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