Untitled Flashcards Set

Chapter 1 -Introduction to Chemistry

Section 1.1 A Story of Two Substances
Use each of the terms below just once to complete the passage.

Earth's (1) atmosphere is made up of several layers. The air we breathe makes up the lowest level. This layer is called the (2) troposphere. The next layer up is called the(3) stratosphere. This level contains a protective (4) ozone layer. Ozone forms when (5) oxygen gas is struck by ultraviolet radiation in the upper part of the stratosphere. The ozone forms a layer around Earth, which absorbs (6) ultraviolet radiation.Without ozone, you are more likely to get a sunburn or possibly skin cancer. The thinning of the ozone  layer, called the (7) ozone hole, is worrisome because without ozone all organisms on Earth are subject to harm from too much radiation.
For each statement below, write true or false.

true  8. CFC is another name for a chlorofluorocarbon.
false 9. CFCs are made up of carbon, fluorine, and cesium.
true 10. All CFCs are synthetic chemicals.
false 11. CFCs usually react readily with other chemicals.
true 12. CFCs were developed as replacements for toxic refrigerants.

Section 1.2 Chemistry and Matter

For each statement below, write true or false.

false 13. The mass of an object can vary with the object's location.
false 14. A mass measurement includes the effect of Earth's gravitational pull on the object being measured.
true 15. Scientists measure the amount of matter in terms of mass.
true 16. Subtle differences in weight exist at different locations on Earth.
false 17. Your mass on the Moon would be smaller than your mass on Earth.

Identify each branch of chemistry described.

18. The study of the matter and processes of living things - Biochemistry

19.The study of carbon-containing chemical - Organic Chemistry

20 The study of the components and composition of substances - Analytical Chemistry

21. The study of matter that does not contain organic chemicals - Inorganic Chemistry

22. The study of the behavior and changes of matter and the related energy changes - Physical Chemistry

Answer the following questions.

1.  Compare the macroscopic world with the submicroscopic world.

The macroscopic world is what we can see with our eyes, while the submicroscopic world involves atoms and molecules that are too small to see.

2. Why are chemists interested in the submicroscopic description of matter?

Chemists study the submicroscopic world to understand how substances behave, react, and interact at the atomic level.

Section 1.3 Scientific Methods
Use the words below to complete the concept map. Write your answers in the spaces below the concept map.

Section 1.4 Scientific Research
For each description below, write A for applied research or P for pure research.

A 1. Is undertaken to solve a specific problem
P 2. Seeks to gain knowledge for the sake of knowledge itself
A 3. Is used to find CFC replacements
P 4. Was conducted by Molina and Rowland.

Chapter 2 -Analyzing Data

Section 2.1 Units and Measurement

Review Base units, SI prefixes and Derived units 

Answer the following questions.

1.Which temperature scale will you use for your experiments in this class? Is this an SI unit.

I will use celsius and it isn’t an SI unit.

2. How many grams are in a kilogram? 

1 kilogram = 1,000 grams.

3. How many liters are in a mega liter?

1 megaliter = 1,000,000 liters.

4. How many centimeters are in a meter?

1 meter = 100 centimeters.

5. What is the difference between a base unit and a derived unit?

A base unit is a fundamental measurement (e.g., meter, kilogram), while a derived unit is a combination of base units (e.g., m³ for volume).

6. What is density?

Density is a ratio that compares the mass of an object to its volume.

7. How can you obtain an object's volume if you know its density and its mass?

volume = mass / density

8. What is the three-part process for problem solving?

Analyze, solve, and evaluate

9. How are degrees Celsius converted to kelvins?

Add 273 to degrees Celsius.

Section 2.2 Scientific Notation and Dimensional Analysis

1. Change the following data into scientific notation.

   1. 5,000,000 km - 5 x 10^6 km  c.   8,394,000,000 s - 8.394 x 10^9 s

   2. 0.000421 g - 4.21 x 10^-4 g  d.   0.03 cm - 3 x 10^-2 cm

Complete the following dimensional analysis problems.

1.Convert 50 kilograms into grams. 50,000 grams

2. Convert 5 meters into centimeters.  500 centimeters

3. Convert 5 liters into kiloliters. 0.005 kiloliters

4. Convert 5 centimeters into meters. 0.05 meters

5. Convert 55 kilometers per hour into meters per second. Use the conversion factor 1 km = 1000 m. 15.28 m/s

Section 2.3 Uncertainty in Data

Use each of the terms below just once to complete the statements.

6.The digits that are reported in an answer are called significant figures.

7. The numeral 9.66 has three significant figures, two known figures and one
   estimated figure.

8. Non-zero numbers are always significant.

9. All final zeros to the right of the decimal place are significant.

10. Zeros that act as placeholders are not significant.

11. Counting numbers have an infinite number of significant figures.

12. When you convert to scientific notation, you remove the placeholder zeros.

13. Round the following to four significant figures.

14. Round 12.783 456 to the requested number of significant figures.

15. Round 120.752416 to the requested number of significant figures.

16. Complete the following calculations. Round off the answers to the correct number of significant figures.

Section 2.4 Representing Data

Sequence the following steps. Write 1 beside the first step in plotting a line graph.
Write 2 beside the second step, and so on.

7  5. Give the graph a title.
3  6. Choose the ranges for the axes.
1  7. Identify the independent and dependent variables.
5  8. Plot the data points.
2  9. Determine the range of the data that needs to be plotted for each axis.
6 10. Draw the "best fit" line for the data.
4 11. Number and label each axis.

Chapter 3-Matter—Properties and Changes

Section 3.1 Properties of Matter

Use each of the terms below just once to complete the passage.

Matter is anything with (1) mass and volume. A (2) substance is a form of matter with a uniform and unchanging composition. Substances have specific, unchanging (3) properties that can be observed. Substances have both physical and chemical properties. (4) Physical properties can be observed without changing a substance's chemical composition. Color, hardness, and (5) density are examples. Other properties cannot be observed without changing the composition of a substance. These are called (6) chemical properties. An example is the tendency of iron to form rust when exposed to air.

Label each property as either physical or chemical.

physical  7. Chemical formula H₂O
chemical   8. Forms green carbonate when exposed to moist air
chemical   9. Remains unchanged when in the presence of nitrogen
physical 10. Colorless
physical 11. Solid at normal temperatures and pressures
chemical 12. Ability to combine with another substance
physical 13. Melting point
physical 14. Liquid at normal temperatures and pressures
physical 15. Boiling point is 100°C
physical 16. Conducts electricity
physical 17. Density is

Label each drawing with one of these words: solid, liquid, gas.

       gas                       solid                         liquid

For each statement below, write true or false.

True 19 . All matter that we encounter in everyday life exists in one of three physical  forms.
True 20 . A solid has definite shape and volume.
False 21. A liquid has a definite shape and takes on the volume of its container.

True 22. A gas has both the shape and the volume of its container.
False 23. The particles in a gas cannot be compressed into a smaller volume.
False 24. Liquids tend to contract when heated.
False 25. The particles in a solid are spaced far apart.
False 26. The words gas and vapor can be used interchangeably.

Section 3.2 Changes in Matter .

What kinds of changes do these words indicate? Write each word under the correct heading. Use each word only once.

boil, crumble, crush, freeze, grind, explode, burn, ferment,oxidize, rot, 

condense, melt, vaporize corrode, rust, tarnish

Answer the following question. Write an equation showing conservation of mass of reactants and products.

6. In a laboratory, 178.8 g of water is separated into hydrogen gas and oxygen gas. The hydrogen gas has a mass of 20.0 g. What is the mass of the oxygen gas produced?

Water(178.8g)→Hydrogen gas(20.0g)+Oxygen gas(158.8g) - 158.8g

Section 3.3 Mixtures of Matter.

Use the words below to complete the concept map.

For each item in Column A, write the letter of the matching item in Column B.

Section 3.4 Elements and Compounds

Label each substance as either an element or a compound.

Element 1. silicon           Compound  2. sodium chloride
Element 3. francium          Element 4. nickel
Compound   5. ice

Write the symbol for each element.          Ne     6. neon                             Ca 7. calcium                         Fe       8. iron                            Ti 9. titanium                          F 10. fluorine 

Use the law of definite proportions and the equation below to answer the questions.

The law of definite proportions states that regardless of the amount, a compound is always composed of the same elements in the same proportion by mass.

11.A 20.0-g sample of sucrose contains 8.4 g of carbon. What is the mass percentage of carbon in sucrose? Show your work.  Mass percentage=20.08.4​×100=42.0%

12. Sucrose is 51.50% oxygen. How many grams of oxygen are in 20.0 g of sucrose? Show your work Mass of oxygen=51.50×20.0÷100=10.3g

13.A 2-g sample of sucrose is 6.50% hydrogen. What is the mass percentage of hydrogen in 300 g of sucrose? Explain your reasoning. The mass percentage of hydrogen is still 6.50% because it remains constant regardless of the sample size.

14.Two compound samples are found to have the same mass percentages of the same elements. What can you conclude about the two samples? The two samples are the same compound because their elements have identical mass percentages.

Use the law of multiple proportions to answer the questions and complete the table below.

The law of multiple proportions states that if the elements X and Y form two compounds, the different masses of Y that combine with a fixed mass of X can be expressed as a ratio of small whole numbers.

15. Two compound samples are composed of the same elements, but in different proportions. What can you conclude about the two samples? The two samples are different compounds because their elements combine in distinct whole-number mass ratios.

Chapter 4 - The Structure of the Atom

Section 4.1 Early Ideas About Matter

For each statement below, write true or false.

False 1. Ancient philosophers regularly performed controlled experiments.
True  2. Philosophers formulated explanations about the nature of matter based on their own experiences.
True   3. Both Democritus and Dalton suggested that matter is made up of atoms.
True  4. Dalton's atomic theory stated that atoms separate, combine, or rearrange in  chemical reactions.
False  5. Dalton's atomic theory stated that matter is mostly empty space.
False   6. Dalton was correct in thinking that atoms could not be divided into smaller particles.

True  7. Dalton's atomic theory stated that atoms of different elements combine in simple whole-number ratios to form compounds.
True   8. Dalton thought that all atoms of a specific element have the same mass.
False 9. Democritus proposed that atoms are held together by chemical bonds, but no one believed him.
True 10. Dalton's atomic theory was based on careful measurements and extensive research.

 Section 4.2 Defining the Atom

For each item in Column A, write the letter of the matching item in Column B.

Section 4.3 How Atoms Differ

For each statement below, write true or false.

False   1. The number of neutrons in an atom is referred to as its atomic number.
True   2. The periodic table is arranged by increasing atomic number.
True   3. Atomic number is equal to the number of electrons in an atom.
True  4. The number of protons in an atom identifies it as an atom of a particular element
False   5. Most atoms have either a positive or a negative charge.

Answer the following questions.

6. Lead has an atomic number of 82. How many protons and electrons does lead have? 82, 82

7. Oxygen has 8 electrons. How many protons does oxygen have? 8

8. Zinc has 30 protons. What is its atomic number? 30

9. Astatine has 85 protons. What is its atomic number? 85

10. Rutherfordium has an atomic number of 104. How many protons and electrons does it have? 104, 104

         11. Polonium has an atomic number of 84. How many protons and electrons does it have? 84, 84

12.Nobelium has an atomic number of 102. How many protons and electrons does it have? 102, 102

Determine the number of protons, electrons, and neutrons for each isotope described below.

13.An isotope has atomic number 19 and mass number 39.19 protons, 19 electrons, 20 neutrons

14. An isotope has 14 electrons and a mass number of 28. 14 protons, 14 electrons, 14 neutrons

15. An isotope has 21 neutrons and a mass number of 40. 19 protons, 19 electrons, 21 neutrons

16. An isotope has an atomic number 51 and a mass number 123.  51 protons, 51 electrons, 72 neutrons

Answer the following question.

17. Which of the isotopes in problems 13-16 are isotopes of the same element? Identify the element. #13 and #15 - potassium

Write each isotope below in symbolic notation. Use the periodic table to determine the atomic number of each isotope.

18. neon-22 ^22 Ne10                              19. helium ^4He2

20 cesium-133 ^133Cs55                          21. uranium-234 ^234U92

Label the mass number and the atomic number on the following isotope notation.

Use the figures to answer the following questions.

24. What is the atomic number of osmium? 76

25.What is the chemical symbol for niobium? Nb

26. What is the atomic mass of osmium? 190.23

27. What units is the atomic mass reported in? amu

28. How many protons and electrons does an osmium atom have? A niobium atom? 76 protons and electrons - 41 protons and electrons

Section 4.4 Unstable Nuclei and Radioactive Decay. ( pg #’s 122 – 124) 

Chapter 5 - Electrons in Atoms

Use each of the terms below just once to complete the passage.

Electromagnetic radiation is a kind of (1) energy that behaves like a(n)
(2) wave as it travels through space. (3) Light is one type of electromagnetic radiation. Other examples include X rays, radio waves, and microwaves. All waves can be characterized by their wavelength, amplitude, frequency, and (4) speed. The shortest distance between equivalent points on continuous wave is called a(n) (5) wavelength. The height of a wave from the origin to a crest or from the origin to a trough is the (6) amplitude. (7) Frequency is the number of waves that pass a given point in one second. The SI unit for frequency is the (8) hertz, which is equivalent to one wave per second.

Use the figure to answer the following questions.

9. Which letter(s) represent one wavelength? Which letter(s) represent the amplitude? A and C represent the wavelengths. B represents the amplitude.

10. If twice the length of A passes a stationary point every second, what is the frequency of the wave? The frequency is 2 waves/s or 2 Hz.

For each statement below, write true or false.

False 11. Like the visible spectrum, an atomic emission spectrum is a continuous range of colors.
True 12. Each element has a unique atomic emission spectrum.
True 13. A flame test can be used to identify the presence of certain elements in a  compound.
True 14. The fact that only certain colors appear in an element's atomic emission  spectrum indicates that only certain frequencies of light are emitted.
False 15. Atomic emission spectra can be explained by the wave model of light.
False 6. The neon atoms in a neon sign emit their characteristic color of light as they absorb energy.
True 17. When an atom emits light, photons having certain specific energies are being emitted.

Section 5.2 Quantum Theory and the Atom.     

  Use each of the terms below to complete the statements.

1. The lowest allowable energy state of an atom is called its ground state.

2. Bohr's model of the atom predicted the frequencies of the lines in hydrogen's atomic emission spectrum.

3. According to Bohr's atomic model, the smaller an electron's orbit, the lower
   the atom's energy level.

4. According to Bohr's atomic model, the larger an electron's orbit, the higher the atom's energy level.

5. Bohr proposed that when energy is added to a hydrogen atom, its electron moves to a higher-energy orbit.

6. According to Bohr's atomic model, the hydrogen atom emits a photon corresponding to the difference between the energy levels associated with the two orbits it transitions between.

7. Bohr's atomic model failed to explain the atomic emission spectrum of elements other than hydrogen.

Answer the following question.

8. How do the Bohr model and the quantum mechanical model of the atom differ in how they describe electrons? The Bohr model shows electrons in fixed orbits, while the quantum model shows electrons in cloud-like areas with different energy levels.

9. In the space at the left, write the term in parentheses that correctly completes the statement.

Do not 1. Atomic orbitals (do, do not) have an exactly defined size.
Two 2. Each orbital may contain at most (two, four) electrons.
Spherically shaped 3. All s orbitals are (spherically shaped, dumbbell shaped).
n 4. A principal energy has (n, n²) energy sublevels.
Electrons 5. The maximum number of (electrons, orbitals) related to each principal   energy level equals 2n².
Three 18. There are (three, five) equal energy p orbitals.
2s and 2p 19. Hydrogen's principal energy level 2 consists of (2s and 3s, 2s and 2p) orbitals.
Nine 20. Hydrogen's principal energy level 3 consists of (nine, three) orbitals.

Section 5.3 Electron Configuration.

Use each of the terms below just once to complete the passage.

The arrangement of electrons in an atom is called the atom's (1) electron configuration. Electrons in an atom tend to assume the arrangement that gives the atom the (2) lowest possible energy. This arrangement of electrons is the most (3) stable arrangement and is called the atom's (4) ground state electron configuration. Three rules define how electrons can be arranged in an atom's orbitals. The (5) Aufbau principle states that each electron occupies the lowest energy orbital available. The(6) Pauli exclusion principle states that a maximum of two electrons may occupy a single atomic orbital, but only if the electrons have opposite (7) spins. (8) Hund’s rule states that single electrons with the same spin must occupy each equal- energy orbital before additional electrons with opposite spins occupy the same orbitals.                               

Review Electron configuration & Electron configuration notation ( pg 156 – 160)

Answer the following questions.

12. What is germanium's atomic number? How many electrons does germanium have? 32, 32

13. What is noble-gas notation, and why is it used to write electron configurations? Noble-gas notation uses the bracketed symbol of the nearest preceding noble gas atom in the periodic table in the electron configuration of an atom. Using noble gas notation allows you to represent the complete electron configuration of an atom with many electrons in a shorthand form. 

14. Write the ground-state electron configuration of a germanium atom, using noble-gas notation. [Ar] 4s^2 3d^10 4p^2

Chapter 6 The Periodic Table and Periodic Law

Section 6.1 Development of the Modern Periodic Table.

For each item in Column A, write the letter of the matching item in Column B.

In the space at the left, write true if the statement is true; if the statement is false, change the italicized word or phrase to make it true.

False, 3 1. There are two main classifications of elements.
False, metals 2. More than three-fourths of the elements in the periodic table are nonmetals.
True 3. Group 1 elements (except for hydrogen) are known as the alkali metals.
False, 2A 4. Group 13 elements are the alkaline earth metals.
True  5. Group 17 elements are highly reactive nonmetals known as halogens.
False, noble gases 6. Group 18 elements are very unreactive elements known as transition metals.
False, nonmetals 7. Metalloids have properties of both metals and inner transition metals.

Section 6.2 Classification of the Elements.

Answer the following questions.

8.Why do sodium and potassium, which belong to the same group in the periodic table, have similar chemical properties?  They have the same number of valence electrons.

  9. How is the energy level of an element's valence electrons related to its period on the periodic table? Give an example. The number of the period is the same number of the highest energy level for a given element found.

Use the periodic table on pages 178-179 in your textbook .

10.Into how many blocks is the periodic table divided? 4 : s, p, d, f 

11.What groups of elements does the s-block contain? Alkali + alkaline earth metals

12.Why does the s-block portion of the periodic table span two groups? The s orbital holds 2 valence electrons.

13.,What groups of elements does the p-block contain? Boron family to noble gasses

14.Why are members of group 18 virtually unreactive? This is because they have a complete octet for their valence shell so they are stable and don’t want to gain/lose electrons by reacting.

15. How many d-block elements are there? 40 (10 across, 4 periods)

16. What groups of elements does the d-block contain? Transition metals 

17. Why does the f-block portion of the periodic table span 14 groups?  The f orbital can hold 14 electrons

18. What is the electron configuration of the element in period 3, group 16? [Ne] 3s^2 3p^4

Section 6.3 Periodic Trends

Answer the following questions. 

19. What is ionization energy? Energy required to remove the outermost electron.

20.  Explain why an atom with a high ionization-energy value is not likely to form a positive ion. It is very hard to remove the electron.

21.What is the period trend in the first ionization energies? Why? Generally increases → higher nuclear charge holds electrons tighter → there are some exceptions though.

22. What is the group trend in the first ionization energies? Why? - Generally decreases → lower nuclear charge due to the shielding effect.

23. State the octet rule. Eight electrons filling the valence shell of an atom.

24. What does the electronegativity of an element indicate? The ability of an atom to attract an element  to itself.

25. What are the periods and groups trends in electronegativities? Periods → increases 

Group → decreases.