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| Anything that takes up space and has mass |
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| Substance that cannot be broken down into other substabces by chem. reactions |
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| Substance consisting of 2 or more diff. elements combined in a fixed ratio |
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| Elements that make up 96% of living matter (4) |
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| Other elements that make up the other 4% of organisms (4) |
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| Required by organisms in small amts. |
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| Iodine- essential for production of thyroid hormones |
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| Form dense core (atomic nucleus) for the atom (2) |
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| Form a cloud around the nucleus |
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| Mass of neutrons and protons |
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| 1.7 x 10 (-24) g or 1 dalton |
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| 1/2000 of a proton or neutron |
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| Number of protons in an atom |
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| How the atomic number is written |
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| Written as a subscript to left of the symbol |
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| Sum of protons and neutrons |
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| How the mass number is written |
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| Superscript to the left of the symbol |
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| Different atomic forms of the same element that have more neutrons and have a greater mass but all share the same number of protons |
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1. C-12 - most common, 99%
2. C-13 1%
3. C-14- very rare |
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| The nucleus decays spontaneously thus giving off particles and E. |
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| Subatomic particle involved in chem. reactions |
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Definition
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| E. matter possesses b/c of location/structure |
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| Diff. states of potential E. that electrons have in an atom |
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| Number of electrons in valence shell |
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| Prop. of atoms with completed valence shells |
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| Unreactive/inert and will not readily interact with other atoms it encounters |
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| 3D space where an electron is found 90% of the time |
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1. 2s orbital
2. 3 2p orbitals |
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| Basis of reactivity of atoms |
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Definition
| Presence of unpaired electrons in 1 or more orbitals of the valence shell |
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| Sharing of a pair of valence electrons by 2 atoms |
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| 2 or more atoms held together by covalent bonds |
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1.Sharing of an electron
2.Represented by a line drawn down between 2 symbols |
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1.number of covalent bonds an atom can form
2.Called the valence
3. equal to the nnumber of unpaired valence electrons |
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| Main component of natural gas |
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| Electronegativity's effect on atoms (2) |
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Definition
1. The more electronegative an atom is, the stronger it's pull on shared electrons.
2. 2 atoms of the same element have the same electronegative pull on each other. |
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1. 1 atom is bonded to a more electronegative atom
2. Electrons aren't shared equally |
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| Basic properties of a water molecule(3) |
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Definition
1. Oxygen is more elctronegative than H
2. Electrons spend more time near the Oxygen atom
3. Unequal sharing of electrons cause the Oxygen atom to have a slight negative charge and the hydrogen atom has a slight postive charge. |
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1.Extreme electronegative cases where 1 atom strips another of its electrons completely
2. When 2 ions of different charges come together |
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| When sodium encounters chlorine |
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| Ionic bonding of sodium and chlorine (2) |
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Definition
1. The valence electrons of sodium is transferred to chlorine
2. Atoms end up with completed valence shells |
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| How cations and anions interact with each other |
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1. natural state of ionic compounds and salts
2. Arranged in a 3-D lattice |
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| Partial negative charge of an atom |
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| Partial postive charge of an atom |
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| Formation of hydrogen bonds |
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Definition
| Forms whenever hydrogen covalently bonds to one electronegative atom is also attracted to another electronegative atom |
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| Van der waals interactions |
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Definition
| whenever electrons randomly accumulate in one particular area of space creating "hot spots" of negatively and positively charged areas that enable atoms to stick together |
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| 4 new hybrid orbitals formed whenever atoms have valence electrons in both s and p orbitals |
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| determines how molecules recognize and respond to each other with specificty |
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| Example of how molecular shape influences interactions between molecules |
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Definition
1. for pain control, endorphins bond to specific molecules (receptors) on brain cells producing euphoria and relieving pain
2. Molecules with similar shape (heroin and opiate) have similar effects and will mimic the endorphinsby binding to the receptors in the brain |
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| making and breaking of chemical bonds leading to changes in the composition of matter |
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| True or false: Most chemical reactions are reversible |
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1. point at which reactants offset one another exactly
2. Concentrations have been stabilized at a particular ratio not that they are equal in concentration |
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