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Structure and Properties
N/A
43
Chemistry
12th Grade
11/08/2012

Additional Chemistry Flashcards

 


 

Cards

Term
J.J Thompson- 1897
Definition

-Matter is composed of atoms that contain electrons

-Ex: blueberry cake

cake is positive(protons)

blueberries are negative(electrons)

Term
John Dalton-1805
Definition
Matter is composed of indestructable, indivisable atoms which are identical for one element, but different for another
Term
Ernest Rutherford-1911
Definition

-An atom is composed of a very small nucleus, which contains positive charges and most of the mass of the atom. The rest of the atom is made up of mostly empty space with very small negative electrons occupying the surrounding area.

-Proved this with gold foil and gamma rays

-some rays went through, some deflected back at different angles. Therefore some sort of positive center or nuclues, and the rest of the atom is mostly empty space

Term
Rutherford and Associates
Definition
-Proton has an equal and opposite charge to and electron and is 1836 times its mass.
Term
James Chadwick-1932
Definition
-Nucleus also contained neutrallly charged particles called neutrons. This explained isotopes
Term
Isotope
Definition

-Atoms with the same number or protons, but differnt number of neutrons

-Ex: C-12, C-14

Term
Standard Atomic Notation
Definition

A: Mass Number

Z: Atomic Number

-Ex: C-12   126C

Term
Radioisotope
Definition
-An isotope that emits radioactive particles as it decays
Term
Planck's Quantum Hypothesis
Definition

-Energy could be gained or transfered in whole-number quanties

-Light it emitted in bursts, packets or quantites of energy. IT IS NOT CONTINOUS

-Photon: unit of light energy

Term
Quantum Numbers
Definition
-It is impossible to simultaneuosly know the exact position and spped of an electron.
Term
Orbital
Definition
-The region around the nucleus where there is a high probibility of finding an electron
Term
Ground State
Definition
-An electrons lowest, most stable energy level
Term
Orbit vs. Orbital
Definition

1. Well defined circular path   1. Region of space

2. 2-D motion                        2. 3-D motion

3. Max electron is 2n2           3. Max electron is 2

4. Circular shape                   4. different shapes

Term
What the quantum number do
Definition

-They describe the quantu mechanical properties of orbitals

Principle (n)

Seconday (l)

Magnetic (ml)

Spin (ms)

Term
Principle Quantum Number (n)
Definition
-The energy level the electron is located (shell)
Term
Secondary Quantum Number (l)
Definition

-Describes the shape of the orbital

0=s orbital (shpere)

1=p orbital (peanut)

2= d orbital (2 peanuts)

3=f

4=g

1=n-1

-Ex: 3n, 1=2,1,0(d,p,s)

Term

 

Magnetic Quantum Number (ml)

 

Definition

-Describes the orientation of the orbital in space relative to the other orbitals

-ml= -l to +l

-Ex: l=2 ml=-2,-1,0,1,2 (5 different orientations)

Term
Magnetic Spin (ms)
Definition

-+1/2 counterclockwise

- -1/2 colckwise

Two electrons in the same shell must be spinning oppositly of each other

Term
Pauli Exclusion Principle
Definition
Every electron in an atom will have its own set of 4 quantum numbers
Term
Hund's Rule
Definition
In a set of orbitals with the same energy level, the lowest energy configuration for an atom is the one with the max number of unpaired electrons. This means that before any 2 electrons can occupy an orbital in a subshell, other orbitals in the sam esubshell must have one electron occupying it already.
Term
Aufbau Principle
Definition
An atom is "bulit up" by the additon of electrons which fill orbiats starting at the lowest availibe energy orbital beofre filing higher energy levels
Term
Energy Level Diagrams-Anions
Definition
-Just add extra electrons
Term
Energy Level Diagrams-Cations
Definition
-Do full E.L.D, then substract amount of charge from the highest possible energy level
Term

Electron Configuration

Na

Sn+1

Definition

Na:1s2, 2s2, 2p6, 3s1

Sn+1: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10

Term

Short Hand E.C

Al

Definition
Al: [Ne] 3s2, 3p1,
Term

Anomilies

Cr, Cu

Definition

Cr:[Ar]4s1, 3d5

cu:[Ar]4s1, 3d10

-it is more stable to have half filled orbitals then orbitals with empty spaces

Term
Magnetism
Definition

Ferromagnetism: Ni, Co, Fe

Paramagnetism: weak magnetic field

Term
Polar Molecules
Definition

-Electronegatitives between 0.4 and 1.7

-If a symmetrical coumpond has polar bonds, the total compund is non polar, because each bond is beinnging pulled in equal and opposite directions

Term
Non Polar Molecules
Definition

-Electronegativites between 0 and 0.4

 

Term
Ionic Molecules
Definition

-Electronegativites 1.7+

-Usually between metals and non-metals

Term
Ionic Solids
Definition

-Metal(anions) and non-metals(cations)

-ex: NaCl

-hard, britte, high melting/boiling points

-crystal

 

Term
Metallic Solids
Definition

-Metals

-ex: Zinc/Iron

-shiny, silvery, flexible and conduct electricity/heat

-nuclei are fixed and valance electrons are mobile (electron sea)

-Electrons act as glue to hold nuclei together

-strong bonding (+nuclei and -valance electrons)

Term
Molecular Solids
Definition

-Non-metals

-ex: iodine, carbon dioxide

-low melting/boiling point, non conductors

 

Term
Covalent Netwrok Crystals
Definition

-ex: diamond and graphite

-very hard and strong, high boiling/melting points

-some can conduct electricity (graphite)

 

Term

VSEPR Theory

A= central atom

X= bonding electrons

E= unbonded electron pairs

Definition

-Valance Shell Electron Pair Repulsion Theory

-helps you to predict the shape of molecules due to their bonding and non-bonding pairs of electrons

 

Term
Linear
Definition

-AX2

-180°

Term
Trigonal Planar
Definition

-AX3

-120°

Term
Tetrahedral
Definition

-AX4

-109.5°

 

Term
Trigonal Pyramidal
Definition

-AX3E2

-Less than 109.5°

 

Term
V-Shaped/Bent
Definition

-AX2E2

-109.5°

Term
Trigonal Bypyrmadial
Definition

-AX5

90° and 120°

Term
Seesaw
Definition

-AX4E

 

Term
Octahedral
Definition

-AX6

90°

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