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76 Cards in this Set
- Front
- Back
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Definition of periodic table |
It organizes info avout all the known elements |
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What part of the periodic table tells us the number of electron shells and orbitals? |
Periods |
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7 characteristics of metals |
-Ductile and shiny -mallable -react w water -good conductor -corrode -Easily lose electrons -High melting point |
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6 characteristics of nonmetals |
-Poor conductors -Nor ductile/dull color -Brittle and light -low melting point -tend to gain electrons -are mostly gases |
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Has a family of its own |
Hydrogen |
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Memorize some elements in different families |
Dond |
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Rule: when atoms of an element react. They tend to lose, gain and share electrons to achieve 8 stable valence electrons such as the noble gases. |
Octet rule |
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A process in which one or more pure substances are converted to one or more pure substances |
Chemical reaction |
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Two laws of physics: bonding |
1. Opposites attract and likes repel 2. Nature moves in the direction of the least resistance (lowest energy) |
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Relative ability of a molecule to attract shared electrons to itself |
Electronegativity |
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Electronegativity increases from ___ to ____ and decreases _____ |
Left to right, decreases down the group |
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Metals are more electropositive |
True |
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What is the most electronegative element and the least electronegative one? |
Fluorine, Francium |
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When elements obtain a charge, they become |
Ions |
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Ionic bonding |
Attraction between negative and positive ions forms ionic compounds |
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Why do ions stick together? |
Electrostatic force |
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Properties of ionic compounds |
-crystalline structure (magnet electrostatic force) -Ions are bonded sTronger -conduct electricity -high melting point |
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Non metal.shares electrons with another nonmetal |
Covalent bonding |
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Covalent bonding is represented by |
Lewis dot structures |
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Hydrocarbon |
Compounds containing hydrogen and carbon |
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A bond between non-metal atoms that have the same electronegativity; thus have an equal sharing of the bonding of electron pair |
Non-polar covalent bond |
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Polar covalent bond |
A bond between 2 nonm metal atoms that have different electronegativities amd thus have an equal sharing of the bonding electron pair |
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Replacement of the nucleus. Releases radiation |
Radioactive decay |
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True or false: The position and momentum of a particle cannot be simultaneously measured with precision |
True |
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Who discovered the uncertainty principle? |
Discovered by W. Heisenberg |
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Quantum Mechanics |
Explains how atoms behave |
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Electrons are not particles but more as ____ w/c gain electronz |
Waves |
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Quantum/ quanta |
Amount of energy that electrons need to gain to move to the next energy level |
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An area where u can find electrons |
Atomic orbitals |
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Calculates the probabilities where you will be able to find electrons |
Quantum mechanics |
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4 quantum numbers |
Principal quantum number Angular Magnetic Spin |
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Describe s orbital (shape and where nucleus is) |
Spherical, nucleus at center |
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Describe p orbital |
Dumbbbel shaped, nucleus at middle |
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Describe d orbital |
Elongated dumbell, nucleus at center |
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Describe f orbital |
Shaped like a jackstone, nucleus in middle |
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Describes the behaviour of an electron w/in a magnetic field |
Electron spin |
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Principal quantum number |
Represents an energy level |
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Angular Quantum Number (2) |
1. Sublevels 2. Rep. The type/shape of an orbital |
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Spin Quantum number |
An energy level can hold a max of 8 electrins and must have opposite spins |
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Describe Pauli's exclusion principle |
Paired electrons occupying the same orbital must have opposite spins |
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Electron spin is described as: |
Quantum (m): -1/2, -/12 |
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Magnetic Quantum Number |
The orientation/ position of the orbitals |
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How many orientations do s, p, d, f have? |
S-1 P-3 D-5 f-7 |
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Shorthand description of how electrons are arranged around the nucleus of an atom |
Electron configurarion |
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Predicts whether two elements will react or not, predict chemical behaviour |
Electron configuration |
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In order to write electron configuration, we need to know 3 rules: |
1. Aufbau principle- Niels Bohr 2. Pauli's Exclusion principle- W. Pauli 3. Hund's Rule- F. Hunds |
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Explain Aufbau Principle |
"Construction" in German Electrons enter the lowest energy levels |
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Explain Hund's Rule |
"Empty bus rule" -states that every orbital in a subshell/orientation is singly occupied with one electron before any one orbital is doubly occupied |
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Explain Hund's Rule |
"Empty bus rule" -states that every orbital in a subshell/orientation is singly occupied with one electron before any one orbital is doubly occupied |
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Three scientists that gave definitions to acids and bases |
1. S. Arrenhius 2.Johannes Bronsted and T. Lowry 3. Gilbert Lewis |
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Which scientist said that acids produce and increase H+ while bases produce and inc H- |
Svante Arrhenius |
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What scientist said that acids donate h+, proton donor while bases accept H+ |
Johannes Bronsted and Thomas Lowry |
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A solution that has an excess of H+ ionz |
Acid |
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Latin of acid |
Acidus meaning "tart" or "sour" |
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Which scientist said that acids accept electron pairs while bases donate electron pairs? |
Gilbert Lewis |
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The more H+ ions, the more acidic the solution |
True |
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H ions do not exist as hydrogen in water. Instead... |
They bond to water molecules |
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Formic Acid (symbol and definition) |
HCO2H. "Pissemyre", "myr' means ant |
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Properties of an acid (8) |
1. Tastes sour 2. Conduct electricity 3. React w/active metals 4. Many acids can corride fabric. Skin and paper 5. Turns blue litmus paper red 6. Gives h+ ions 7. Neutrakize bases 8. Ionic compound |
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Uses of acids (5) |
Acetic acid- Citric acid ascorbic acid sulfuric acid car batteries |
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A solution that has an exvess OH-ions |
Base |
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Another word for base |
Alkali |
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Contains properties of bases |
Basic/ alkaline solution |
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Properties of a base (8) |
-bitter -Feels slippery -corrosive -can conduct electricity (alkaline batteries) -do not react w/ metals -can turn litmus paper red into blue -neutralize acids -Ionic conpounds |
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Uses of Base |
Soap, ammonia and many other cleaning products, chalk |
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A measure of how acidic or basic a solution is |
Ph |
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Ph scale ranges from |
0-14 |
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A solution of ph 0 is |
Very acidic |
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Pure water has a pH of |
7 |
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True or falze. A change of 1ph unit represents a tenfold change in the acidity of the solution |
Tru |
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A reaction between an acid and base is called |
Neutralization |
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A solution that resist the change in pH when an acid |
Buffer |
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Common salts |
1. Sodium chloride- food preservative and flavoring 2. Potassium iodide - additive in iodized salt that prevents iodine deficiency |
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Saturated hydrocarbons |
Alkanes |
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If alkalenes have single bonds, they are called |
Cycloalkanes |
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Functions of carbons (6) |
1. Halocarbons- halogen based 2. trichloromethane- chlorofoam 3. Methanol - methyl alcohol 4. Ethanol - ethyl alcohol 5. ether- 6. Carbonyl.group |
