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Rhea Mohan Honors Chemistry 1st Semester Review 1st Period…

- - - - tendency of an atom to attract a shared pair of electrons towards itself
        
        increase left to right, decrease up to down
    - - radius of an atom's ion in ionic crystals structure
        
        decrease left to right, increase up to down
    - - measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding cloud of electrons
        
        decreases left to right, increases up to down
  - - - gaseous elements helium, neon, argon, krypton, xenon, and radon, occupying Group 0 (18)
    - - found in group 1 of the periodic table (formerly known as group IA), are very reactive metals that do not occur freely in nature
    - - five non-metallic elements found in group 17 (salt formers)
    - - six chemical elements in group 2
    - - Metalloids are the elements found along the stair-step line that distinguishes metals from non-metals
  - - - classified by wavelength into radio wave, microwave, terahertz (or sub-millimeter) radiation, infrared, the visible region that is perceived as light, ultraviolet, X-rays and gamma rays
      - colors identify the element through radioactive decay and release of gamma rays
    - - qualitatively defined as the amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated gaseous atom to form a cation
- - - - electrons orbiting a fixed, positively charged nucleus in set, predictable paths
    - - atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus
    - - electrons surrounded by soup of positive charge
    - - round sphere with no electrons, protons, or neutrons
      - first atomic model
    - - atoms indivisible particles similar to plum pudding
  - - - PURE - cannot be separated physically
        
        ELEMENT - only one type of atom
        
        Oxygen
        
        Carbon
        
        COMPOUND - two or more types of atoms
        
        Salt (NaCl)
        
        Water (H2O)
      - MIXTURE - can be physically separated
        
        HOMOGENEOUS - solution, uniform throughout
        
        salt disolved in water
        
        HETEROGENEOUS - nonuniform
        
        chocolate chip cookie, soil
  - - - Most mass of all subatomic particles
      - no charge
      - determines isotopes
      - in neucleus
    - - least amount of mass (practically none)
      - negative charge -1
      - determine many physical phenomena
      - in electron shells outside of nucleus
    - - positive charge +1
      - slightly less mass than neutron
      - in neucleus
  - - - mass of an atom of a chemical element expressed in atomic mass units
    - - number of protons in the nucleus of an atom, which determines the chemical properties of an element and its place in the periodic table
    - - number of protons and neutrons in the atom
    - - two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical properties
    - - the time taken for the radioactivity of a specified isotope to fall to half its original value
      - equations
- - - - color
      - Molecular Weight
      - volume
      - state
      - 5 senses
    - - reactivity
      - flammibility
      - oxidation states
      - heat of combustion
      - toxicity
  - - - separate mixture into compounds
      - change of state
      - crystalize
      - change of strength/duribility
      - change in texture
    - - decomposition
      - combustion
      - change of chemical makeup
- - - - high energy/speed positron
      - radioactive decay of nucleus releases beta particles
      - one more proton one less neutron
    - - most destructive
      - photons with highest range
    - - identical to helium 4, 2 protons 2 neutrons
      - least dangerous
  - - - two light nuclei combine into one
      - releases vast amounts of energy
    - - splitting heavy unstable nucleus into 2 lighter nuclei
      - releases heat energy
      - bombarded with neutrons
- - - - orbital angular momentum quantum number - block 0 1 2 3
    - - the magnetic quantum number - -n to +n
    - - principle quantum number - energy level 1 2 3 4
    - - electron spin quantum number - m(l) +or- 1/2
  - - - quantum mechanical principle which states that two or more identical fermions (particles with half-integer spin) cannot occupy the same quantum state within a quantum system simultaneously
    - - you can never simultaneously know the exact position and the exact speed of an object
    - - ground state of an atom or ion, electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels
    - - every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin
- - - - Properties of Ionic Compounds
        
        Conductive when liquid - Ions are charged particles, but ionic compounds can only conduct electricity if their ions are free to move. Ionic compounds do not conduct electricity when they are solid - only when dissolved in water or melted.
        
        High melting and boiling points - Ionic bonds are very strong - a lot of energy is needed to break them. So ionic compounds have high melting and boiling points.
      - Properties of covalent Compounds
        
        covalent compounds softer then ionic compounds
        
        Covalent compounds don’t conduct electricity
        
        Covalent compounds don’t dissolve well in water
        
        Covalent compounds are more likely to be flammable
    - - resonance
        
        mesomerism is a way of describing delocalized electrons within certain molecules or polyatomic ions where the bonding cannot be expressed by one single Lewis structure
      - Ionic
        
        chemical bond that involves the electrostatic attraction between oppositely charged ions, and is the primary interaction occurring in ionic compounds
      - Covalent
        
        Electrons exist outside of an atom ‘s nucleus and are found in principal energy levels that contain only up to a specific number of electrons.
        
        Lewis symbols are diagrams that show the number of valence electrons of a particular element with dots that represent lone pairs.
  - - - chemical reaction in which a single compound breaks down into two or more elements or new compounds
    - - chemical reaction where an element reacts with a compound and takes the place of another element in that compound
    - - exothermic reaction in which something reacts with oxygen. The combustion of organic compounds usually takes the form organic compound + oxygen => water + carbon dioxide
    - - type of chemical reaction where two compounds react, and the positive ions (cation) and the negative ions (anion) of the two reactants switch places, forming two new compounds or products.
    - - synthesis reaction is a type of reaction in which multiple reactants combine to form a single product. Synthesis reactions release energy in the form of heat and light, so they are exothermic
- - - - k = cC dD / aA bB
- - - - mol limit x mol excess/mol limiting RATIO = mol # excess
- - - - heat lost/gained = mass x specific heat x change in temp
  - - - 333 J/g
        
        melting + freezing -
    - - 2240 J/g
        
        condense + evaporate -
- - - - P1V1=P2V2
    - - V1/T1 = V2/T2
    - - P1/T1 V = P2/T2 V
    - - P1V1/T1 = P2V2/T2
    - - pressure x volume = number of moles x (gas constant) x Temperature IN KELVIN