 and 4 |
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if you add all superscript or arrows the # should = |
# of electrons
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Distinguishing electron |
last electron added to electron configuration |
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Noble Gas |
element located in the far right column; colorless gas and not very reactive |
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Representative Element |
element located the S area of or the first 5 columns of the P |
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4 most abundant elements in human body |
C, H, O, N |
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Alkali metals |
most left column; excluding H, react rapidly with water to form flammable H2 gas and alkaline or base solutions, low melting points, ; soft shiny metals |
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Alkaline earth Metals |
second column to the left; |
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Transition Metal |
element located in d area; metals; |
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Inner Transition metal |
Man made elements in f subshell |
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How can we find atomic weight without table? |
% isotope/ 100 X mass of isotope +
%/100 X mass of isotope
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Z represents |
# of protons
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A represents |
# of Neutrons |
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Types of electron Configurations |
1. Long hand complete 2. Orbital 3. Short hand
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How do you short hand electron configurations? |
You bracket the last noble gas and add form there
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Valence Shell |
outermost shell with highest energy |
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Valence electrons |
electrons in outermost valence shell that have a lot of energy and are loosely held |
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What is important in determining an electron's properties? |
valence electrons |
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Halogens and Halides |
F, Cl, Br, I and Ar; Colorful corrosive nonmetals, found in nature with other in combination with other elements ie: NaCl |
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Octet Rule |
1. Atoms want 8 valence electrons 2. They will react to gain or lose until they have 8 3. Atoms that gain or lose electrons by reacting with another atoms is an ion |
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Do Noble gas gain or lose electrons easy? |
No |
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Can Transition Metals form more than one oxidation state? |
Yes |
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Al oxidation state |
+3 |
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Zn oxidation state |
+2 |
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Ag oxidation state
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+1 |
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Chemical compound |
attractive force that holds two atoms together |
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Ionic Compound |
compound that contains ions |
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Covalent Bond (molecular Bond) |
chemical bond formed by sharing of one or more electrons
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ion |
atom that has added or lost an electron
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Cation |
ion with a positive charge |
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Anion |
ion with a negative charge |
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Fixed oxidation state |
only make one oxidation state ie: Alkalis +1, Alkalines +2 |
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variable oxidation state |
atom may make a + or negative oxidative state C and N columns and transition metals vary
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Group |
Vertical column on periodic table
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Period |
horizontal row on periodic table
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Metals Always make what type of ions? |
Cations |
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Nonmetals usually make what type of ions? |
Anions |
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Compounds have what charge? |
Always neutral, no charge
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ionic bond |
electrical attractions between ions of opposing charges |
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Oxidation State |
charge on an ion |
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FeCl2 |
Cl is 1- iron must be 2+ |
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ions
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Write Cation 1st
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Polyatomic ion |
composed of more than 1 atom |
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Naming Ionic Compounds |
1. Write cation name 1st 2. Write anion+ide 3. If cation has more than one oxidation state write it |
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Roman Numerals |
Type 1 only make one ion NO Roman! Type 2 makes more than 1 cation ROMAN NUmeral! |
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Chlorate
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Iodate
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Fluorate
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Phosphate
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Nitrate
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Hydrogen Phosphate
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dihydrogen hosphate
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Hydrogen sulfate / bisulfate
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Thiosulfate
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Oxolate
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Permanganate
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Hydroxide
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Acetate
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Acetate
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Ammonium
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Chromate
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Cyanide
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Dichromate
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How do you go from Bromate to Perbromate?
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Add an oxygen when you add Per
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How do you go from Bromate to Bromite?
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Going from ate to ite you take away an oxygen
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How do you go from Bromite to hypobromite?
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going from ite to hypo+ite you take away an oxygen
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What happens when you have a polyatomic ion ending in ate and you add a H?
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you take away one electron (charge)
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