Term
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Definition
| Anything with mass that takes of space |
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Term
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Definition
| Building blocks of matter |
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Term
| What are the 3 basic states of matter? |
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Definition
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Term
| What are characteristics of gases? |
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Definition
- Disorder
- Much empty space
- Complete freedom of motion
- Particles far apart
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Term
| What are characteristics of liquids? |
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Definition
- Some disorder
- Particle clusters free to move relative to eachother
- Particles close together
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Term
| What are characteristics of solids? |
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Definition
- Ordered arrangement
- Particles essentially in fixed positions
- Particles close together
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Term
| What are examples of physical changes to a substance? |
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Definition
| Change of state; solid to liquid |
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Term
| What are examples of chemical changes of a substance? |
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Definition
| Creating a new chemical substance by combustion, oxidation, decomposition, etc. |
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Term
What is an intensive property?
Give examples. |
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Definition
- Independent of the amount of substance present
- Color, Density
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Term
What is an extensive property?
Give examples. |
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Definition
- Dependent on the amount of substance present
- Mass, volume
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Term
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Definition
| Use of boiling points to separate a homogenous mixture |
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Term
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Definition
| Separating a substance on the basis of solubility in water |
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Term
| If matter is unifofrm throughout and can't be separated into other substance by physical processes, but can be decomposed into other substances by chemical processes, it is called a __________. |
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Definition
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Term
| Define accuracy vs. precision |
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Definition
- Accuracy: refers to the proximity of a measurement to the true value
- Precision: refers to the proximity of several measurements to eachother
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Term
| What are the 4 postulates of Daltons atomic theory of matter? |
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Definition
- All elements are made of tiny particles called atoms
- All same type atoms are identical in properties, but different type atoms can be distinguished
- An atom can't be converted to another type of atom
- Compounds can be formed
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Term
| Who discovered the electron? |
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Definition
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Term
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Definition
| Spontaneous emmision of radiation by an atom |
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Term
| Who discovered the nucleus? |
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Definition
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Term
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Definition
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Term
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Definition
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Term
| What is a combination reaction? |
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Definition
| Combining 2 or more substances to form 1 product |
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Term
| What is a decomposition reaction? |
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Definition
| Breaking apart a comound into 2 or more substances |
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Term
| What is a combustion reaction? |
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Definition
| A rapid reaction that produces a flame, often involving hydrocarbons reacting with oxygen in the air |
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Term
| What is an empirical formula? |
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Definition
| Formula reduced to represent the smallest ration of elements in a compound. |
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Term
| What is Avogadros number? |
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Definition
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Term
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Definition
| Substance that dissociates into ions when dissolved in water |
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Term
| Describe a strong electrolyte vs. a weak electrolyte. |
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Definition
- Strong: dissociates completely when dissolved in water
- Weak: partially dissociates when dissolved in water
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Term
| What is a non electrolyte? |
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Definition
| Does not dissociate into ions when dissolved in water |
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Term
| What is a main purpose of electrolytes? |
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Definition
| Dissociated ions allow a current to be passed through a solution |
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Term
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Definition
| What you have the most of in a solution |
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Term
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Definition
| Substance dissolved into the solvent |
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Term
| What is an oxidation reduction reaction? |
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Definition
| Corrosion of a metal when it interacts with some other substance in the environment |
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Term
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Definition
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Term
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Definition
| When a substance gains electrons |
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Term
| What is the numonic device to remember what oxidation is and what reduction is? |
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Definition
OIL RIG
Oxidation Is Loss
Reduction Is Gain |
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Term
What are rules for determining oxidation numbers?
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Definition
- ON of a monatomic ion is the same as its charge
- Nonmetals usually have - ON's
- Sum of ON's in a neutral compund is 0
- Always change during redox reactions
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Term
| What is the definition of work as it pertains to thermochemistry? |
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Definition
| Energy used to cause an object with mass to move. |
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Term
| What is the definition of heat as it pertains to thermochemistry? |
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Definition
| Energy used to cause an objects temperature to rise |
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Term
| What is the formula for work? |
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Definition
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Term
| What is the 1st law of thermodynamics? |
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Definition
| Energy is neither created nor destroyed |
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Term
| What is an endothermic reaction? |
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Definition
| A reaction that absorbs heat |
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Term
| What is an exothermic reaction? |
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Definition
| Reaction that releases heat |
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Term
| What is electromagnetic radiation? |
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Definition
| The emission of light thats composed of electric and magnetic fields |
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Term
| What is the Pauli Exclusion Principle? |
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Definition
| No 2 electrons in the same atom can have the same energy |
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Term
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Definition
| If you have unpaired electrons in an atom, they will fill all orbitals before pairing up |
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Term
| What are quantum numbers? |
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Definition
| Used to describe the position of which electrons may be found |
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Term
| What is the principle quantum number (n)? |
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Definition
| Describes the energy level on which the orbital resides |
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Term
| What is the angular momentum quantum number (l)? |
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Definition
| Defines the shape of an orbital |
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Term
| What is the magnetic quantum number (ml)? |
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Definition
| Describes the 3D orientation of the orbital |
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Term
| How do you determine possible values for l? |
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Definition
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Term
| How do you determine possible values for ml? |
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Definition
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Term
| Describe the trend of effective nuclear charge across the periodic table. |
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Definition
| Increases from left to right |
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Term
| What factors determine ionic size? |
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Definition
| Nuclear charge, Number of electrons, and the orbitals in which the electrons reside |
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Term
| Describe the size of cations |
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Definition
| Smaller than their parent atoms |
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Term
| Describe the size of anions |
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Definition
| Larger than their parent atoms |
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Term
| What is ionization energy? |
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Definition
| Amount of energy required to remove an electron from the ground state of an atom |
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Term
| Describe how ionization energy increases on the periodic table. |
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Definition
| Increases as you go up the periodic table and from left to right |
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Term
| What is first ionization energy? |
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Definition
| Amount of energy required to remove the first electron from an atom |
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Term
| Describe the concept of electron configuration of ions. |
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Definition
| Electrons are removed from the highest principle quantum number first. |
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Term
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Definition
| Bond between a metal and a non metal |
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Term
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Definition
| Bond between 2 non metals |
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Term
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Definition
| In a covalent bond, electrons are not equally shared |
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Term
| What is a non polar bond? |
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Definition
| In a covalent bond, electrons are equally shared |
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Term
| What is electronegativity? |
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Definition
| Ability of atoms in a molecule to attract electrons to themselves. |
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Term
| What is the trend of electronegativity on the periodic table? |
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Definition
| Increases from left to right and bottom to top |
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Term
| What's the relationship between polarity and electronegativity? |
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Definition
| The greater difference in electronegativity, the more polar the bond is |
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Term
| What is the VSEPR theory? |
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Definition
| Best arrangement of electron domains to minimize repulsions among them. |
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Term
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Definition
| Characterized by head to head overlap, always single bonds |
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Term
| What are characteristics of single bonds? |
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Definition
| Stronger bond with lower energy |
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Term
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Definition
| Characterized by side to side overlap, prevent bond rotation |
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Term
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Definition
| One sigma bond, and the rest are pi bonds, weaker than sigma bond. |
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Term
| What is the internal energy of a system? |
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Definition
| Sum of the potential and kinetic energies of the components |
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Term
| When a system gives off heat and does work on its surroundings, the change in energy is _________ __________. |
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Definition
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Term
| The energy of a photon light is __________ proportional to its frequency an _________ proportional to its wavelength. |
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Definition
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Term
| In regards to the periodic table, how does atomic radius increase? |
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Definition
| Down a group and from left to right across a period. |
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Term
| What does it mean to be isoelectronic? |
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Definition
| Ion that has the same electron configuration |
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