Download Unit 4 Study Guide - Key - Effingham County Schools

Unit 4 Study Guide
Review Timeline and Chapter 4 Sections 2 and 3 Review Worksheets
1. Visible light is a kind of _electromagnetic radiation_____, which is a form of energy
that exhibits _wave-like___________ behavior as it travels through space.
2. Do all forms of electromagnetic radiation travel at the same speed? __yes_________
3. What does the formula c = λν represent? _c = speed of light; λ = wavelength; ν =
frequency_________________________________
4. Wave motion can be characterized by two properties: _wavelength and
_frequency__________.
5. _Wavelength____________ (λ) is the distance between corresponding points on
adjacent waves. What is its unit? _m, cm, or nm_________
6. _Frequency____________ (ν) is defined as the number of waves that pass a given
point in a specific time. What is its unit? _waves/second or hertz(Hz)___________
7. Are frequency and wavelength directly or inversely proportional? _inversely_______
8. A _quantum______________ is the minimum amount of energy that can be lost or
gained by an _atom_________.
9. A _photon_____________ is a particle of electromagnetic radiation having zero mass
and carrying a quantum of energy.
10. The _photoelectric______________________ effect refers to the emission of
electrons from metals that have absorbed photons.
11. In terms of energy, what must happen for an atom to change from the ground state to
an excited state? _absorb energy________________________
12. If an electron is at its lowest energy it is in the _ground_____________ state.
13. What is the Heisenberg principle? __impossible to determine simultaneously both
the position and velocity of an electron or any other particle
14. __Bohr’s___________ model of the hydrogen atom suggested that an _electron____
can circle the nucleus only in allowed paths, or __orbits____________.
15. _Quantum_______________ theory describes mathematically the wave properties of
electrons and other very small particles.
16. An _orbital_______________ is a three-dimensional region around the nucleus that
indicates the probable location of an _electron__________.
17. According to quantum theory, can an electron’s position in an atom be known
precisely? __no__________
18. Quantum _numbers___________ specify the properties of atomic _orbitals______
and the properties of electrons in orbitals. How many quantum numbers are needed
to describe the energy state of an electron in an atom? ___4________
19. The _magnetic______ __quantum______ number describes the position of an orbital.
20. Which quantum number describes the main energy level? _principal quantum______
21. Which quantum number indicates the shape of an orbital? angular momentum_____
22. What does the spin quantum number describe? indicate the spin state of an e-_____
23. The arrangement of electrons in an atom is known as the atom’s _electron_________
__configuration__________.
24. Three basic rules govern the placement of electrons in orbitals. They are
Aufbau___________, __Pauli_________________, and __Hund’s_______________.
25. According to the _Aufbau principle_____________ , an electron occupies the lowestenergy orbital that can receive it.
26. According to the _Pauli exclusion principle_________, no two electrons in the same
atom can have the same set of four quantum numbers.
27. According to Hund’s rule________, orbitals of equal energy are each occupied by
one electron before any orbital is occupied by a second electron, and all electrons in
singly occupied orbitals must have the same spin.
1s2s2p3s3p4s3d4p5s
28. Up to the 5s orbital, what is the correct order to fill atomic orbitals? Hint: 1s2s2p…
29. What is the shape of an s orbital? _spherical_____________
30. What is the shape of the p orbitals? _dumb bells_________________
31. How many electrons are needed to fill the 1st energy level? __2_______ the 2nd
energy level? ____8________ the 3rd energy level? __18___________ the 4th energy
level? ____32________
32. In _orbital ______ __notation_________, an unoccupied orbital is represented by a
line, ____, with the orbital’s name written underneath the line.
33. _Electron_______ _configuration______ notation shows the number of electrons in a
sublevel by adding a superscript to the sublevel designation.
34. The electron configuration of carbon is 1s22s22p2. How many electrons are present in
carbon? _6_____ What is the atomic number of carbon? _6_______
35. Write the electron configuration of the element sulfur, which has an atomic number of
16. _1s22s22p63s23p4______________________________
36. Write the complete electron configuration notation, the orbital notation, and the noble
gas notation for titanium, Ti. How many electron containing orbitals are there in an
atom of titanium?
1s22s22p63s23p64s23d2
[Ar]4s23d2
12 electron containing orbitals (have to draw orbital notation to determine this)
37. Given the electron configuration for oxygen is 1s22s22p4, answer the following
questions:
a. How many electrons are in each oxygen atom?
8
b. What is the atomic number of this element?
8
c. What is the highest occupied energy level?
2