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| theorized that matter is composed of small particles |
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| assigned the concepts of positive and negative and to electric charges |
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proposed the atomic theory:
1.all matter is composed of atoms
2. all atoms of a GIVEN ELEMENT are identical
3. compounds are made of different atoms which are combined in small whole number
4. in chemical reactions atoms are rearranged but not created or destoryed |
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| isolated radium and polonium and discovered radioactivity |
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NAME THAT MAN:
J.J. Thompson |
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Definition
| discovered the electron, concluded that it has mass |
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-discovered the proton
-Defined the nucleus of the atom as a dense central core with a positive charge |
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Definition
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| What did Rutherford discover in his famous alpha-particle scattering experiment? |
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-nucleus is the densest part of the atom
-what was in them was a positive charge |
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Definition
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Definition
| mass of g in 1 mol of an element |
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| what is an atomic mass unit? |
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Definition
| 1/12 the mass of an atom that has 6 protons and neutrons |
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| why are protons and neutrons close to 1u? |
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Definition
| helps to approximate the mass of an atom |
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What does all of this stuff mean?
A\/
Z/\ |
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Definition
Atomic mass ELE
Atomic # MENT |
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Definition
| found charge of electron to determine mass |
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| which is bigger: protons, neutrons, or electrons? |
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| three kinds of radiation? |
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Definition
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| the distance between two successive wave crests |
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| number of wave cycles per unit time |
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| ELECTROMAGNETIC RADIATION |
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Definition
| radio waves, radar, microwaves, infrared, visible light, UV, X-rays, gamma rays |
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| the frequencies of light emitted by an element |
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| the series of visible lines in the emission spectra of an element. AKA the emission spectra |
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| the pattern of colored lines formed when light from excited atoms in the gaseous state is passed through a ______??? |
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| What is plank's constant? |
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Definition
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| v stands for what, c stands for what, h stands for WHAT, while lambda stands for.... |
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Definition
frequency
speed of light
plank's constant
wavelength |
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Definition
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| DEFINE: PHOTOELECTRIC EFFECT |
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Definition
| ejection of electrons when light strikes the surface of a metal |
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| Experiments with photoelectric cells show that electrons are ejected from the surface ONLY if ________ |
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Definition
| the frequency of the light if high enough |
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| Explain photoelectric cells |
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Definition
| when light strikes the cathode of the cell, electrons are ejected from the cathode surface and move to a positively charged anode |
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| the greater number of ____, the greater the number of photons with this energy that strike the suraface |
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Definition
| photons with needed energy to remove photon w/ atom |
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Definition
| Electrons are arranged around atomic nuclei like planets around the sun |
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Definition
Electrons occupy areas around atomic nuclei like clouds
AKA cloud model |
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| Define: ELECTRON STRUCTURE |
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Definition
| Electrons are arranged around the nucleus in energy levels, sub-levels and orbitals |
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| Define: Energy levels/sub levels |
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Definition
| The distance from the nucleus to an electron is found |
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| The space where there is a high probability the electron occupies |
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| How are main levels identified? |
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Definition
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| How does emission spectra give evidence for energy sub-levels? |
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Definition
| Big gaps in emission spectra lines indicate the distance between main energy levels; small gaps indicate the distance between sub-levels. |
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| How are sub levels identified? |
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Definition
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| How are orbitals identified? |
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Definition
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| How are spins identified? |
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Definition
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| Define: the aufbao principle |
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Definition
| electrons occupy the orbitals of lowest energy first |
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Term
| The pauli exclusion principle |
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Definition
| an orbital can hold a maximum of 2 electrons, and they must have opposite spins....NO 2 ELECTRONS CAN HAVE THE SAME SET OF QUANTUM #S |
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Definition
| One electron enters each orbital of that sub-level contain 1 electron with the same spin direction |
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| What is the Heisenberg Uncertainty Principle? |
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Definition
The position and energy of velocity of an electron cannot be measured at the same time...
a maximum of 2 electrons can be held in any orbitals.
Electrons fill energy levels as atomic number increases generally by filling the lowest first.
Valence electrons of the main group elements occupy the S and P sub-levels of the outermost energy levels.
The position of any element on the periodic table shows which sub-level, S, P, D, or F the valence electrons occupy.
The periodic table not only reflects electron structure according to the number of valence electrons, main groups 1, 2, - valence electrons in S sub-level, groups 13-18 valence electrons in S and P sub-levels. |
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Definition
N
Main level or quantum shell
(1,2,3,4,5, etc) |
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Definition
l
sublevel/subshell (s->0, p->1, d->2, f->3) |
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Term
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Definition
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| The # of possible orbitals in a sublevel is given by the formula... |
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Definition
| (2L+1), where 1= the sublevel or subshell # 0, 1,2, or 3 |
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Definition
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| Electrons in the outer energy levels of atoms which take part in chemical reactions |
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On the periodic table, does ATOMIC SIZE increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
increase
The number of energy levels increases as you move down a group as the number of electrons increases. Each subsequent energy level is further from the nucleus than the last.
decrease
The concentration of more protons in the nucleus creates a "higher effective nuclear charge." In other words, there is a stronger force of attraction pulling the electrons closer to the nucleus resulting in a smaller atomic radius. |
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Term
On the periodic table, does IONIZATION ENERGY increase or decrease...
going down the periodic table?
going across the periodic table?
Why? |
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Definition
decrease
Electrons are further from the nucleus and thus easier to remove the outermost one.
increase
As you move across a period, the atomic radius decreases, that is, the atom is smaller. The outer electrons are closer to the nucleus and more strongly attracted to the center. Therefore, it becomes more difficult to remove the outermost electron. |
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| Define: ionization energy |
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Definition
| electron's ability to pull electrons off of another atom |
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| define: electronegativity |
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Definition
| atom's ability to hold onto its electrons |
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Term
On the periodic table, does IONIC SIZE increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
| ionic size increases across the periodic table |
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Term
On the periodic table, does ELECTRONEGATIVITY increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
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Term
On the periodic table, does NUCLEAR CHARGE increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
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Term
On the periodic table, does SHIELDING increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
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Term
| When electrons are added to an atom, does it become more or less metallic? |
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Definition
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| Why must orbitals have different shapes? |
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Definition
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Name the shapes of orbitals in the
s
p
d
f
orbital |
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Definition
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| How many orbitals are in the p level? How are they positioned? |
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Definition
3x,3y,3z (so...3)
they are all positioned in different coordinate planes |
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Term
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Definition
| total charge of all the protons in the nucleus. It has the same value as the atomic number. |
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•The shielding effect describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell.
•Shielding electrons are the electrons in the energy levels between the nucleus and the valence electrons. They are called "shielding" electrons because they "shield" the valence electrons from the force of attraction exerted by the positive charge in the nucleus. |
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| Why are anions larger than their respective atoms? |
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Definition
| electrostatic repulsion, also protons cannot pull extra electrons as tightly towards the nucleus |
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| Metals tend to ____ electrons to acquire stable energy levels, while non-metals tend to ___ electrons to do so |
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Definition
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| Name: the electron pairs around atoms which are not involved in bonding |
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Definition
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| what is the rule that says atoms like 8 electrons around them? |
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Definition
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| name: electron pairs around atoms which are not involved in bonding |
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Definition
| lone pairs or non-bonding pairs |
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Definition
-different atoms
-same # of valence electrons
-same Lewis structures |
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| name: the situation resulting when more than 1 electron structure can represent a molecule or ion |
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Definition
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| define: the ability of an atom to hold its electrons |
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Definition
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a covalent bond between 2 atoms tends to shift towards the atom with...
what does this do? |
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Definition
the greater electronegativity
creates polarization |
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Term
| When molecules are THIS range in bond length, they are nonpolar covalent |
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Definition
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| To determine the polarity of a non-symmetrical molecule, what must one do? |
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Definition
1. determine the polarity of each bond in the molecule
2. eliminate all bonds which cancel
3. Remaining bonds will determine molecular polarity |
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Term
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Definition
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| What does VSEPR stand for? What does it mean? |
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Definition
Valence Structure Electron-Pair Repulsion [Theory]
states that because electron pairs repel, molecules adjust their shapes so that the valence electron pairs are as far apart as possible |
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| What are the possible electron geometry shapes? |
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Definition
-linear (180)
-trigonal planar (120)
-tetrahedral (109.5)
-trigonal bipyramidal (120/90) |
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Term
| electron pair geometry is... |
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Definition
| the geometry taken up by ALL valence electron pairs in the central atom |
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Term
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Definition
| the arrangement in space of the central atom, and the atoms directly attached to it |
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| Lone pairs of electrons on the central atoms occupy... |
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Definition
| spatial positions even though their locations are not included in the verbal description of the shape of the molecule or ion |
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| Anything beyond the WHAT period can be hypervalent, and anything below WHAT period can be hypovalent? |
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Definition
3-hypervalent
2-hypovalent |
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| WHAT DETERMINES MOLECULAR GEOMETRY? |
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Definition
| ELECTRON PAIR GEOMETRY!!! |
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| In terms of resonance structure, what is going on in reality? |
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Definition
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| Do bond and lone electron pairs in valence shells repel or attract one another? |
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Definition
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| The strength of repulsion between electrons are strongest when what and what are bonded? |
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Definition
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| The top pole of a molecule is called the ___ position |
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Definition
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| The side pole of a molecule is called the ___ position |
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Definition
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Term
| 5 bonds and no valence electrons= |
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Definition
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| 4 bonds and 1 lone pair = |
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Definition
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| 3 bonds and 1 lone pair = |
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Definition
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| 2 bonds and 3 lone pairs = |
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Definition
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| six bonds and no lone pairs = |
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Definition
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| 5 bonds and 1 lone pair = |
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Definition
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V/F: Mult. bonds do not affect the overall molecular shape...
Why/not? |
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Definition
Verum
e- pairs in same region occupy same nuclei/region of space |
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Term
How do you calculate the formal charge of an atom?
Bond length? |
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Definition
group # of atom-dots &dashes
----
dashes/legs |
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| What is pure covalent bonding? |
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Definition
| atoms share e- pairs equally (similar atoms) |
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Term
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Definition
| atoms share e- bonds unequally |
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| Why are certain (polar) atoms more positive/negative? |
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Definition
| differing ionization energies mean that some atoms cannot hold on to their electrons as well, and this means that electrons are attracted to certain atoms more than others |
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Term
| Define: electronegativity |
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Definition
| ability of an atom to attract electrons to itself |
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| When the electron pair geometry is tetrahedral, what are the three possible molecular shapes? (and the degrees of their angles) |
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Definition
-tetrahedral:109.5
-trigonal-pyramidal:107.5
-bent:104.5 |
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| 4 bond pairs and 2 lone pairs = |
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Definition
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| When the electron-pair geometry is a trigonal bipyramid, what are the possible molecular shapes? |
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Definition
-trigonal bipyramid
-seesaw
-t-shaped
-linear |
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| When the electron-pair geometry is an octahedron, what are the possible molecular shapes? |
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Definition
-octahedron
-square pyramidal
-square-planar |
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| What are the angle measurements for an octahedron? |
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Definition
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| When molecules are THIS range in bond length, they are moderately polar covalent |
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Definition
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| When atoms are more polar, what happens to bond length? |
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Definition
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Term
| Molecules that are symmetrical are ___ |
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Definition
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| Electronegativity increases... |
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Definition
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Term
| When molecules are THIS range in bond length, they are very polar covalent |
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Definition
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Term
| When molecules are THIS range in bond length, they are ionic |
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Definition
| greater than or equal to 2 |
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