Chemistry test

Straight Pipet or Graduated Pipet

Volumetric Pipet

Dropper Bottle

Solution Bottle

Wash Bottle

Micro Well Plate

Beaker

Florence Flask

Volumetric Flask

Erlenmeyer Flask

Buret

Butane Burner

Scoopula

Bunsen Lighter or Stricker

Forceps

Tongs

Beaker Tongs

Funnel

Utility Clamp

Brushes

Thistle Tube

Buret Clamp

Test Tube Clamp

Test Tube Rack

Ring Stand

Iron Ring

Safety Goggles

Test Tube

Chemical Spoon

Microspatula

Crucible and Lid

Evaporating Dish

Watch Glass

Mortar and Pestle

Calorimeter

Balance

Clay Triangle

Wire Gauze

Desiccator

Graduated Cylinder

Hot Hands

Dropper Pipet

Rubber Policeman

Thermometer

Metric units for length

meter (m)

Metric units for mass

kilogram (kg)

Metric units for tempature

kelvin (k)

Define the Law of Conservation of Matter

Matter cannot be created or destroyed

Define the Law of Conservation of Energy

Energy cannot be created or destroyed

5 signs of a chemical change

• color change

• change in texture

• gas is produced (bubbling fizzing)

• change in temperature

• precipitate is formed (solid formed with 2 liquids mix)

Element

Matter composed of only one type of atom; the simplest form of matter; cannot be changed to another element except by a nuclear reaction (Ex: carbon)

Compound

Substances composed of more than one type of atom chemically joined (Ex: H2O water)

Give three examples of a physical property

density, melting point, and malleability

What is the definition of a chemical property? Give three examples of this type of property.

Chemical properties of matter describe how the substance reacts with something else.

• How does it react with acids?

• Does it react with water?

• Does it burn?

In what state of matter is a material most likely to resist being compressed (squished together)?

Solid

Gas

Has neither a definite shape nor definite volume

Liquid

Has definite volume but not definite shape

Solid

Has definite shape and definite volume

Law of Conservation of Mass

Matter cannot be created or destroyed (in ordinary chemical reactions)

Mass

Measure of quantity of matter; unit is in grams (g)

Solute

The component which “disappears;” phase changes

Solution

A uniform mixture of two or more substances which are not chemically bonded; retains original identity and properties

Solvent

Component which remains unchanged

Melting Point

Temperature which a solid changes to a liquid

Freezing Point

Temperature which a liquid changes to a solid

Boiling Point

Temperature which a liquid changes to a gas

Rules of significant figures

1. All non-zero digits are significant

2. Zeroes at beginning of numbers are not significant

3. Zeroes between non-zero digits are significant

4. Zeroes at the end of a number are only significant if a decimal is present

When naming a compound, how does the metal ion’s name change?

It doesn’t

When naming a compound, how does the non-metal ion’s name change?

Ending of ion’s name is changed to “-ide”

When do you use prefixes?

For covalent/molecular compounds only

When is a roman numeral needed in the name of a compound?

When the metal does not have a set charge

What is a period?

Horizontal row

What is a group/family?

Vertical column

What seven elements are diatomic?

Br2, I2, N2, Cl2, H2, O2, F2

What is the most electronegative element on the periodic table?

Fluorine

Anion

A negatively charged ion that gains an e-

Cation

A positively charged ion that loses an e-

Metals form _____ but nonmetals form _______

cations; anions

Where are the reactants in an equation?

left

Where are the products in an equation?

right

What does the arrow mean in an equation?

Yield

Mole Relationship in a Chemical Reaction Lab

We reacted Na2CO3 w/ excess HCl to form NaCl and H20. Discovered Na2CO3 was the limited reactant and we calculated the percent yield of NaCl. Used an evaporating dish, watch glass, a butane burner, a striker, ring stand, wire gauze, electronic balance, and pipet

Mendeleev

Arranged elements into 7 groups with similar properties

Mosely

Discovered the atomic number of all the elements known at the time

Democritus

Hypothesized matter could be subdivided again and again until it is at its smallest. Atoms

Dalton

Created first full atomic theory

1. All elements are composed of small particles called atoms

2. all atoms of the same element are identical

3. atoms of different elements are different

Rutherford

Gold foil experiment which proved the atom was mostly space and that all of the postive was located in the central nucleus

What information does the atomic number give you about an element?

Number of protons in nucleus as well as what element it is

What particles are located in the nucleus?

Protons and neutrons

Isotope

Atoms with same number of protons and different number of neutrons

Ion

An atom with a charge

Hund’s Rule

Electrons will occupy orbitals of equal energy singularly with their spins parallel until forced to pair

Aufbau’s Principle

Electrons will fill an atom from lowest to highest enegery positions

Electronmagnetic Spectrum Project

We used a spectroscope to look at 5 different light sources. We used a striker, butane burner, and burned different wooden splints that were soaked in a solution. We observed the colors of the flames.

Sharing electrons creates a what type of bond?

Covalent

A bond created by the attraction of positive and negative ions is a ____ bond

Ionic

What types of elements make a covalent bonds?

2 or more non-metals

What types of elements make ionic bonds?

Metal and non-metal

Polyatomic ion and non-metal

Metal and polyatomic ion

2 polyatomic ions

Define polar molecule

Contains a molecular dipole which is formed when bond dipoles do not cancel out

What determines the electron geometry?

Total domains