Chemistry 1 Final Review Test Questions – Flashcards
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| What is matter? |
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| Anything with mass that takes of space |
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| What are atoms? |
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| Building blocks of matter |
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| What are the 3 basic states of matter? |
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| Solid, Liquid and Gas |
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| What are characteristics of gases? |
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| What are characteristics of liquids? |
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| What are characteristics of solids? |
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| What are examples of physical changes to a substance? |
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| Change of state; solid to liquid |
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| What are examples of chemical changes of a substance? |
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| Creating a new chemical substance by combustion, oxidation, decomposition, etc. |
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What is an intensive property? Give examples. |
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What is an extensive property? Give examples. |
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| What is distillation? |
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| Use of boiling points to separate a homogenous mixture |
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| What is chromatography? |
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| Separating a substance on the basis of solubility in water |
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| 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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| Comound |
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| Define accuracy vs. precision |
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| What are the 4 postulates of Daltons atomic theory of matter? |
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| Who discovered the electron? |
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| J.J. Thompson |
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| What is radioactivity? |
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| Spontaneous emmision of radiation by an atom |
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| Who discovered the nucleus? |
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| Rutherford |
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| Who discovered protons? |
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| Rutherford |
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| Who discovered neutrons? |
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| Chadwick |
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| What is a combination reaction? |
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| Combining 2 or more substances to form 1 product |
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| What is a decomposition reaction? |
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| Breaking apart a comound into 2 or more substances |
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| What is a combustion reaction? |
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| A rapid reaction that produces a flame, often involving hydrocarbons reacting with oxygen in the air |
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| What is an empirical formula? |
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| Formula reduced to represent the smallest ration of elements in a compound. |
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| What is Avogadros number? |
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| 6.02*10^23 molecules/mol |
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| What is an electrolyte? |
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| Substance that dissociates into ions when dissolved in water |
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| Describe a strong electrolyte vs. a weak electrolyte. |
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| What is a non electrolyte? |
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| Does not dissociate into ions when dissolved in water |
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| What is a main purpose of electrolytes? |
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| Dissociated ions allow a current to be passed through a solution |
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| What is a solvent? |
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| What you have the most of in a solution |
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| What is a solute? |
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| Substance dissolved into the solvent |
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| What is an oxidation reduction reaction? |
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| Corrosion of a metal when it interacts with some other substance in the environment |
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| What is oxidation? |
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| Loss of electrons |
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| What is reduction? |
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| When a substance gains electrons |
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| What is the numonic device to remember what oxidation is and what reduction is? |
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OIL RIG Oxidation Is Loss Reduction Is Gain |
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What are rules for determining oxidation numbers?
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| What is the definition of work as it pertains to thermochemistry? |
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| Energy used to cause an object with mass to move. |
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| What is the definition of heat as it pertains to thermochemistry? |
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| Energy used to cause an objects temperature to rise |
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| What is the formula for work? |
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| Work = Force * Distance |
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| What is the 1st law of thermodynamics? |
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| Energy is neither created nor destroyed |
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| What is an endothermic reaction? |
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| A reaction that absorbs heat |
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| What is an exothermic reaction? |
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| Reaction that releases heat |
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| What is electromagnetic radiation? |
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| The emission of light thats composed of electric and magnetic fields |
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| What is the Pauli Exclusion Principle? |
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| No 2 electrons in the same atom can have the same energy |
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| What is Hund's rule? |
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| If you have unpaired electrons in an atom, they will fill all orbitals before pairing up |
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| What are quantum numbers? |
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| Used to describe the position of which electrons may be found |
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| What is the principle quantum number (n)? |
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| Describes the energy level on which the orbital resides |
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| What is the angular momentum quantum number (l)? |
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| Defines the shape of an orbital |
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| What is the magnetic quantum number (ml)? |
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| Describes the 3D orientation of the orbital |
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| How do you determine possible values for l? |
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| Can range from 0 to n-1 |
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| How do you determine possible values for ml? |
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| Can range from -l to l |
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| Describe the trend of effective nuclear charge across the periodic table. |
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| Increases from left to right |
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| What factors determine ionic size? |
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| Nuclear charge, Number of electrons, and the orbitals in which the electrons reside |
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| Describe the size of cations |
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| Smaller than their parent atoms |
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| Describe the size of anions |
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| Larger than their parent atoms |
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| What is ionization energy? |
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| Amount of energy required to remove an electron from the ground state of an atom |
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| Describe how ionization energy increases on the periodic table. |
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| Increases as you go up the periodic table and from left to right |
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| What is first ionization energy? |
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| Amount of energy required to remove the first electron from an atom |
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| Describe the concept of electron configuration of ions. |
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| Electrons are removed from the highest principle quantum number first. |
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| What is an ionic bond? |
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| Bond between a metal and a non metal |
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| What is a covalent bond? |
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| Bond between 2 non metals |
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| What is a polar bond? |
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| In a covalent bond, electrons are not equally shared |
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| What is a non polar bond? |
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| In a covalent bond, electrons are equally shared |
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| What is electronegativity? |
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| Ability of atoms in a molecule to attract electrons to themselves. |
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| What is the trend of electronegativity on the periodic table? |
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| Increases from left to right and bottom to top |
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| What's the relationship between polarity and electronegativity? |
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| The greater difference in electronegativity, the more polar the bond is |
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| What is the VSEPR theory? |
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| Best arrangement of electron domains to minimize repulsions among them. |
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| What are sigma bonds? |
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| Characterized by head to head overlap, always single bonds |
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| What are characteristics of single bonds? |
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| Stronger bond with lower energy |
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| What is a pi bond? |
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| Characterized by side to side overlap, prevent bond rotation |
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| Describe multiple bonds. |
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| One sigma bond, and the rest are pi bonds, weaker than sigma bond. |
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| What is the internal energy of a system? |
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| Sum of the potential and kinetic energies of the components |
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| When a system gives off heat and does work on its surroundings, the change in energy is _________ __________. |
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| Always negative |
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| The energy of a photon light is __________ proportional to its frequency an _________ proportional to its wavelength. |
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| Directly, Inversely |
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| In regards to the periodic table, how does atomic radius increase? |
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| Down a group and from left to right across a period. |
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| What does it mean to be isoelectronic? |
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| Ion that has the same electron configuration |
