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185 Cards in this Set
- Front
- Back
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Atoms are most stable if they have a filled or empty outer layer of electrons.Except for H and He What is the name of this rule? |
The octet rule |
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A filled layer contains 8 electrons |
an octet |
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Atoms that gain or lose electrons. Type of compound? |
ionic |
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atoms that share electrons. Type of compound? |
covalent |
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The outermost electrons of an atom, which are important in determining how the atom reacts chemically with other atoms. The electrons that occupy the highest energy level in an tom. Represented by the groups numbers |
Valence electrons |
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valence electrons that are mobile within a metal. What type of chemical bond is this called? |
metallic |
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______ suggested a means of keeping track of outer (or valence) electrons |
Lewis |
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Each atom wants either ___ or ____ valence electons |
8 or 0 |
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The diagram that we draw, the element symbol in the middle with a certain number of dots surrounding it depending on the amount of valence electrons that element has. |
Lewis Diagram |
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The alkali metals, or group1, has a oxidation number of |
+1 |
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The alkaline metals, or group2, has a oxidation number of |
+2 |
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group 13 has a oxidation number of |
+3 |
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group 14 has a oxidation number of |
+,- 4 |
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Group 15 has an oxidation number of |
-3 |
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Group 16 has an oxidation number of |
-2 |
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Group 17 has an oxidation number of |
-1 |
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An element that has given away or obtained electrons giving it a positive or negative charge |
ion |
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____ ion consist of two atoms |
binary |
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____ ions consist of one aton |
monatomic |
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____ ions consist of 3 or more atoms |
polyatomic |
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ionic bonding- a force of attraction between ___ charged ions |
oppositely |
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Ionic bonds occur between a _____+ ______ or ______+______ |
Metal+ Nonmetal or Cation+ Anion |
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Polyatomic always is ____ |
ionic |
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Representative unit for ionic compounds |
Formula units |
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Each ionic formula represents _____ formula unit |
one |
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KBr= ____ formula unit of potassium bromide |
1 |
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MgCl2 = ____ formula unit of magnesium chloride |
1 |
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Formula units represents the ____________ of ions in an ionic compound |
lowest whole # ratio |
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Ionic compounds are |
neutral |
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Characteristics of ionic compound- Physical state @ STP= ______. Generally _______ melting points (above 300 degrees C) Generally _____ solubility in water. ________ electrical conductivity in aqueous solutions. |
Solid, Higher, high, good. |
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Ability to dissolve |
solubility |
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dissolved in water |
aqueous |
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When metals transfer their valence electrons to nonmetals. The oppositely charged ions attract each other to form an ___ bond |
ionic |
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Metallic bonding- Metals are made up of closely packed ______ rather than neutral atoms. |
cations |
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Metallic bonding- the cations are surrounded by ____ valence e, which can ____ from one part of the metal to another |
mobile, drift |
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A metallic bond consists of the attractions of _______ valence electrons for the positively charged metal ions (cations) |
free-floating |
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Free-floating valence e, are sometimes referred to as a _______ |
sea of valence electrons |
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__ bonding |
Metallic |
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The physical properties of metals are the result of the delocalisation of the electrons involved in |
metallic bonding |
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They physical properties of _____ are, conduct heat, conduct electricity, generally high melting and boiling point, strong, malleable, ductile, metallic lustre, opaque |
solid metals |
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Can be hammered or pressed out of shape without breaking |
malleable |
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Able to be drawn into a wire |
ductile |
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reflect light |
opaque |
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The chemical bonding that results from the attraction between metal cations and the surrounding sea of electrons |
metallic bonding |
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Vacant ___ and ___ orbitals in metal's outer energy levels overlap, and allow outer electrons to move freely throughout the metal |
p and d |
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in metallic bonding valence electrons do not |
belong to any one atom |
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occurs when two nonmetal (and sometimes metalloid) atoms share one or more pairs of electrons to become stable. Molecular compounds are formed. |
Covalent bonding |
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latin- "together" |
co |
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"to be strong" |
valere |
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Some elements in nature are |
molecules |
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neutral group of atoms covalently bonding |
molecules |
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Ex. Air contains 0 molecules, 2 O atoms joined covalently |
diatomic molecule |
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All the diatomic molecules (there are 7 total) - show on periodic table |
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What is the purple and the green elements |
purple is diatomic Green is polyatomic |
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All the diatomic molecules in group17 have ____ bond |
one |
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The diatomic molecule in group 16 has __ bonds |
two |
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The diatomic molecule in group 15 has __ bonds |
3 |
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The diatomic molecule in group 1 has _ bond |
1 |
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Representative unit for covalent compounds; formed when two or more atoms bond covalently |
molecule |
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Examples of ____- water (H2O), Methane (CH4), Ammonia (NH3), Diatomic molecules, carbohydrates, fats, and proteins, and DNA (deoxyribonucleic acid) |
molecules |
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Characteristics of covalent compounds- physical state @STP = ______________, generally ______ melting points (below 300 degrees C), generally _____ solubility in water, _____ electrical conductivity in aqueous solutions |
solid, liquid, or gas, lower, lower, poor |
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Fluorine has seven valence electrons, a second atom also has seven, by sharing electrons..... bond end with ________ |
full orbitals |
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Covalent bonds can be ____ (1 shared pair), ____ (2 shared pairs), or _____ (3 shared pairs) |
single, double, or triple |
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_____ bonds can have this |
covalent bonds |
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A single covalent bond is ______ 2 valence electrons |
2 |
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____ can only form single bonds |
hydrogen |
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A single covalent bond is different from ionic bonds because they actually form _____ |
molecules |
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A single covalent bond is ______ joined |
2 specific atoms |
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A single covalent bond is in an ionic solid, _____ which atom electrons move from or to |
you can't tell |
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Water is formed with covalent bonds, by using an ______ _____ _____ |
electron dot diagram |
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Sometimes atoms share _________ pair of valence electrons |
more than one |
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Atoms share 2 pairs of electrons (4 total) |
double bond |
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Atoms share 3 pairs of electrons (6 total) |
triple bond |
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When drawing a dot diagram always put the element with the lowest _______ in the middle, always ignore hydrogen though. |
electronegativity |
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Carbon dioxide required ____ bonds, and each atom can count _______ in the bond |
2 double, all the electrons |
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carbon dioxide |
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Hydrogen only needs _ electrons to be happy |
2 |
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Be need ___ electrons to be happy |
4 |
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B needs __ electrons to be happy |
6 |
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1. Count total e-'s needed to make all atoms individually happy (add all oxidation numbers), for polyatomics add or subtract the the oxidation number after step 1. 2. Divide by 2 (this step tells how many ___ to draw) 3. Choose central atom (least electronegative) 4. Start with most _______ atom, fill in remaining valence electrons to fill atoms up |
bonds,most. This whole thing teaches how to draw Lewis structures |
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Lewis structure examples |
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As bond order increases, bond length ______, and bond energy ____ |
decreases, increases |
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When more than one valid dot diagram is possible. Consider the two ways to draw ozone. |
Resonance |
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It's _____ of both, shown by double- headed arrow. (you draw the arrow to represent resonance |
hybrid |
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Resonance is found in ______ structures |
double bond |
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_____ in Ozone. Note the different location of the _______ |
Resonance, double bond |
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___________ structure is correct in resonance, Actually a hybrid of the two. To show it, draw all possible structures, and join them with a _________ arrow |
Neither single, double-headed |
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occurs when more than one valid lewis structure can be written for particular molecule (due to position of double bond) |
resonance
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____ |
resonance |
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Note the different positions of the double bond in ____________ |
polyatomic ions |
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The double bond is in different places |
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molecules which have the same molecular formula but have different connectivities (the order they are put together) |
Structural isomers |
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structural isomers |
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Two ways to classify covalent bonds |
polar and non-polar |
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the _____ in electronegativity values between two bonded atoms determines if a bond is polar or non-polar |
difference |
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the ability of an atom to attract electrons when chemically bonded |
electronegativity |
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The father apart two elements are on the periodic table, the _____ the difference is in their elctronegativities |
greater |
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0.0-0.4 = _______ covalent |
non-polar |
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0.41-1.0 = _____ covalent |
polar |
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1.1-2.0 = _____ covalent |
polar |
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if its greater or equal to 2.0 = |
ionic |
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a covalent bond in which the valence electrons are not shared equally |
polar |
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One atom has a greater attraction for the electrons in the bond compared to the other atoms |
polar covalent bond |
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______ molecule = asymmetrical (unbalanced or uneven) |
polar |
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______ molecule= ___________ surrounding the central atom Ex: CH2Cl2 |
polar, different atoms |
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______molecule = _____ ______ of lone pairs around central atom |
polar, one or more |
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a covalent bond in which the valence electrons are shared equally, zero or very little difference in electronegativity values |
non polar covalent bond |
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_____ molecules = symmetrical= balanced.
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non polar molecules |
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non-polar molecules has: the ___ elements surrounding the central atom. ____ lone pairs (unshared electrons on the central atom) |
same,no |
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why are they all the way they are |
top left, polar because its not the same element surrounding it. Top right polar, has a lone pair of electrons. Bottom left nonpolar, has no lone pair electrons and all the elements surrounding are the same. Bottom middle nonpolar, has no lone pair electrons and the same elements surrounding, the bottom right polar, doesnt have all the same elements surrounding. |
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Polar bond tends to make ______ _____ "polar |
entire molecule |
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molecule with 2 poles called _____ like HCl |
dipole |
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effect of polar bonds on polarity of entire molecule depends on _______ _______ |
molecule shape |
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CO2 has 2 polar bonds, linear, ____ molecule |
nonpolar |
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effect of polar bonds on molecule polarity depends on ____ |
shape |
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water has 2 polar bonds- ____ shape |
bent |
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highly electronegative O pulls valence electrons away from H- ___ polar |
very |
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______ __ of water molecule |
polar bond |
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VSEPR stands for |
valence shell electron pair repulsion |
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VSEPR predicts ____ ____ of molecules |
3D shape |
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outside electrons |
valence shell |
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electrons pairs try to get as far away as possible from each other |
electron pair repulsion |
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VSEPR determines ___ ___ ___ |
angles of bonds |
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VSEPR is based on the number of pairs of valence electrons, ____ and ____ |
bonded and unbonded |
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unbonded pair of electrons is called a |
lone pair |
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three or more atoms placed at an expected bond angle of 180 degrees |
linear |
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one atom at the center and three atoms at the corners of a triangle, all in one plane. Have 120 degree angles |
trigonal planar |
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Central atom with four atoms located at the corners of a ______. The bond angles about 109.5 degrees |
tetrahedral |
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One atom at the apex and three atoms at the corners of a trigonal base |
Trigonal pyramid |
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have a non-linear shape and have an angle of about 105 degrees, 3 atoms |
bent |
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4 atoms bonded: basic shape ______, pyramid with _____ base, same shape for everything with 4 pairs |
tetrahedral, triangular |
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VSEPR for methane (a gas): ____ bonds fill all atoms. 4 pairs of electrons pushing away. The furthest they can get away is _______ |
single, 109.5 |
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Ammonia has an angle of 107 called |
pyramidal |
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____ ____ hold the solid and liquid states together. |
intermolecular forces |
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Intermolecular forces exist ____ molecules. |
between |
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Bonds exist ___ molecules |
within |
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only apply to systems that use covalent bonding within the molecules |
intermolecular forces |
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Forces of attraction between molecules. |
intermolecular forces |
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Intermolecular forces are ___ compared to covalent bonds |
weak |
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Covalent bonds are forces of attraction ___ molecules |
within |
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Think of intermolecular forces as "___" that holds molecules together |
glue |
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are attractions |
intermolecular forces |
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types of intermolecular forces |
hydrogen bonding and Van Der Waals (Dipole-Dipole and London dispersion forces) |
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Generally the STRONGEST of the intermolecular forces |
Hydrogen Bonding |
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forces that apply to polar molecules |
hydrogen bonding and dipole-dipole |
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intermolecular force for all nonpolar molecules |
London dispersion forces |
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Hydrogen bonding-______ than expected melting/bonding points. More _____ substances (liquids are "thicker" to pour). has ____ tension and ______ action |
higher, viscous, surface, capillary |
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An inward pull that minimizes the surface area of a liquid |
surface tension |
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A general term used to define the attraction of intermolecular forces between molecules. |
Van Der Waals Forces |
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There are two kinds of Van der Waals forces: weak ________ and stronger _______ |
London Dispersion Forces, and dipole-dipole |
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Molecular Solid (Van der Waals)- Within molecules __________ |
covalent bonding |
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Molecular Solid (Van der Waals)- Between molecules, ________
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intermolecular forces |
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Molecular Solid (Van der Waals)- molecules are held in play by _______
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intermolecular forces |
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Molecular Solid (Van der Waals)- properties are ______ to _____ melting point and boiling point, ____ and ________ conductive
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low to moderate, soft, non |
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The weakest intermolecular forces |
London Dispersion Forces |
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A temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles |
London Dispersion Forces |
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London Dispersion Forces are sometimes called an induced ______ _____ ______ ___ |
dipole- induced dipole attraction |
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London Dispersion Forces are the attractive forces that cause ____ _____to condense to liquids and to freeze into solids when the temperature is lowered sufficiently |
nonpolar substances |
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The attractive forces between the positive end of one polar molecule and the negative end of another polar molecule |
Dipole-Dipole forces |
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are much weaker than ionic or covalent bonds and have a significant effect only when the molecules involved are close together (touching or almost touching) |
dipole-dipole forces |
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dipole-dipole forces |
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london dispersion forces |
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THE MOST IMPORTANT DIPOLE DIPOLE FORCE |
Hydrogen Bonding |
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Occurs between molecules with a H attracted to a molecule with either O,N,or F (the three most electronegative elements on the periodic table) |
Hydrogen Bonding |
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Hydrogen bonding occurs between molecules with a __ attracted to a molecule with either ___, ____, or _____ (the three most electronegative elemetents on the periodic table) |
H, O, N, F |
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_______ are the strongest type of intermolecular force |
H-bonds |
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elements that an _____ would touch to be ____ Bonding |
H, hydrogen |
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The hydrogen bonding in water explains its ____ ___ ___ |
high surface tension |
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an attractive force that pulls down on the particles at the surface of a liquid. In water, the attractive force responsible is ____ ___ |
surface tension. hydrogen bonding |
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_______ |
surface tension
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The hydrogen bonding in water also explains its relatively ____, considering that is is a small molecule. Remember, the H-bonds are like glue that holds the water molecules together as a liquid, so you have to head it a lot before it will change to a gas. Molar mass( or size) definintely affets boiling point, but so do intermolecular forces. |
high boiling point |
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If a liquid has strong intermolecular forces it will have a ___ boiling point, it will evaporate _____ it will have a ____ surface tension |
high, slowly, high |
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If a liquid has weak intermolecular forces it will have a _____ boiling point, it will evaporate __________, it will have a ____ surface tension |
low, easily/quickly, low |
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polyatomic is mostly |
anions |
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metal is a |
cation |
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non metal is a |
anion |
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anions doesn't have |
romal numerals |
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atoms covalently bonded are called |
molecules |
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lone pairs are more ___ than bonded pairs |
repulsive |
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Any element in group 17 can only form ___bond |
one |
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LOOK AT NOTEBOOK FOR THING GLUED IN AND LOOK AT ALL THE WARM EXAMPLES OF ALL THE DIAGRAMs |
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much less than 1+ or 1- in ionic bond |
partial charges |
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What is this |
partial charges |
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look at khan academy video |
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