Final Review Flashcards
Rank the following photons in terms of increasing energy:
Blue: 453 nm
Red: 660 nm
Yellow: 595nm
Lowest Energy
Red
Yellow
Blue
Which form of electro magnetic radiation has the shortest wavelength
a) gamma rays
B) red light
C) radio waves
D) infrared radiation
E) x-ray
A) gamma rays
The Heisenberg berg Uncertainty principle states that
A) no two electrons in the same atom can have the same set of four quantum numbers
B) two atoms of the same element must have the same number of protons
C) it is impossible to determine accurately both the position and momentum of an electron simultaneously
D) electrons of atoms in their ground states enter energetically equivalent sets of orbitals singly before they pair up in any orbital of the set
E) charged atoms (ions) must generate a magnetic field when they in motion
C) it is impossible to determine accurately both both the position and momentum of an electron simultaneously
Which of the following statements are/is true?
1. An excited atom can return to its ground states by absorbing electromagnetic radiation
2. The energy of an atom is increased when electromagnetic radiation is emitted from it
3 the energy of electromagnetic radiation increases as its frequency increases
4. An electron in the n = 4 state in the hydrogen atom can go to the n = 2 state by emitting electromagnetic radiation at the appripropiate frequency
A) 2, 3, 4
B) 3
C) 1, 2, 3,
D) 3 & 4
C) 1, 2, 4
D) 3 & 4
Which statement about electromagnetic radiation is false?
A) as frequency increases, wavelength decreases
B) as wavelength increase, energy increases,
C) as wavelength increases, frequency decreases
D) Wavelength and frequency are inversely proportional
E) wavelength and energy are inversely proportional
B) as wavelength increase, energy increases
What information does the square of the wave function (fork)^2 of an electron in an atom provide
Probability of finding electron in the atom
Rank in order of decreasing atomic/ionic radius
Cl Al K Na
Largest
K
Na
Al
Cl
Smallest
Increasing strength (Leftest to bottom)
Rank in order of decreasing atomic/ionic radius
I- , Bi 3+, Pb2+, Cs+
Largest
Iodine
Cesium
Lead II
Bismuth
Smallest
Atoms having greatly differing electronegativities are expected to form
A) no bonds
B) polar covalent bonds
C) nonpolar covalent bonds
D) ionic bonds
E) covalent bonds
D) ionic bonds
The ionic solid NaCl is more stable than a mixture of Na and Cl atoms. This is best explained by:
A) The large, negative crystal lattice energy compensates for the energy required when forming Na+ and Cl-
B) both the electron affinity for Cl and the ionization energy for Na are negative values.
C) The negative value for the electron affinity for Cl is larger than the ionization energy required for Na.
D) The negative value for the ionization energy required for Na is larger than the electron affinity for Cl
E) None of these is the correct explaination
A) the large, negative crystal lattice energy compensates for the energy required when forming Na+ and Cl-
The ____ bonds there are between atoms of the same two elements, the ___ the bond length and the ___ the bond
A) more; greater; weaker
B) more; shorter; stronger
C) fewer; shorter; stronger
D) fewer; greater; stronger
E) more; shorter; weaker
B) more; shorter; stronger
Based on electronegativity differences, which of the following is most likely to be ionic?
A) CaF2
B) Br2
C) BH3
D) BO
E) CF4
A) CaF2
When electrons in a molecule are not found between a pair of atoms but move throughout the molecule, this is called
A) ionic bonding
B) covalent bonding
C) polar covalent bonding
D) delocalization of the electrons
E) a dipole moment
d) delocalization of the electrons
