Chem test 2
Mono
1
Deca
10
What is the electron configuration for bromine?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
Di
2
Penta
5
Hepta
7
Octa
8
How many unpaired electrons does a ground state atom of sulfur have? A) 2 B) 4 C) 0 D)3
A
A possible quantum numbers for the last electron added to complete an atom of germanium in its ground state is. n I m1 ms A) 4 0 0 +1/2 B) 3 0 +1 -1/2 C) 4 1 -1 +1/2 D) 3 1 +1 -1/2
C
How many electrons are in a triple bond? A) 2 B) 0 C) 6 D) 4
C
Potassium permanganate is a strong oxidizer do reacts explosively with easily oxidized materials. What is the formula? A) KMnO3 B) K(MnO4)2 C) K2MnO4 D) KMnO4
D
Select the element with the most negative electron affinity. A) H B) Li C) Ne D) F
D
The compound, P4S10, is used in the manufacture of safety matches. What is its name? A) phosphorus sulfite B) posphourus decasulfide C) phosphorus sulfide D) tetraphosphorus decasulfide
D
Visible light, radio waves, microwave radiation, infrared, ultraviolet radiation, x-rays and gamma rays all constitute the electromagnetic spectrum. With similar characteristics do all of the spectrum to share? A) They all have equal energies. B) They all have the ability to generate heat in objects. C) they all have the same electron spin state. D) they are all the transmission of energy in the form of waves. E) they all have the same frequencies.
D
Amplitude
Height of a wave
covalent compound
Nonmetals + metals Metalloids + nonmental
l=1
P
l=0
S
Wavelength
The distance between identical points on a successive waves
Pauli Exclusion Principle
no two electrons in the same atom can have the same set of four quantum numbers
electrostatic energy
potential energy that results from the interaction of charged particles
Bond dipole moment
separation of charge in a bond that depends on the difference in electronegativity and the bond distance represented by partial charges or a vector
Tri
3
Treta
4
Hexa
6
Nona
9
" no two electrons in an atom of the same four quantum numbers" is a statement from? A) the pauli exclusion principle B) de Broglies relation C) hunds rule D) Bohrs equation
A
An element with the electron configuration [noble gas] ns^2(n-1)d^10np^3 has _____ valence electrons. A) 5 B) 10 C) 2 D) 15
A
Iron(lll) chloride hexahydrate is used as a coagulant sewage and industrial wastes. What is its formula? A) FeCl3•6H2O B) Fe3Cl•6H2O C) FeCl3(H2O)6 D) Fe3Cl(H2O)6
A
The FM station KDUL broadcast music at 99.1 MHz. Find the wavelength of these waves (c=3.00x10^8 m/s) A) 3.03 B) 0.330 C) 5.33x10^2 m D) >10^3
A
The covalent bond with the greatest polarity would form in which of these atom pairs? A) B-O B) S-O C) Br-Br D) C-O
A
The solar radiation spectrum peaks at what a wavelength of approximately 500 nm calculate the energy of the photon of the radiation ( c=3.00 x 108 m/s;h = 6.63 x 10-34 j•s) A) 4x10 ^-19 j B) 2x10 ^-25 j C) 6x10 ^14 j D) 1x10 ^-27
A
Which of These elements are the highest first ionization energy? A) As B) Ga C) Bi D) K
A
Triple bond
A chemical bond formed when atoms share three pairs of electrons
Double bond
A chemical bond formed when atoms share two pairs of electrons
chemical energy
A form of potential energy that is stored in chemical bonds between atoms.
Electronegativity
A measure of the ability of an atom in a chemical compound to attract electrons. Lower—> Higher Lower Higher
Single bond
A pair of shared electrons
Henry Moseley
Arranged the periodic table by atomic number instead of mass number
Calculate the energy, and joules, required to excite a hydrogen atom by causing an electronic transition from the N=1 to the N=4 principal energy level. Recall that the energy levels of each atom are given by En = -2.18x10^-18 J (1/n^2) A) 2.07x10^-29 B) 2.04x10^-18 C) 3.27x10^-17 D) 2.25x10^-18
B
How many electrons are in a double bond? A) 2 B) 4 C) 1 D) 6
B
Line spectrum from all regions of the electromagnetic spectrum including the paschen series of infrared lines for hydrogen are used by astronomers to identify elements present in the atmosphere of stars. Calculate the wavelength of the photon admitted with a hydrogen atom undergoes a transition from n=5 to n=3 (R=1.096776x10^7 m-1) A) 683.8 nm B) 1282 nm C) 205.1 nm D) 384.6 nm
B
The maximum number of electrons that can occupy an energy level described by the principal quantum number,n, is? A) n B) 2n^2 C) 2n D) n^2
B
What is the wavelength of light having a frequency of 4.8x10^14 s^-1 (c=3.00x10^8 m/s) A) 1600 m B) 630 nm C) 1600 nm D) 6.3x10^-7
B
Which element has the following ground state electron configuration? [Kr] 5s^2 4d^10 5p^2 A) Te B) Sn C) Pb D) Ge
B
Which of the following is a correct set of quantum numbers for an electron in a 3-D orbital. A) N = 3, L =2, M1=3 B) N= 3, L =2, M1 = -2 C) N= 3, L =1, M1 = +3 D) N= 3, L =3, M1 = +2
B
Which one of the following sets of the quantum numbers is not possible. n I m1 ms A) 4 3 -2 +1/2 B) 3 0 1 -1/2 C) 3 0 0 +1/2 D) 2 1 1 -1/2
B
Who noticed that the periodic table was arranged in order of atomic mass were every eighth Ellemen had similar properties and called this the law of octaves but this was not excepted by the scientific community? A) Thompson B) Newlands C) Moseley D) Mendeleev
B
Arrange the following bonds in order of decreasing polarity A) H - F > H - C > H - N > H - O B) H - C > H - N > H - O > H - F C) H - F > H - O > H - N > H - C
C
Arrange these ions in order of increasing ionic radius: K+, P^3-, S^2, Cl- A) P^3 < S^2- < Cl- < K* B) Cl- < S^2 < K+ < P^3- C) K+ < Cl- < S^2- < P^3- D) K+ < P^3- < S^2 < Cl-
C
Consider the element with the electron configuration [Kr] 5s^2 4d^7. This element is? A) a noble gas B) an actinide element C) a transition metal D) a halogen
C
What is the correct formula for copper(ll) phosphate? A) Cu2PO3 B) Cu(PO3)2 C) Cu3(PO4)2 D) Cu(PO4)2
C
What is the name of PCI3 A) trichlorophosphide B) phosphoric chloride C) phosphorus trichloride D) phosphorus chloride
C
Which of the following subshells has the highest energy in the element tantalum? A) 4d B) 5p C) 4f D)4s
C
Consider the set of isoelectronic atoms and ions A^2- , B- , C , D+ E^2+ . Which arrangement of relative radii is correct? A) A^2- < B- < C > D+ > E^2+ B) E^2+ > D+ > C > B- > A^2- C) none of these are correct D) A^2- > B- > C > D+ > E^2+
D
Hund's Rule states that most stable our arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with parallel spin are_____. A) not revenant B) minimized C) nullified D) neutral
D
In the quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed? n I m1 A) 3 0 0 B) 3 1 -1 C) 3 2 2 D) 3 3 2
D
In which of these substances are the atoms held together by polar covalent bonding? A) s8 B) SrCl2 C) CsCl D) CIF
D
What is the definition of an isoelectronic series? A) a series that has two or more species that have identical nuclear charges, but have different electron configuration's. B) a series that can have only up to three species and have similar electron configurations and nuclear charges. C) A series that has the same nuclear charge. D) A series that has two or more species that have identical electron configuration's, but different nuclear charges.
D
Which of these atom has the smallest radius? A) As B) Al C) Na D) P
D
Which of these compounds is most likely to be ionic? A) CO2 B) CS2 C) CC D) KF
D
Which of these pairs consist of isoelectronic species? A) Zn^2+ and Cu^2+ B) Na+ and K+ C) Mn2+ and Ar D) K+ and CL-
D
Which one of these pairs consist of isoelectronic species? A) Na+ and K+ B) Mn^2+ and Ar C) Zn^2+ and Cu^2+ D) K+ and Cl-
D
l=2
D
Law of Conservation of Energy
Energy cannot be created or destroyed
l=3
F
formal charge equation for Lewis structure
Formal charge = valence electrons - lone pair - 1/2 # bonding (Valence - dots + sticks)
dipole moment
a property of a molecule whose charge distribution can be represented by a center of positive charge and a center of negative charge
potential energy
stored energy that results from the position or shape of an object
Frequency
the number of complete wavelengths that pass a point in a given time
