Semester Test Review: Unit 0 and 1

​Semester Test Review Part One

By Laura Korenek

N x 10ⁿ

​
Move the decimal behind the first non-zero to make N

Count how many places to make n

left is positive
right is negative

Scientific Notation

Multiple Choice

Convert 0.0000037 to Scientific Notation.

• .37 x 10^-7

• 3.7 x 10^-6

• 37 x 10^-5

• 370 x 10^-4

Multiple Choice

Mercury’s average distance from the sun is 57,190,000 km. What is the distance in scientific notation?

• 5719 x 10⁴

• 571.9 x 10⁵

• 57.19 x 10⁶

• 5.719 x 10⁷

Erlenmeyer Flask; hold and mix chemicals

Beaker;

Hold and mix chemicals

Lab Equipment to Know

Balance; accurately measures mass

Graduated Cylinder;
Accurately measure volume of liquids

Lab Equipment to Know

Multiple Choice

What is used to measure (but not precise), heat, and mix large amounts of liquids?

• beaker

• flask

• test tube

• graduated cylinder

Multiple Choice

What equipment allows you to measure liquid's volume and measures in milliliters?

• test tube

• beaker

• flask

• graduated cylinder

Multiple Choice

Which equipment holds, measures, and mixes liquids (not a precise measurement), and measures in milliliters?

• flask

• test tube

• beaker

• graduated cylinder

Meniscus - curved shaped of the water due to the water particles "sticking" to the sides of the glass

​

Measuring Volume

Multiple Choice

When reading the volume in a graduated cylinder, look at the ___ of the meniscus.

• top

• bottom

• It doesn't matter.

• What is a meniscus?

Multiple Choice

What is the volume?

• 23 mL

• 28 mL

• 36 mL

• 38 mL

Multiple Choice

What is the volume?

• 42 mL

• 43 mL

• 44 mL

• 45 mL

All non-zeros are always significant.

Some zeros are significant and some are not.

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Significant Figures

Multiple Choice

How many sig figs are there in the following measurement?

100.00 m

• 1

• 3

• 4

• 5

Multiple Choice

How many sig figs are there in the following measurement?

100000000 km

• 1

• 9

• 10

• 8

Multiple Choice

How many sig figs are there in the following measurement?

4004 grams

• 1

• 2

• 3

• 4

How close a group of values are to each other

Precision

How close a value is the correct or accepted value

Accuracy

Accuracy vs Precision

Multiple Choice

Which student was the most precise?

• Student A

• Student B

• Student C

• Cannot be determined

Multiple Choice

This bullseye demonstrates...

• High Accuracy & High Precision
• High Accuracy & Low Precision
• Low Accuracy & High Precision
• Low Accuracy & Low Precision

Multiple Choice

Which student is the most ACCURATE?

• A

• B

• C

can be separated

Mixture

Cannot be separated
Elements and compounds

Pure Substance

Classification of Matter

Multiple Choice

This diagram represents a _____.

• pure substance that is a compound
• mixture of elements
• pure substance that is an element
• mixture of compounds

Multiple Choice

This diagram represents a _____.

• pure substance that is a compound
• mixture of elements
• pure substance that is an element
• mixture of compounds

Lab Safety

Some Important Reminders

• always wear safety goggles

• waft when smelling chemicals

• never perform unauthorized experiments

• Clean up and dispose of chemicals appropriately

Multiple Choice

You should always wash your hands after a lab even if you wear gloves.

• true

• false

Multiple Choice

The proper technique for smelling chemicals is ______________

• keeping your nose close to the glassware
• wafting
• to sniff only a small amount
• Trick question; you never are allowed to smell chemicals in class

Multiple Choice

After completing an experiment, all wastes should be

• taken home

• tossed in the trash can

• disposed of according to your teacher's directions

• left out for someone else to clean

A more dense object would have a greater mass over a smaller volume.

mass - grams
volume - ml
density - g/ml

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Calculating Density

Multiple Choice

A bar of copper has a mass of 216g and a volume of 24 cm3. What is the density of copper?

• 9g/cm3

• 5184g/cm3

• .11g/cm3

• 322mL

Multiple Choice

Helium balloons rise on earth because

• helium is less dense than air
• helium is more dense than air
• helium is cooler than air
• helium is warmer than air

Multiple Choice

A chef fills a 50.0 mL container with 43.5 g of cooking oil. What is the density of the oil?

• 1.15 g/mL

• 0.87 g/mL

• 2,175 g/mL

• 6.5 g/mL

Subatomic Particles

Neutrons

Located in Nucleus
Positive charges
makes up part of the mass

Protons

Electrons

Located in Nucleus
Nuetral charges
makes up part of the mass

Located in electron cloud
Negative charges
makes up insignificant part of mass

Multiple Choice

Protons are

• Negative

• Positive

• No charge

• Atomic Number

Multiple Choice

Neutrons have

• Negative

• Positive

• No charge

• Atomic Number

Multiple Choice

Electrons are

• Negative

• Positive

• No charge

• Atomic Number

Multiple Choice

In the nucleus you can find the

• Protons, neutrons and electrons

• Protons and neutrons

• Protons and electrons

• Neutrons

Multiple Choice

The smallest subatomic particle

• Protons

• Neutrons

• Electrons

• Atoms

# of protons and neutrons
can vary depending on the number of neutrons

Mass number

# of protons;
identifies the element
cannot be changed.

Atomic Number

Atomic Theory

Show the element symbol;
The mass number
Atomic number
oxidation number​

Nuclear Atomic Symbol

Indicated Element name and mass number
Mass Number = Protons + Neutrons

Multiple Choice

What property determines if an atom is identified as Flourine?

• it has 10 neutrons

• it has an atomic mass of 19

• it has 9 protons

• Its element symbol is Fl.

Multiple Choice

For an atom to be electrically neutral, it must contain the same number of _____

• protons and neutrons
• neutrons and electrons
• protons and electrons
• nucleons and electrons

Multiple Choice

An element has 5 protons, 6 neutrons, and 5 electrons. What is the mass number?

• 5

• 10

• 11

• 16

Multiple Choice

An element has 5 protons, 6 neutrons, and 7 electrons. What is the charge of the atom?

• +2

• -1

• +1

• -2

Multiple Choice

An element has an atomic number of 9 and a mass of 19 amu. What is the number of protons this element has?

• 9

• 19

• 10

• 28

Multiple Choice

What gives you the identity of an element?

• Mass

• Atomic number

• Protons

• Electrons

Multiple Choice

How many Neutrons does Hydrogen have?

• 1

• 0

Isotopes

• Atoms of the same element with different Mass Numbers and therefore different numbers of Neutrons

• Protons cannot change!!!! The identify the element.

• Example; Carbon-12, Carbon-13; Carbon -14
  

Multiple Choice

Potassium-39 has how many neutrons?

• 19

• 18

• 20

• 21

Multiple Choice

Isotopes of an element have a different number of...

• Protons

• Neutrons

• Electrons

• Mass

Multiple Choice

Choose the correct hyphenated symbol for an element with 76 protons and 114 neutrons

• Osmium-114

• Osmium-76

• Osmium-190

• Osmium-190.23

Multiple Choice

Which of the following is/are conclusions based on Rutherford’s gold foil experiment?

• Atom is mostly empty space

• The nucleus is positively charged

• The atom has a small dense nucleus

• All answers are correct

Multiple Choice

Proposed that electrons move around the nucleus in specific layers, or shells.

• Bohr

• Rutherford

• Chadwick

• Thomson

Multiple Choice

According to the Plum Pudding Model, what is the structure of an atom?

• Negatively charged sphere with positively charged electrons embedded in it.

• Positively charged sphere with negatively charged electrons embedded in it

• Positively charged sphere with positively charged electrons embedded in it.

• Negatively charged sphere with negatively charged protons embedded in it.

Multiple Choice

Believed that atoms of the same element are identical to each other

• Bohr
• Rutherford
• Dalton
• Thomson

Multiple Choice

Who discovered the electron?

• J.J. Thomson

• Marie Curie

• Isaac Newton

• Albert Einstein

Multiple Choice

What contribution did John Dalton make to atomic theory? 

• He discovered that every atom was positively charged. 
• He discovered that every element consisted of one type of atom that couldn't be divided. 
• He discovered that atoms had nuclei. 
• He discovered that atoms could be divided into smaller parts. 

Electrons fill orbitals in a specific order.
Lowest Energy to Highest energy
s,p,d,f

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Electron Configuration

Multiple Choice

How many electrons can the first energy level hold?

• 1
• 2
• 8
• 0

Multiple Choice

Which electron configuration belongs to Chlorine (Cl)?

• 1s² 2s² 2p⁶ 3s² 3p⁵
• 1s² 2s² 2p⁶ 3s² 3p⁶
• 1s² 2s² 2p⁶ 3s² 3p⁷

Multiple Choice

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

• Zinc
• Copper
• Nickel
• Germanium

Use arrows to illustrate spin and location of electrons

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Orbital Diagrams

Multiple Choice

Which element is pictured?

• neon
• fluorine
• magnesium
• argon

Multiple Choice

This orbital diagram represents:  

• C
• B
• N
• O

Multiple Choice

What is incorrect about this orbital diagram?

• Both arrows in the 2p box should be pointing up
• There is nothing incorrect with this diagram
• In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
• All the arrows should be pointing up.

Since every element has a unique arrangement of electrons, it will emit a unique combination of light.

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Atomic Emission Spectra

Multiple Choice

Which has the longest wavelength?

• Orange

• Green

• Violet

• Yellow

Multiple Choice

The color of light with the LONGEST wavelength is

• violet

• green

• red

• indigo

Multiple Choice

The color of light with the HIGHEST energy is

• violet

• green

• red

• indigo

Multiple Choice

The unknown emissions spectrum belongs to the element

• Hydrogen

• Mercury

• Neon

• Sodium