CHEM Midterm: Chemistry Period Elements, Chemistry Unit 1, Chemistry Unit 4 Test, Chemistry Unit 5&6, CHEM Significant Figures, Chem Ch 3&10

Which of the following choices has the greatest number of significant figures? 5.050 g 51.0 g 50.050 g 505000 g

50.050 g

How many protons are in atoms of iodine?

53

If an atom contains 45 protons and has a mass number of 102, how many neutrons does it contain?

57

How many significant figures are there in each of the following data? 23,486.5 41.200 0.0085 30.61

6 5 2 4

Find the mass, in grams, of 1.40x10^23 molecules of N2

6.51 g

Find how many centimeters are in 6.51 miles using dimensional analysis (1 mile = 5280 feet, 1 ft = 12 in, 1 in = 2.54 cm)

6.51m (5280 ft/1 m)(12 in/1 ft)(2.54cm/1 in) 6.51 x 5280 x 12 x 2.54 = 1047682.944 = 1.05 x 10^6

What is the correct scientific notation for 0.0006903?

6.903 x 10^-4

What is the volume of an object with a density of 7.73 /cm3 and a mass of .40x10^2g

69.9 cm^3

7100 cm = ____ m

71

Write the following numbers in scientific notation: .000882 .00000059 .00004

8.82 x 10^-4 5.9 x 10^-7 4 x 10^-5

When are zeros significant and when are they place holders?

80.00 has 4 sig figs 41,200 has 3 sig figs

How many total atoms are in one molecule of magnesium nitrate, Mg(NO3)2

9

What is the charge of a potassium ion? +1 +2 -1 -2

A.) +1

Approximately how many molecules are in 11 grams of carbon dioxide gas? The atomic masses of carbon and oxygen are 12.0 and 16.0, respectively: 1.5 x 10^23 3.0 x 10^23 6.0 x 10^23 2.4 x 10^23

A.) 1.5 x 10^23

What is the volume of a salt crystal measuring 2.44x10^-2 m by 1.4x10^-3 m by 8.4x10^-3 m? - 2.9x10^-7 - 2.9x10^-6 - 2.9x10^-5 - 2.9x10^-4

A.) 2.9x10^-7

What is the quantity 7896 millimeters expressed in meters? - 7.896 m - 78.96 m - 789.6 m - 789600 m

A.) 7.896 m

All of the following are equal to Avogadro's number EXCEPT: - the number of atoms of bromine in 1 mol Br2 - the number of atoms of gold in 1 mol Au - the number of molecules of nitrogen in 1 mol N2 - the number of molecules of carbon monoxide in 1 mol CO

A.) the number of atoms of bromine in 1 mol Br2

A burning candle is an example of:

A combustion reaction

When are numbers exact, and when do they contain uncertainty?

A measurement is exact when there are no zeros to the right of the decimal place. Measurements are uncertain because they are estimations and have margins of error.

Atoms are incredibly small; there are an uncountable number of atoms in visible matter. What unit is used to count the number of particles in a substance? Meters Moles Megabytes Dozens

B.) Moles

Three different people weigh a standard mass of 2.00 g on the same balance. Each person obtains a reading of 7.32 g for the mass of the standard. These results imply that the balance that was used is: - accurate - precise - accurate and precise - neither accurate nor precise

B.) precise

How many significant figures are in the measurement 40,500 mg? - two - three - four - five

B.) three

Ba

Barium

Be

Beryllium

B

Boron

Explain the difference between a gaseous element and a gaseous compound

Both a gaseous element and a gaseous compound are spread out and not densely packed, but a gaseous element is singular atoms of one element moving quickly, while a gaseous compound is compounds of two or more elements bonded together are moving around quickly

Cu

Copper

Which of the following elements requires the least amount of energy to ionize?

Na

prefix, power, abbreviation 1 billionth

Nano 10 ^-9 n

Precision

Narrowness of range of measurements

Who is credited with the discovery of the model with electron energy levels?

Neil's Bohr

Ne

Neon

Sr

Strontium

Na

Sodium

S

Sulfer

Mass

The quantity of matter an object contains

Which electron transition results in the emission of energy? a.) 3p to 3s b.) 3p to 4p c.) 2s to 2p d.) 1s to 2s

a

Which has the greatest energy? a.) ultraviolet radiation b.) infrared radiation c.) green light d.) blue light

a

Which is the ground state electron configuration of a magnesium atom? a.) 1s2s2p3s b.) 1s2s3s3p c.) 1s2s3s2p d.) 1s2s2p3s

a

What is a combustion reaction?

a chemical change in which an element or compound reacts with oxygen, often producing energy in the form of heat and light

A burning candle is an example of...

a combustion reaction

Define mass

a measure of the amount of matter that an object contains

Define volume

a measure of the space occupied by a sample of matter

Define heterogeneous mixtures

a mixture that is not uniform in composition; components are not evenly distributed throughout the mixture

Define homogeneous mixtures

a mixture that is uniform in composition; components are evenly distributed and not easily distinguished

Define distillation

a process used to separate dissolved solids from a liquid, which is boiled to produce a vapor that is then condensed into a liquid

Why is a hypothesis?

a proposed explanation for an observation based on limited information

What are physical properties?

a quality or condition of a substance that can be observed or measured without changing the substance's composition

Define precipitate

a solid that forms and settles out of a liquid mixture

Define compound

a substance that contains two or more elements chemically combined in a fixed proportion

All of the following are examples of electromagnetic radiation EXCEPT __. microwaves visible light cosmic rays infrared radiation

cosmic rays

prefix, power, abbreviation billion

giga 10 ^9 G

Group 2 elements are (metals/nonmetals) that are (stable/reactive) as elements. When they react, they (gain/lose) (electrons/protons) to become (atoms/ions) with a _____ charge

metals, reactive, lose electrons, ions +2

The energy of an atom in the excited state is ________ than its energy in the ground state

more

Group 17 elements are (metals/nonmetals) that are (stable/reactive) as elements. When they react, they (gain/lose) (electrons/protons) to become (atoms/ions) with a _____ charge

nonmetals, reactive, gain electrons, ions -1

Group 18 elements are (metals/nonmetals) that are (stable/reactive) as elements.

nonmetals, stable

What are chemical properties?

the ability of a substance to undergo a chemical change

What is accuracy?

the closeness of data to the accepted value

Isotopes of an element differ in...

the number of neutrons in the nucleus

Which family of elements tend to form -2 ions when they react with metals to form compounds

the oxygen group

What is precision?

the reproducibility of a set of data

Compares to a 2p orbital, a 3p orbital can contain ______ electrons

the same number of

Define element

the simplest form of matter that has a unique set of properties; an element cannot be broken down into simpler substances by chemical means

What is chemistry?

the study of the composition of matter and the changes that matter undergoes

An estimate is only as good as...

the tool and the method used

What is an independent variable?

the variable that the scientist controls and changes to test what effect the independent variable has on the dependent variable

What is a dependent variable?

the variable that the scientist measures and doesn't control

Which of the following is a pure substance? diet coke air CO2 a plant cell

C.) CO2

What are the elements that need to be in pairs (diatomic elements)

"The 7 that make a 7 and hydrogen" Hydrogen Nitrogen Oxygen Fluorine Chlorine Bromine Iodine Astatine

Calculate the atomic mass of an unknown element, given that 99% of its atoms have a mass number of -238, and the other atoms have a mass number of 235. Show your work.

(99 x 238) + (1 x 235)

electromagnetic spectrum high to low energy

gamma ray, xray, ultraviolet, vivible, infrared, microwave, radio

To be in proper scientific notation the number must be written with:

- a number between 1 & 10 - multiply by a power of 10

The Group 16 nonmetals form ions with a ____ charge

-2

Round off the measurement of 0.0030955 m to three signifigant figures.

.00310 m

What is the density of a 12.5 mL aqueous solution that has a mass of 10.081 g?

.8

Standard temperature and pressure

0 degrees C and 1 atm

Which of the following measurements contains three significant figures? 0.01 g 0.010 g 0.01010 g 0.0100 g

0.0100 g (trailing zeros to the right are significant if there is a decimal point)

A student calculated a length measurement to be 0.06748 cm. What is this length rounded to three significant digits? 0.0674 cm 0.07 cm 0.0675 cm 0.068 cm

0.0675 cm

1 L = ____ dm^3

1

1 mL = ___ cm^3

1

Picture two hydrogen atoms. The electron in the first hydrogen atom is in the n=1 level. The electron in the second hydrogen atom is in the n=4 level. - Which atom has the ground state electron configuration? - Which atom can emit electromagnetic radiation - In which atom is the electron in a larger orbital? - Which atom has a lower energy?

1 4 4 1

What is the most stable arrangement of 4 electrons in the "p" sublevel?

1 pair and 2 unpaired

Calculate the wavelength of light with a frequency of 7.5 x 1013s-1. The speed of light is 3.0 x 108m/s. 4.0 x 10 -6m 2.3 x 10 21m 2.5 x 10 5m 3.3 x 10 -9m

4.0 x 10 -6m

One mole is equal to 6.02 x 10^23. How many atoms are in 0.25 mole of lead (Pb).

1.50 x 10^23

1 meter = ___ cm

100

1 L = ____ mL

1000

1 kg = ____ g

1000

How man protons, neutrons and elections do 27 Al 3+ particles have?

13 protons 10 electrons 14 neutrons

Using the rules for significant figures, the sum of 12.04 liters and 1.091 liters should be expressed as ____ 13.10 liters 13.131 liters 13.1 liters 13.13 liters

13.13 liters

How many atoms of sulfer are in 8 molecules of carbon disulfide?

16

What is the correct electron configuration for atoms of arsenic in the ground state 1s22s22p63s23p5 1s22s22p63s23p3 1s22s22p63s23p64s24p3 1s22s22p63s23p63d104s24p3

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3

What is the maximum number of electrons that can go into the following sublevels?: - 2s - 5s - 3p - 4d - 4f - 4p - 5d - 5f

2 2 6 10 14 6 10 14

What is the percent by mass of hydrogen in aspirin C9H8O4

4.44%

Which orbital that follows has the most energy associated with it? 4d 4p 5s 4s

4d

How many neutrons are in atoms of 9Be?

5

Calculate the energy associated with light that has a frequency of 4.3 x 1014s-1. Planck's constant, h = 6.63 x 10-34J s. 28.5 J 6.5 x 1047 J 2.8 x 10-19 J 1.5 x 10-48 J

2.8 x 10-19 J

How many electrons are in a chromium (III) ion, 52Cr 3+? 21 52 55 27 24

21

How many electrons are in a chromium ion, 52 Cr 3+

21

29 kg = ____ g

29000

How many representative particles are in 1.45 g of a molecular compound with a molar mass of 237 g?

3.68 x 10^21 molecules

Find how many minutes a woman has lived by her 35th birthday using dimensional analysis

35 y (360d/1y)(24h/1d)(60m/1h) 35 x 360 x 24 x 60 = 1839600 = 1.84 x 10^7

How many protons are in atoms of an element with atomic number 39 and mass number 89?

39

How many protons are in atoms of an element with atomic number 39 and mass number 89? 39 50 51 89 128

39

What is the mass number of an ion of K+, with 18 electrons, 19 protons, and 20 neutrons?

39

What is the mass number of an ion of K+, with 18 electrons, 19 protons, and 20 neutrons? 39 38 37 36

39

How many orbitals total are in the 4th energy level? 10 4 16 32

4

How many unpaired electrons are there in iron atoms?

4

The molar volume of a gas at STP occupies: - 22.4 L - 0 degrees C - 1 kilopascal - 12 grams

A

When the component gases of air are mixed together in the same proportions are found in air, no change in energy is noticed. What does this observation indicate?

Air is a mixture

Which of the following particles have a charge?: Atoms neutrons protons electrons anions cation

All except atoms and neutrons

Al

Aluminum

Define ion

An atom with net electric charge due to the loss or gain of one or more electrons (but it's still the same element because there's still the same number of protons)

Representative Particle

An atom, an ion, or a molecule, depending upon the way a substance commonly exists

What is the difference between an atomic element and a molecular element

An atomic element would be an element whose atoms roam independently, and a molecular element is an element whose atoms are bonded together in bonds of two or more atoms (ex: Ne is an atomic element but O2 is a molecular element)

Ar

Argon

As

Arsenic

How many moles of tungsten atoms are in 4.8x10^25 atoms of tungsten? - 8.0x10^2 moles - 8.0x10^1 moles - 1.3x10^-1 moles - 1.3x10^-2 moles

B.) 8.0x10^1 moles

Which lab equipment would be used to accurately measure 26.0 mL of distilled water? beaker erlenmeyer flash graduated cylinder electronic balance

C.) graduated cylinder

Name two ways the isotopes of an element differ.

Atomic mass and number of neutrons

What part of Dalton's Atomic Theory are no longer accepted today?

Atoms cannot be subdivided, created, or destroyed; we now know that atoms of made of of particles called protons, neutrons, and electrons

How is an average mass different from a weighted mass?

Average is all of the masses are weighted the same and one isn't more important than another. Weighted mass is when certain masses carry more weight/are more abundant than other masses.

What is the percent by mass of carbon in acetone, C3H6O? - 20.7% - 62.1% - 1.61% - 30%

B

What is true about the molar mass of chorine gas? - The molar mass is 35.5g - The molar mass is 71.0g - The molar mass is equal to the mass of one mole of chlorine atoms - None of the above

B

Which of the following sets of empirical formula, molar mass, and molecular formula is correct? - CH, 78 g, C13H13 - CH4N, 90 g, C3H12N3 - CaO. 56 g, Ca2O2 - C3H8O, 120 g, C3H8O2

B

Which of the following units is the largest? - 1 cg - 1 dg - 1 mg - 1 ng

B.) 1 dg

How many moles of water are in 1,000 grams? 18 55.5 180 1000 18,000

B.) 55.5

Br

Bromine

What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight? - C3HN2 - C4H14N2 - C2H8N - CH4N7

C

What is the molar mass of (NH4)2CO3? - 144g - 138g - 96g - 78g

C

What is the number of moles in 432g Ba(NO3)2? - .237 mol - .605 mol - 1.65 mol - 3.66 mol

C

Which of the following measurements contains two signifigant figures? - 0.00400 L - 0.00404 L - 0.00044 L - 0.00440 L

C.) 0.00044 L

What is the mass of one mole of Ca(NO3)2? 82 g/mol 102 g/mol 164 g/mol 204 g/mol

C.) 164 g/mol

What is the mass in grams of one mole of the element containing 12 protons?: 6 12.011 24.31 36

C.) 24.31

The smallest particle of an element is: a chemical formula a mixture an atom a compound

C.) An atom

What are the products of a combustion reaction?

CO2, H2O, and energy

Which particle has the same electron configuration as an atom of Argon?

Ca2+

Ca

Calcium

C

Carbon

prefix, power, abbreviation 1 hundredth

Centi 10 ^ -2

What are the indications or signs of a chemical change?

Change in color, formation of precipitate (a new solid substance that settles out of a solution), the production and release of gas, light given off, change in temperature

Cl

Chlorine

Cr

Chromium

Accuracy

Closeness to true value

Co

Cobalt

Which of the following compounds has the lowest percent gold content by weight? - AuOH - Au(OH)3 - AuCl3 - AuI3

D

The quantity 44 liters expressed in cubic meters is____? - 0.000044m^3 - 440000m^3 - .44m^3 - 0.044m^3

D. 0.044m^3

How many molecules are in 2.10 mol CO2? - 2.53 x 10^24 - 3.79 x 10^24 - 3.49 x 10^-24 - 1.26 x 10^24

D.) 1.26 x 10^24

Which of the following equalities is NOT correct? - 100cg=1g - 1000mm=1m - 1cm^3=1mL - 10kg=1g

D.) 10kg=1g

A cube of iron measures 3.0 centimeters on each side, with a volume of 27 cm^3. The density of iron is 7.86 g/cm^3. What is the mass in gras of this sample of iron? 0.87 g 34 g 71 g 210 g

D.) 210 g

A student weighs a cube of aluminum and records the mass as a 18.76 grams. What is the estimated digit? 1 8 7 6

D.) 6

When multiplying and dividing measured quantities, the number of significant figures in the results should be equal to the number of significant figures in: - all of the measurements - the least and more precise measurements - the most precise measurement - the least precise measurement

D.) the least precise measurement

prefix, power, abbreviation 1 tenth

Deci 10 ^ -1 d

How do the isotopes of a given element differ from one another?

Different amounts of neutrons and different atomic masses

What process can be used to purify water?

Distillation

Which process can be used to purify water?

Distillation

How many moles of CaCO3 are in 50 grams? 1 2 .2 4 .5

E.) .50

What distinguishes the atoms of one element from the atoms of another?

Each element's atoms all have a certain number of protons. For example: All of element A's atoms all have 13 protons (no matter how many neutrons or electrons it has)

Define isotope

Each of two or more forms of the same element that contain equal number of protons but different numbers of neutrons in their nuclei (and hence differ in atomic mass)

What makes the periodic table such a useful tool?

Easily compare the properties of elements in an organized way.

List the three subatomic particles and identify their relative masses, charges and locations within the atom.

Electrons are negative, have negligible mass, and are outside of the nucleus. Protons are positive, have a mass of 1 amu, and are in the nucleus. Neutrons are neutral, are in the nucleus and have a mass of 1.001 amu.

How are the elements arranged in the modern periodic table?

Elements in the periodic table are arranged by horizontal rows called periods and by vertical columns called groups.

How to find energy when given frequency

Energy = planck's constant times freq

True or False? Mendeleev is credited with the modern atomic theory

False

F

Fluorine

Who is credited with the discovery of the nuclear model of the atom?

Ernest Rutherford

What are random errors?

Errors due to a lack of consistency or precision

What are systematic errors?

Errors resulting from making the same mistake for every trial

Why do neon lights produce characteristic line spectra? Excited neon atoms give off light when their electrons return to lower energy levels. The neon electrons orbit the nucleus in a single energy level. Neon's electrons move faster when electricity passes through. Light is given off when the electrons orbit faster.

Excited neon atoms give off light when their electrons return to lower energy levels.

Which group of elements are called the halogens?

Group 17

Which elements are too reactive to be found as elements in nature? They lose 2 electrons to become stable Group 2, the alkaline earth metals Groups 3 - 12, the transition metals Group 1, the alkali metals Group 13, the aluminum group

Group 2

Which element groups are entirely metallic elements?

Groups 1-12

Which element groups contain some metals and some nonmetals?

Groups 13-16

Which element groups are made entirely of nonmetals?

Groups 17 and 18

Which of the following trends is accurate for the periodic table? From left to right in a period the ionization energy increases. From left to right in a period, the atomic radius increases. From left to right in a period the ionization energy increases. From top to bottom in a group, the atomic radius decreases. From left to right in a period the metallic character increases.

From left to right in a period the ionization energy increases

Ga

Gallium

Ge

Germanium

Au

Gold

He

Helium

Centi

Hundredth

H

Hydrogen

When is an idea a hypothesis, and when is it a theory?

Hypothesis: based on limited information Theory: well-tested explanation for a broad set of observations

Define solids, liquids, and gases

In a gas the particles are far apart and moving randomly. Solids or liquids contain particles that are more closely packed. In a solid, they are tightly packed in a fixed, organized pattern.

Fe

Iron

Who is credited with the discovery of the Plum Pudding Model?

JJ Thomson

Who is credited with the discovery of the indivisible atom?

John Dalton

Signifigant Figure

Known or estimated in a measurement

Kr

Krypton

Pb

Lead

V

Vanadium

Li

Lithium

Which elements are too reactive to be found as elements in nature? They lose 2 electrons to become stable.

Losing 2 electrons results in a +2 charge. Group 2 ions have a +2 charge

Mg

Magnesium

Mn

Manganese

What equation tells you how to calculate the number of neutrons in an atom?

Mass number - atomic number = number of neutrons

What does the number represent in the isotope Platinum-194? Write the symbol for this atom.

Mass number. Symbol: 194 Pt 78

How do you read a graduated cylinder?

Measure the amount at the bottom of the curve, minus one.

Hg

Mercury

prefix, power, abbreviation 1 millionth

Micro 10 ^ -6 μ

prefix, power, abbreviation 1 thousandth

Milli 10 ^ -3 m

Mega

Million

Micro

Millionth

How can there be more than 1000 different atoms when there are only about 100 different elements

Most elements have multiple isotopes

Ni

Nickel

N

Nitrogen

A cube of a gold-colored metal with a volume of 59 cm^3 has a mass of 980 g. The density of pure gold is 19.3 g/cm^3. Is the metal pure gold? Show calculations to justify your answer.

No; mass/volume = 17 g/cm^3

O

Oxygen

P

Phosphorus

What is the difference between a chemical change and a physical change?

Physical change: Physical properties are altered, but its chemical composition remains the same ex - phase change, grinding, tearing, dissolving, mixing Chemical change: Change in the chemical makeup of something. Results in the formation of one or more substances ex - color change, texture change, odor released

Pt

Platinum

K

Potassium

Sc

Scandium

Se

Selenium

What are significant figures? How do they imply the uncertainty of a measurement?

Sigificant figures are all of the certain digits and exactly one uncertain digit

Si

Silicon

Ag

Silver

How do you organize data, present it and analyze it?

Tables, graphs, ANOVA and T-tests

Deci

Tenth

Kelvin temp. scale

The SI Scale for temperature

Mole

The SI unit used to measure amount of substance

Which group of elements are highly reactive metals that form ions with a +1 charge?

The alkali metals

Weight

The force of gravity on an object

What is the atomic mass of an element?

The atomic mass of an element is a weighted average mass of the atoms in a naturally occurring sample of that element.

How does the microscopic model explain the macroscopic observations of matter?

The closer the particles are packed in something (on a microscopic level) the more dense something is (on a macroscopic level)

Absolute zero

The lowest point on the Kelvin scale

When water is heated and turned into water vapor, does the molecular size change? How is the mass effected? Density?

The molecular size doesn't change, the mass doesn't change (unless you are measuring in the same amount of space) and the density decreases as the water evaporates

Which group of elements are characterized by their chemical stability?

The noble gases

Celsius temp. scale

The non-SI scale for temperature

Avogadro's number

The number of representative particles of a substance present in 1 mole of that substance

Copper has 2 isotopes, 63 Cu and 65 Cu. Which isotope is more abundant? Support your answer.

The one with the mass nearest in value to the atomic mass for the element in the Periodic Table since that is the average atomic mass.

Percent composition

The percent by mass of each element in a compound

Empirical formula

The smallest whole number ratio of the atoms in a a compound

Which metals tend to be rather stable, but form colored compounds when they oxidize?

The transition metals

Kilo

Thousand

Milli

Thousandth

Sn

Tin

Ti

Titanium

The atomic masses of elements are generally not whole numbers. Explain why.

They represent a weighted average of the mass and the abundance of the isotopes

How is uncertainty in a measurement expressed explicitly? Implicitly?

Uncertainty can be shown using a plus or minus sign, or using vocabulary: about, roughly, approximately etc

U

Uranium

Find: Mass Given: # Moles and element

Use dimensional analysis: #Moles (Atomic mass/1 mole) = mass

Find: # Moles Given: Mass and element

Use dimensional analysis: Mass (1 mole/atomic mass) = # moles

How is atomic mass calculated?

Weighted average of the isotopes: multiply the mass of each isotope by its natural abundance, expressed as a decimal, and then add the products

Can elements change into compounds or visa versa?

Yes - chemical changes

Can elements change into other elements?

Yes - nuclear changes

Can mixtures be separated into pure substances?

Yes - physical changes

What data must you know about the isotopes of an element to calculate the atomic mass of the element?

You need to know the abundance of each isotope and the mass of each isotope

Zn

Zinc

A substance that is composed of two or more elements combines chemically in a fixed proportion by mass is: a. a compound b. a mixture c. an atom d. a solid

a. compound

How is percent error calculated?

absolute value of ((experimental value - actual value)/actual value) x 10^2

What are significant figures?

all of the certain digits and exactly one uncertain digit

Which atom contains a partially filled 3p orbital in its ground state? iron argon aluminum calcium

aluminum

Which particle consists of 13 protons, 14 neutrons, and 10 electrons?

an aluminium ion

What is matter?

anything that has mass and occupies space

The characteristic of an electromagnetic wave that is associated with the energy of that radiation is its: a.) amplitude b.) frequency c.) speed d.) momentum

b

The first scientist to show that atoms emit tiny negative particles was: a. JJ Thompson b. Lord Kelvin c. Ernest Rutherford d. William Hurst

b. Lord Kelvin

Where on the periodic table are the most metal characteristics

bottom left

Where on the periodic table is the larger atomic radius

bottom left

"Pieces" of energy are known as: a.) isotopes b.) particles c.) quanta d.) line spectra

c

The lowest sublevel in each principal energy is represented by the symbol: a.) f b.) p c.) s d.) d

c

Which of the following radiation types is not a part of the electromagnetic spectrum?: a.) microwave b.) x-ray c.) beta-ray d.) infrared

c

Which of the following will give rise to a spectrum most different from the other three? a.) sunlight b.) moonlight c.) red fireworks d.) white fireworks

c

prefix, power, abbreviation ten

deca 10 D

The shape of a typical p orbital is similar to a _______

dumbell

The second principal energy level of an atom can hold a total of ____ electrons

eight

Aufbau principle

electrons fill up the lowest energy levels before higher energy levels

The __________ the frequency, the higher the energy of its photons

greater

The electron configuration of an atom gives the distribution of electrons in the _________

ground state

prefix, power, abbreviation hundred

hecto 10 ^ 2 H

Hund's Rule

if there are multiple electrons at the same energy level, they will arrange themselves in separate orbitals whenever possible. there will be a maximum number of unpaired electrons in the outermost level

pauli exclusion principle

in an atom or molecule, no two electrons can have the same four electronic quantum numbers. As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

Which element has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d6? zinc copper manganese iron

iron

prefix, power, abbreviation thousand

kilo 10 ^ 3 K

How do we know the quality of data?

larger number of significant figures = more precision

The longer the wavelength, the _________ its frequency

lower

How do we communicate uncertainty?

margin of error - the last digit recorded, plus or minus notation

prefix, power, abbreviation million

mega 10 ^6 M

Group 1 elements are (metals/nonmetals) that are (stable/reactive) as elements. When they react, they (gain/lose) (electrons/protons) to become (atoms/ions) with a _____ charge

metal, reactive, lose electrons, ions +1

Explain the difference between an orbit and an orbital

orbits are the paths for electrons proposed by bohr and rutherford. they are not included in space where an electron with a particular energy is likely to be found. orbits describe the motion of electrons, but orbitals do not.

prefix, power, abbreviation trillionth

pico 10 ^ -12 p

How do we measure volume?

record number at bottom of meniscus plus one digit

What must be true for 2 electrons to occupy the same orbital? They must have opposite spins. They must be oppositely charged. They must remain at a constant distance from the nucleus. They must enter the orbital simultaneously.

they must have opposite spins

How are compounds separated?

through a chemical change (ex: boiling)

How are mixtures separated?

through a physical change (ex: filtering)

Where on the periodic table are the most nonmetal characteristics

top right

Where on the periodic table is the most electronegativity

top right

Where on the periodic table is the most ionization energy

top right

In which part of the periodic table are the most electronegative elements found? upper left lower left upper right lower right

upper right

How are all measurements made?

using a measuring tools to compare

relationship between wavelength and frequency

wavelength / frequency = speed of light