Final 9 Teoria Flashcards
Science that studies the properties of matter and its changes
Chemistry
Anything that takes up space and has mass
Matter
Capacity to do work
Energy
Physical combination of two or more substances, in which the distinct identities are retained
Mixture
Atoms of the same element with different mass but the same atomic number
Isotope
Information that indicates the location of the electrons in the atom
Quantum numbers
Notation that shows how the electrons are distributed among the atomic orbitals and energy levels
Electronic configuration
Principle that establishes that each new electron added to an atom, will enter in the available orbital with less energy
Aufbau’s Principle
Rule that says that the electrons are going to enter each orbital with a parallel spin until all orbitals are complete
Hund’s Rule
Rule that claims that electrons in the same atom cannot have the same four quantum numbers, they must have opposite spins
Paulli’s Rule
Attraction forces that hold atoms together
Chemical bond
Establishes that atoms can become stable by having eight electrons in the outer energy level
Octet rule
Type of bond that is made between metals and non-metals where one of the atoms loses electrons and the other atom gains them.
Ionic bond
Electrostatic attraction in which a hydrogen atom forms a bridge between two electronegative elements
Hydrogen bond
One half of the distance between the nuclei of identical atoms bonded together
Atomic radius
Energy required to remove one electron from a neutral atom of an element
Ionization energy
A single kind of matter with a specific composition and properties
Pure substance
Matter is the same, the original matter can be recovered, and the particles of the substance are rearranged
Physical change
Matter is different, the old matter is no longer present and cannot be reverted, and particles are broken apart forming a new substance
Chemical change
What are the subatomic particles?
The particles that make up an atom:
Electron (-)
Proton (+)
Neutron (+-)
Notations used to show now the orbitals of a sup-shell are occupied by electrons.
Diagram of orbitals
Is defined as the change in energy of a neutral atom when an electron is added to the atom to form a negative ion.
Electron affinity
Attraction force between the nuclei of non-metals and the pair of electrons that is shared between them.
Covalent bond
Examples of heterogeneous mixtures
Water and oil
Sandwich
Salad
Examples of homogeneous mixtures
Sea water
Tequila
Sand and water
Mention 3 separation methods
Magnetism
Chromatography
Distillation
Magnetism
Involves using a magnet to attract another magnetic object away from the substance it is in
Chromatography
The process of separating colored chemicals
Distillation
The substances separates with heat
States of matter
Solid
Liquid
Gas
Solid
Retains a fixed volume and shape
Little free space between particles
Rigid particles cannot move
Liquid
Assumes the shape of part of the container which it occupies.
Not easily compressible.
Flows easily.
Gas
Assumes the shape and volume of its container.
Compressible
Flows easily
Timeline representing the evolution of the atom
Dalton
Thomson
Rutherford
Chadwick
Bohr
Sommerfeld
Schrödinger Heisenberg
Families’ names of the periodic table
Alkali metals
Alkaline earthmetals
Transition metals
Earth
Carbon family
Nitrogen familiy
Oxygen family
Halogens
Inert Noble Gases
(LOS DE ABAJO DE LA PERIODIC TABLE)
Lathanide series
Actinide series
Characteristics of the metals
Good conductors
Ductile
Crystal structure
High densities
Most of them solid
Characteristics non-metals
Poor conductors
Brittle
Low densities
Low melting points
Dull appearance
Characteristics of the metalloids
Semi-conductors
Solid and may have luster
Similar properties to metals and non-metals
H
Hydrogen
Li
Lithium
Na
Sodium
K
Potassium
Rb
Rubidium
Be
Beryllium
Mg
Magnesium
Ca
Calcium
Sr
Strontium
Ba
Barrium
Radium
Ra
Boron
B
Aluminium
Al
Gallium
Ga
Carbon
C
Silicon
Si
Fluorine
F
Chlorine
Cl
Bromine
Br
Iodine
I
N
Nitrogen
P
Phosphorus
As
Arsenic
Sb
Antimony
Bi
Bismuth
O
Oxygen
S
Sulfur
Rn
Radon
Co
Cobalt
Ni
Nickel
Astatine
At
Helium
He
Neon
Ne
Argon
Ar
Krypton
Kr
Xenon
Xe
Mercury
Hg
Gold
Au
Platinum
Pt
Silver
Ag
Cu
Copper
Zn
Zinc
Pd
Palladium
Sn
Tin
Cd
Cadmium
Ti
Titanium
W
Tungsten
Cr
Chromium
Mn
Manganese
Fe
Iron
Pb
Lead
Kg -> g
*1000
G -> kg
/1000
Ml -> L
/1000
L -> ml
*1000
KG=
L
G=
ML
(S)
Solid
(g)
Gas
(l)
Liquid
(aq)
Aqueous
(triangle)
Heat
(Arrow looking up)
Escape of gas
Arrow looking down
Precipitation
(Thunder)
Electric current
Aufbau’s Principle
1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p
VALUES “s,p,d,f” for electron configuration
S= 2
P= 6
D= 10
F= 14
Values “s,p,d,f” for the quantum number “l”
S= 0
P= 1
D= 2
F= 3
Percent by mass formula
Mass of solute/mass of solution *100
Percent by volume formula
Volume of solute/volume of solution *100
Molarity formula
Moles of solute/liter of solution
Molality formula
Moles of solute/kilogram of solvent
Mole fraction formula
Moles of solute/ moles of solute + moles of solvent
Dilution formula
C1 (V1) = C2 (V2)
Units for % volume
Solute= ml
Solution= ml
% volume= %
Units for % mass
Solute= g
Solution= g
% mass= %
Units for molarity
Solute= moles
Solution= liters
Molarity= M
Units for molality
Solute= moles
Solvent= kg
Molality= m
Units for mole fraction
Solute= moles
Solvent= moles
Mole fraction= no units
Units for dilution
Volume= ml
Concentration= M
Atomic radius/ metallic character
-
+ -
Ionization energy/ electron affinity/ electronegativity
+
- +
Synthesis
A + B > AB
Decomposition
AB > A + B
Single replacement
AB + C > AC + B
Double replacement
AB + CD > AD + BC
Combustion
> CO2 + H2O
Neutralization
OH
Cation
Positive value
Anion
Negative value
Si el valor es menor que 0.4
Covalent non polar
Si el valor es mayor es mayor que 0.4 pero menor que 1.7
Covalent polar
Si el valor es mayor que 1.75
Ionic
