Chemistry
Study of the composition of matter.
Biochemistry
Study of chemical changes in living things.
Organic Chemistry
Chemistry of things containing carbon.
Matter
Anything that occupies space and has mass.
Solid
Object with a definite volume and shape (close attractive force)
Liquid
Substance with a definite volume but takes that shape of its container.
Gas
Substance with NO definite volume or shape.
Heterogeneous
If a mixture is not uniform throughout, it is called…
Intensive Properties
Properties that depend on the type of material present (boiling point, melting point, density, etc.)
Extensive Properties
Properties that depend on the amount of mater present (volume, mass, length, etc.)
Qualitative Observations
Observations dealing with the quality of a substance (the shoes are old and brown)
Quantitative Observations
Observations dealing with the quantity of data (John Bapt has 2 Ms. Ortiz)
Kilogram
SI unit for mass.
Meter
SI unit for length
Precise
Measurements that fall in the same range/area.
Accurate
Measurements falling close to the actual/true value.
4
Number of significant figures in the measurement 0.0004080 kg.
Nucleus
The Gold Foil experiment proved the existence of what?
J.J. Thompson
Who discovered the electron?
Electron
Cathode Ray Tubes led to the discovery of the…
Isotope
Atoms of the same element with different numbers of neutrons.
Albert Einstein
Who is credited with the photoelectric effect?
1
Number of s orbitals?
3
Number of p orbitals?
5
Number of d orbitals?
7
Number of f orbitals?
Speed
All electromagnetic radiation has the same what?
Released
For an electron in an atom to change from an excited state to a ground state, energy must be…..
Copper and Chromium
Which two elements have different electron notations than expected?
Ionization Energy
The energy required to remove an electron is known as what?
Increases
As we go down a group, the atomic radius….
Triple
Which type of bond is the strongest, single, double, or triple?
Ionic Compounds
Which have higher melting points, ionic or covalent (molecular) compounds?
Tetrahedral
What is the molecular geometry of CH4?
Removed
To make a bond, must energy be added or removed?
-1
What is the oxidation number of Fluorine?
N2F5
What is the formula for dinitrogen pentafluoride?
Charge of the ion
In a polyatomic ion, the sum of the oxidation numbers is equal to the…
Aluminum Fluoride
Name AlF3
Copper (II) chloride
Name CuCl2
Oxygen difluoride
Name OF2
Nitrite
Name NO2^-
6.62 g/cm^3
What is the density of 39.56 g of material whose volume is 5.98 cm^3?
6.022 x 10^23 atoms
The number of atoms in 1 mol of Silicon is?
12.0107 g
The mass of 1 mol of Carbon is?
1s^2 2s^2 2p^6 3s^2 3p^2
The electron notation for Si is…
Nonmetals
Poor conductors of heat and electricity; extremely brittle
Pure
Elements and compounds are ….. substances?
Atom
The smallest unit of matter that maintains its chemical identity.
Chemical
Any substance that has a definite composition
Mixture
A blend of any two or more kinds of matter, as long as each maintains its own unique properties.
Groups/families
The vertical columns on the Periodic Table
Periods
The horizontal columns on the Periodic Table
Precipitate
Formed when two liquids are mixed to form a solid.
100 C
Boiling point of water
0 C
Freezing point of water
Weight
The gravitational pull on a substance/object.
Hypothesis
A statement that can be tested experimentally.
1 cm^3
I mL is equal to…
Theory
Generalization that explains known facts that everyone agrees on.
4.05 g
The density of aluminum is 2.70 g/cm^3. What is the mass of a solid piece of aluminum with a volume of 1.50 cm^3?
0.071 cm^3
The density of pure diamond is 3.5 g/cm^3. What is the volume of a diamond with a mass of 0.25 g?
5.55 g/cm^3
What is the density of 37.72 g of material whose volume is 6.80 cm^3?
1060 mL
1.06 L of water is equivalent to how many mL?
0.036 g
0.035550 g rounded off to two significant figures would be…
3 m/s
When 5.7m is divided by 2s, the quotient is correctly reported as…
1.246
What is 1.245 633 501 x 10^8 rounded to four significant figures?
2.8 x 10^-9 kg/mL
When 1.92 x 10^-6 is divided by 6.8 x 10^2 mL, the quotient equals…
10^10
The result of dividing 10^7 by 10^-3 is…
2.5 x 10^-1 L
The capacity of a Florence flask is 250 mL. Its capacity in L expressed in scientific notation is….
| experimental value - actual value | over actual value x 100%
How do you calculate percent error?
420 m^3
Convert 4.2 x 10^8 cm^3 to m^3
Standard
The periodic table is a …. scale.
6.022 x 10^23
Avogadro’s number
John Dalton
Who proposed the Atomic Theory?
3
Number of isotopes in hydrogen.
1/2000th the size of an atom
Size of an electron.
Ernest Rutherford
Conducted the Gold Foil Experiment.
Protons + Neutrons
Mass number of an element.
Democrates
Discovered the atom.
Law of Conservation of Mass
Reactants = Products Law
Law of Definite Proportions
Law stating that formulas are ALWAYS written in small whole number ratios.
None
The most common form of Hydrogen has how many neutrons?
8
Carbon-14 (atomic number 6), has how many neutrons?
Average atomic mass
To determine the molar mass of an element, one must know the element’s…
1.204 x 10^23
A prospector finds 39.39 g of pure gold (atomic mass 196.9665 amu). She has how many atoms of Au?…
2.56
Determine the number of moles in 100. g of potassium. The molar mass of potassium is 39.10 g/mol.
1.88 x 10^23
Calculate the number of atoms in 10.0 g of sulfur (molar mass of 32.07 g/mol)
UV rays
Waves that are small, have high frequency, and have high energy. (Often used in tanning booths)
Schrodinger
He determined that electrons move around the nucleus in orbitals.
Pauli’s Exclusion Principle
Electrons in the same orbital must have opposite spins.
Hund’s rule
Orbitals must have one electron each before a second can be added to any of them.
Radio waves
Waves that are long, have high frequency, and emit little energy (used in broadcasting)
Quantum Theory
Theory stating that an atom has orbitals that only predict the probability of the location of the electron.
Dumbbells
The p orbitals are shaped like…
5
How many orientations can an s orbital have around the nucleus?
[Ar] 4s^1 3d^10
Noble Gas notation for copper
6.76 x 10^14 Hz
If the wavelength ( λ ) of green light is 4.44 x 10^-7 m, what is the frequency ( v )?
8.42 x 10^-19 J
How much energy is released when an electron with a wavelength of 2.37 x 10^-7 m is excited?
E = hv (h= planck’s constant)
Bohr
Created a model showing that electrons orbit the nucleus in electron orbitals.