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162 Cards in this Set

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  • Back
Which of the following elements is in the same period as phosphorus? carbon, nitrogen, magnesium, oxygen
Magnesium.
Of the elements Pt, V, Li, and Kr, which is a nonmetal?
Kr.
The atomic number of an element is the total number of which particles in the nucleus?
Protons.
In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly? In, 49 p+ 49 e-. Cs, 55 p+ 132.9 e-. Zn, 30 p+ 60 e-. F, 19 p+ 19 e-.
In, 49 p+ 49 e-.
Which of the follwing is true about the electron configurations of the noble gasses? The highest s and p sublevels are completely filled. The highest occupied s and p sublevels are paritally filled. The electrons with the highest energy are in a d sublevel. The electrons with the highest energy are in an f sublevel.
The highest occupied s and p sublevels are completely filled.
The region of high probabilty of finding an electron.
Atomic orbital.
States the impossibility of knowing both velocity and position of a moving particle at the same time.
Heisenberg uncertainty principle.
The lowest energy level.
Ground state.
The tendency of electrons to enter orbitals of lowest energy first.
Aufbau principle.
The arrangement of electrons around atomic nucleus.
Electron configuration.
Each orbital has at most two electrons.
Pauli exclusion principle.
In the Bohr model of the atom, an electron in an orbit has a fixed _____.
Energy.
How does the energy of an electron change when the electron moves closer to the nucleus?
It decreases.
The principal quantum number indicates what property of an electron?
Energy level.
What is the shape of the 3p atomic orbital?
Dumbbell.
How many energy sublevels are in the second principal energy level?
2.
What is the maximum number of f orbitals in any single enrgy level in an atom?
7.
What is the maximum number of d orbitals in a principal energy level?
5.
What is the maximum number of orbitals in the p sublevel?
3.
What is the maximum number of electrons in the second principal energy level?
8.
When an electron moves from a lower to a higher energy level, the electron _____.
Absorbs a quantum of energy.
What types of atomic orbitals are in the third principal energy level?
S, p, and d only.
What is the next atomic orbital in the series 1s, 2s, 3s, 3p?
4s.
According to the aufbau principle, _____.
Electrons enter orbitals of the lowest energy first.
What is the number of electrons in the outermost energy level of an oxygen atom (valence electrons)?
6.
What is the elctron configuration of potassium?
1s2 2s2 2p6 es2 4s1
If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?
One electron in each orbital.
Which color of visible light has the highest energy?
Violet.
How are the frequency and wavelength of light related?
They are inversely proportional to each other.
Emission of light from an atom occurs when an electron ____.
Drops from a higher to a lower energy level.
Give the electron configuration for calcium.
1s2 2s2 2p6 3s2 3p6 4s2
How many valence electrons does Bromine have?
7.
How many valence electrons does Platinum have?
2.
Why does the 4s get filled up before the 3d?
There is an overlapping of energy levels, making the 4s actually closer to the nucleus.
Give the electron configuration for Iron?
1s2 2s2 2p6 3s2 3p6 4s2 3d6.
Give the shorthand configuration for Iodine.
(Kr) 5s2 4d10 5p5.
What do the Lewis Dot Structures tell us about an atom?
How many valence electrons there are.
Give the quantum number set for the last electron in Arsenic.
4 1 1 1/2.
Give the electron configuration for Nitrogen.
1s2 2s2 2p3.
Give the shorthand configuration for Sodium.
(Ne) 3s1.
What do the horizontal rows on the Periodic Table tell us?
Energy levels.
What does the third number in the quantum number set tell us?
Specific orbital.
Give the quantum number for both of strontium's valence electrons.
5 0 0 1/2 5 0 0 -1/2.
give the shorthand configuration for Zirconium.
(Kr) 5s2 4d2.
How many third level electrons are in Phosphorus?
5.
How many dots would we place around Bromine in our Lewis Dot Structure?
7.
Draw the shorthand configuration for Argon.
(Ne) 3s2 3p6.
What would be the second quantum number in the set for a 4p electron?
1.
How many dots would be placed around Uranium in the Lewis Dot Structure?
2.
How many maximum electrons can fit in the f section?
14.
The atomic number of an element is the toal number of which particles in the nucleus?
Protons.
How does atomic radius change from top to bottom in a group in the periodic table?
It tends to increase.
How does atomic radius change from left to right across a period in the periodic table?
It tends to decrease.
What element in the second period has the largest atomic radius?
Lithium.
Which of the following elements has the smallest atomic radius?
Chlorine.
What is the charge of a cation?
A positive charge.
Which of the following statements is true about ions?
Anions form when an atom loses protons.
The metals in Groups 1A, 2A, and 3A ____.
Lose electrons when they form ions.
Which of the following statements is NOT true about ions?
When a cation forms, more electrons are transfered to it.
In which of the following sets are the charges given correctly for all the ions? Na+, Mg+, Al+. K+, Sr2+, O-2
K+, Sr2+, O-2.
What is the element with the highest electronegativity value? cesium, helium, calcium, fluorine.
Fluorine.
Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?
Increase in atomic size.
Which of the following elements has the smallest ionization energy?
Potassium.
Electronegativity generally increases from ____ to ____ across a period.
Left to right.
As you move from left to right across the second period of the periodic table ____.
Ionization energy increases.
The atomic number of an element is the toal number of which particles in the nucleus?
Protons.
How does atomic radius change from top to bottom in a group in the periodic table?
It tends to increase.
How does atomic radius change from left to right across a period in the periodic table?
It tends to decrease.
What element in the second period has the largest atomic radius?
Lithium.
Which of the following elements has the smallest atomic radius?
Chlorine.
What is the charge of a cation?
A positive charge.
Which of the following statements is true about ions?
Anions form when an atom loses protons.
The metals in Groups 1A, 2A, and 3A ____.
Lose electrons when they form ions.
Which of the following statements is NOT true about ions?
When a cation forms, more electrons are transfered to it.
In which of the following sets are the charges given correctly for all the ions? Na+, Mg+, Al+. K+, Sr2+, O-2
K+, Sr2+, O-2.
What is the element with the highest electronegativity value? cesium, helium, calcium, fluorine.
Fluorine.
Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?
Increase in atomic size.
Which of the following elements has the smallest ionization energy?
Potassium.
Electronegativity generally increases from ____ to ____ across a period.
Left to right.
As you move from left to right across the second period of the periodic table ____.
Ionization energy increases.
Of the following elements, which one has the smallest ionization energy?
Aluminum.
How many valence electrons are in an atom of phosphorus?
5.
How many valence electrons are in an atom of magnesium?
2.
How many valence electrons does a helium atom have?
2.
How many valence electrons are in a silicon atom?
4.
What is the name given to the electrons in the highest occupied energy level of an atom?
Valence electrons.
What is the charge on the strontium ion?
2+.
How many electrons does barium have to give up to achieve a noble-gas electron configuration?
2.
Which of the following elements does not form an ion with a charge of 1+?
Fluorine.
How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?
3.
Which of the following occurs in an ionic bond?
Oppostiely charged ions attract.
What is the net charge of the ionic compound calcium fluoride?
0.
Which of the following particles are free to drift in metals?
Electrons.
What is the basis of a metallic bond?
The attraction of metal ions to mobile electrons.
How do atoms achieve noble-gas electron configuration in single covalent bonds?
Two atoms share one electron each.
why do atoms share electrons in covalent bonds?
To attain a noble-gas electron configuration.
Which of the following elements, when bonded to itself, are held together by triple covalent bonds/
Nitrogen.
Valence electrons that do not participate in bonding in diatomic oxygen molecules?
Unshared pair.
Which of the following diatomic molecules is joined by a double covalent bond?
O2.
A molecule with a single covalent bond is _____.
Cl2.
How many electrons can occupy a single molecular orbital?
2.
According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?
Pairs of valence electrons.
Experimental evidence suggests that the H-C-H bond angles in ethene, C2 H4 are
120 degrees.
What type of hybrid orbital exists in the methane (CH4) molecule?
sp3.
What type of hybridization occurs in the orbitals of a carbon atom participating in a triple bond with another carbon atom (ex. C2Cl2)?
sp.
If two identical carbon atoms bond together, they form what type of bond?
Nonpolar covalent.
The B-F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is
Ionic.
In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded by
8 electrons.
Compared with nonmetals, the number of valence electrons in metals is generally.
Smaller.
What is the hybridization of the central atom in PF3?
sp3.
What is the molecular geometry of water?
Bent.
What is the domain geometry of C02?
Linear.
What is the hybridization of the each carbon in C2H4?
sp2
What sublevels are involved in valence electrons?
s and p.
A physical blend of two or more components.
Mixture.
Part of a sample having unifrom compostition and properties.
Phase.
Not uniform in composition.
Heterogeneous mixture.
A substance formed in a chemical raction.
Product.
Starting substance in a chemical reaction.
Reactant.
An example of an extensive property of matter.
Mass.
Evaporation is a ____ change.
Physical.
Air cannot be classified as a ____.
Substance.
Soil is a ____ mixture.
Heterogeneous.
A ____ mixture cannot be considered a single phase.
Heterogeneous.
____ mixtures are known as solutions.
Heterogeneous.
Air is a ____ misture.
Heterogeneous.
Salt Water is a ____ mixture.
Homogeneous.
____ are substances.
Compounds.
Silver is a ____.
Substance.
What is one difference between a mixture and a compound?
A compound can only be seperated into its components by chemical means.
In the chemical reaction in which sucrose is heated and decomposes to form carbon dioxide and water, which of the ____ is a reactant.
Sucrose.
Fermenting of cheese is not a ____ change.
Physical.
Decomposing _____ involve a physical change.
Doesn't.
When paper turns yellow-brown upon exposure to sunlight, what type of chnage is likely taking place?
A chemical change.
A fracture formation ____ indicate that a chemical change may have taken place.
Doesn't.
What happens to matter during a chemical reaction?
Matter is neither destroyed or created.
The total mass of the reactants ____ the total mass of the products.
Equals.
Who was the man who lived from 460BC-370BC and was among the first to suggest the idea of atoms?
Democritus.
Which theory included that atoms of the same element are always identical?
Dalton's Atomic Theory.
In ____ particles, the mass of a neutron nearly equals the mass of a proton.
Subatomic.
Who conducted experiments to determine the quntity of charge carried by an electron?
Millikan.
All atoms are ____.
Neutral, with the number of protons equaling the number of electrons.
As a consequence of the discover of the nucleus by ____, Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
Rutherford.
The atomic number of an element is the total number of ____ particles in the nucleus.
Protons.
What does the number 84 in the name krypton-84 represent?
The mass number.
Isotopes of the same element have different ____.
Numbers of neutrons.
Determine the number of neutrons in 16 O.
8.
How many protons, electrons, and neutrons does an atom with the atomic number 50 and mass number 125 contain?
50 protons, 50 electrons, 75 neutrons.
True or false: Atoms are mostly empty space.
False.
How is the number of neutrons in the nucleus of an atom calculated?
Subtract the number of protons from the mass number.
How many neutrons does 238/92 U have?
146.
What unit is used to measure weighted average atomic mass?
Amu.
True or false: Neutrons are located in the nucleus of an atom.
False.
The average atomic mass of an element depends upon the ____.
Mass and relative abundance of each isotope of that element.
What particle is emitted in alpha radiation?
Helium nucleus.
What is the change in the atomic number when an atom emits an alpha particle?
Increases by 2.
What is the change in atomic number caused by the emission of gamma radiation?
Remains the same.
What symbol is used for beta radiation?
0/-1 e
What is the change in atomic mass number when an atom emits an alpha particle?
Decreases by 4.
If an isotope decays by the process of beta emission, ____.
The atomic number changes.
Nuclear fusion ____.
Takes place in the sun.
What device was created by JJ Thomson in his discovery of the electron?
Cathode ray tube.