Honors Chemistry - Midterm

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.