MIDTERM EXAM REVIEW 2015: Chapter 3,4,11
1. Describe the motions of particles in the three common states of matter.
2. How does a physical change differ from a chemical change?
3. Give three examples of chemical changes and three examples of physical changes.
4. List the 7 diatomic molecules.
5. Distinguish between a chemical and physical property. List 5 physical properties and 3 chemical properties.
6. How does an element differ from a compound? How does a compound differ from a mixture?
7. Identify the following as an element, a compound, a homogeneous mixture, or a heterogeneous mixture.
a. CH4
d. Salt water
b. Al
e. Distilled water
c. Concrete
f. CH2O
8. How is a homogeneous mixture different from a heterogeneous mixture?
9. Describe the processes of distillation and filtration. What types of mixtures are best separated by each
process? Can you separate a compound using either of the techniques? Why or why not?
10. What is an isotope? How do isotopes of one element differ from each other?
11. What are Dalton’s five postulates? Which of them are no longer valid?
12. Explain the experiment depicted below and identify the scientist responsible. What was discovered?
13. Explain the experiment depicted below and identify the scientist responsible for conducting it.
14. For the following elements give the number of protons, neutrons, and electrons.
a. Br – mass number= 80
b. Pd+2 mass number= 106
c. Cs-1
mass number= 133
d. cadmium-114
15. If you change the number of protons in an atom what do you create?
16. If you change the number of electrons in an atom what do you create?
17. If you change the number of neutrons in an atom what do you create?
18. What is the difference between the Bohr and Rutherford atomic models?
19. List 5 types of electromagnetic radiation.
20. Relate the frequency, wavelength and energy of any form of electromagnetic radiation.
21. Distinguish between the ground state and the excited state of an atom.
22. How many total orbitals are in the second principal energy level? third principal energy level?
23. How many total electrons are found in:
a. the first principal energy level
b. the second principal energy level
c. the third principal energy level
d. the fourth principal energy level
24. What are valence electrons? Give an example.
26. Write the electron configuration, the orbital notation and the noble gas notation of the following elements:
a. Cl
b. Zn
c. Ba
27. Compare and contrast the shape and number of orbitals in the s, p and d sublevels.
28. Which group in the periodic table corresponds to the alkali metals? Alkaline Earth Metals? Halogens?
Noble gases?
29. The d block includes which type of elements?
30. Define the following terms:
a. Ionization energy
c. Atomic Radius
31. What is the trend for atomic size as you go across a period? Down a group?
32. What is the trend for ionization energy as you go across a period? Down a group?
33. What type of ion will the following elements make?
a. Al
b. Mg
c. Br
d. N
34. What is the difference between a cation and an anion?
35.. Explain the pictures below. Think about the atomic models and experiments we discussed in class.
Chapter 3 Objectives
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To understand the processes of filtration and distillation
To learn to distinguish between chemical and physical properties
To learn to distinguish between chemical and physical changes
To understand the definitions of elements and compounds
To learn to distinguish between mixtures and pure substances
Chapter 3 Vocabulary
Matter
States of matter
Solid
Liquid
Gas
Physical properties
Chemical properties
Physical change
Chemical change
Reaction
Element
Compound
Mixture
Pure substance
Homogeneous mixture
Solution
Heterogeneous mixture
Distillation
Filtration
Chapter 4 Objectives
Elemental symbols
Law of constant composition
Dalton’s atomic theory
Atom
Compound
Chemical formula
Electron
Nuclear atom
Nucleus
Proton
Neutron
Isotopes
Atomic number
Mass number
Periodic table
Groups
Alkali metals
Alkaline earth metals
Halogens
Noble gases
Transition metals
Metals
Nonmetals
Metalloids
Diatomic molecules
Ion
Cation
Anion
Ionic compound
Chapter 4 Vocabulary
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To learn about the relative abundances of the elements
To learn the names and symbols of some elements
To learn about Dalton’s Theory of atoms.
To understand and illustrate the law of constant composition
To learn how a formula describes a compound’s composition
To learn about the internal parts of an atom and their important features.
To understand Rutherford’s experiment to characterize the atom’s structure
To understand the meaning of the terms isotope, atomic number, and mass number from the element’s
symbol
To learn about various features of the periodic table and properties of metals, nonmetals, and metalloids
To learn the natures of the common elements
To understand the formulation of ions from their parent atoms and how to name them
To learn how the periodic table can help predict which ion a given element forms
To learn how ions combine to form neutral compounds
To learn the groups in the periodic table
Chapter 11 Vocabulary
Electromagnetic radiation
Wavelength
Frequency
Photon
Quantized energy levels
Wave mechanical model
Orbital
Principal energy levels
Sublevels
Pauli exclusion principle
Electron configuration
Orbital (box) diagram
Valence electrons
Core electrons
Lanthanide series
Actinide series
Main-group representative
elements
Metals
Nonmetals
Metalloids
Ionization energy
Atomic size
Chapter 11 Objectives
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To describe Rutherford’s model of the atom
To explore the nature of electromagnetic radiation
To understand wavelength, frequency and energy relationships
To understand the relationship between color and energy of ER
To see how atoms emit light (the processes of absorption and emission)
To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy
To learn about Bohr’s model of the hydrogen atom
To understand how the electron’s position is represented in the wave mechanical model
To learn about the shapes of orbitals designated by s, p, and d
To review the energy levels and orbitals of the wave-mechanical model of the atom
To learn about electron spin
To understand how the principal energy levels fill with electrons in atoms beyond hydrogen
To learn about valence electrons and core electrons
To learn about the electron configurations of atoms with Z greater than 18.
To learn about noble gas notation