Name: Period: Date: KIPP NYC College Prep General ...chemistrykippnyc.weebly.com/.../chem_bootcamp_units_1_and_2.pdf · KIPP NYC College Prep General Chemistry CHEMISTRY BOOTCAMP

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Name: ____________________________________ Period: ________ Date: ___________________ KIPP NYC College Prep General Chemistry

CHEMISTRY BOOTCAMP #1:

MATTER AND ATOMS

TASK: As a recruit of Chemistry Bootcamp, you have been enlisted to review the foundational

concepts of Matter and The Atom, which were covered in units 1 and 2 this year.

Proceed diligently through this packet with your Bootcamp Instructor and adhere to the following signs:

Stop Sign: Answer questions pertaining to information you just learned

Checkpoint: Exercise a skill you just learned

Regents Drill: Earn points to pass the lesson by answering Regents questions.

You can monitor your ranks by writing your points to each lesson below.

Good Luck! The Chemistry Team UNIT 1 - MATTER

Lesson #1- What are pure types of matter? _____ /17 pts

Lesson #2- How do types of mixtures vary? _____/ 8 pts

Lesson #3- How are the states/phases of matter held together? _____/4 pts

Lesson #4- How can you describe matter? _____/4 pts

Lesson #5- What products are made in physical and chemical changes? _____/ 4pts

Unit 1 Drill Points _____/ 37 points

UNIT 2 – THE ATOM

Lesson #6- How is the periodic table divided? _____/ 6pts

Lesson #7- How has the structure of the atom evolved? _____/ 6pts

Lesson #8- How do subatomic particles of an atom differ? _____/ 7 pts

Unit 2 Drill Points _____/ 19 points

BOOTCAMP FREE RESPONSE: _____/ 8 points

_____ 51 - 64 DRILL POINTS – ROCKED BOOTCAMP

______ 38- 50 DRILL POINTS – Satisfactory Cadet

______ 1-37 DRILL POINTS… RETURN TO BOOTCAMP

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Lesson #1 – What are pure types of matter?

MATTER: Any substance that has MASS and TAKES UP SPACE.

Are you made of matter? Support your answer.

CHECK YOUR UNDERSTANDING: CHECK YOUR UNDERSTANDING: Check anything on the list that would qualify as matter: In order to measure the mass of an object, you must

____ Gold Earrings use a __________________________________ found in the lab.

___ Sunlight It can also be called a balance.

___ Carbon Dioxide

1) All matter can be divided into these two

categories:

_______________________ & ________________________

2) Two examples of pure matter are

____________________________ & ____________________

3) Using the particle diagrams, state how elements and compounds are different if they are

both pure substances?

PURE SUBSTANCE #1: ELEMENTS

An element is type of matter composed (made up) of only ONE TYPE of atom.

All elements can be found on the periodic table All elements are made out of ATOMS! Pure aluminum is made up of only ALUMINUM ATOMS.

Brass is made up of copper and zinc atoms. Is brass an element? Explain.

An element’s symbol always has one capital letter (O, F, Ar, Pt or Cl) If it is on the periodic table… it is an element! Elements CANNOT be broken down any further.

Symbol Name Name Symbol 1. C: ___________________________________________________ 2. O: ___________________________________________________ 3. Hg: ___________________________________________________

4. Calcium: ____________ 5. Tungsten: ____________ 6. Potassium: ____________

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Example 1. Cu

a) What is the name? b) How many atoms in the formula Cu?

Example 2. O2

a) What is the name? b) How many atoms are in the formula O2?

Example 3. N3

a) What is the name? b) How many atoms are in the formula N3?

DRAW 6 particles in particle diagram:

Draw or depict 6 particles in particle diagram:

Depict 6 particles in particle diagram:

Why is NaCl NOT an element? _________________________________________________________________________________

DRILL POINTS! 10/17 points available

1. Determine the formula of the following elements. [1pt each] Mercury: _______________ Titanium: __________________

2. Determine the name of the following elements. [1pt each] Br: ________________________________________ Mn_____________________________________ B: Mg: Ni: N:

3. In the boxes provided: a) Using particle diagrams, draw two elements, one in each box, using the representations for

atoms of element X2 and element Z given below. [1]

KEY: Atom of element X =

Atom of element Z =

3 particles of X2 3 particles of Z

4. What is the total number of different elements present in NH4NO3? [1] (1) 7 (2) 9 (3) 3 (4) 4

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PURE SUBSTANCE #2: COMPOUNDS

A compound is a pure substance that is composed of 2 or more different elements chemically combined in a

FIXED PROPORTION.

A compound CAN be broken down into the elements of which it is composed.

3C’s – Chemically Combined Compounds

Place a check, if the substance is a compound:

Hint: Every capital letter is another element!

CO2 Ni BaCl2 NO3 AlF3 Cs O2

1. If compose means to make up, what does decompose mean? 2. O2

- Element or compound?

- What is the name of O2?

- How many atoms are in O2?

3. C6H12O6

- Element or compound?

- How many C’s? H’s? O’s?

- How many TOTAL atoms in glucose?

Draw particle diagrams of the following substances:

Use O = and H = H2 H2O H2O2 O2

Which diagrams above depict elements? _________________________ compounds? _________________________

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DRILL POINTS! 7/17 points available

1. Which substance can be broken down by a chemical change? [1] (1) Silicon (3) propane (2) mercury (4) Radon

2. Which substance can not be broken down by a chemical change? [1]

(1) Methane (3) tungsten (2) propanal (4) water

3. Which substance can be broken down by a chemical change? [1]

(1) Co (3) CO (2) C (4) Ca

Base your answer to 4 on the diagrams below.

(1) (2) (3) (4)

4. Explain why particle diagram (1) above does NOT represent a compound, even though it has two

different elements. [1]

__The next two questions are based on the particle diagram to the right: 5. Why is particle diagram #1 a compound? [1]

6. Why is particle diagram #3 not a compound even though it has two different elements? [1]

7. Two substances, A and Z, are to be identified. Substance A cannot be broken down by a chemical change.

Substance Z can be broken down by a chemical change. What can be concluded about these substances? [1]

(1) Both substances are elements.

(2) Both substances are compounds.

(3) Substance A is an element and substance Z is a compound.

(4) Substance A is a compound and substance Z is an element.

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Lesson #2 – How do types of mixtures vary? If matter is not pure (an element or a compound), it is a MIXTURE.

There are two types of mixtures: Homogeneous and Heterogeneous

Elements/Compounds are physically combined, not chemically combined.

Mixture Homogeneous Heterogeneous

Prefix “homo” means same or uniform “hetero” means different

Definition

Example

HINT HINT All aqueous (aq) solutions are

homogenous.

HOMOGENEOUS AND HETEROGENOUS ONLY REFER TO MIXTURES! REGENTS TIP! If you see “homogeneous compound” or “heterogeneous compound,” eliminate those answer

choices immediately!

Explain how a mixture differs from a pure substance.

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Classify each as an element (E), compound (C), or mixture (M).

1. Gatorade _________ 4. Hydrogen Peroxide(H2O2) _________ 2. Copper (Cu) _________ 5. Distilled water _________ 3. NaOH (aq) _________ 6. C6H12O6 _________

How do we represent mixtures in a particle diagram? Circle the correct answer.

DRILL POINTS! 5/8 points available 1. A dilute, aqueous potassium nitrate solution is best classified as a

(1) homogeneous compound (2) homogeneous mixture (3) heterogeneous compound (4) heterogeneous mixture

2. One similarity between all mixtures and compounds is that both

(1) Are heterogeneous (2) Are homogeneous (3) Combine in a definite proportion (4) Consist of two or more substances

3. Which sample represents a homogeneous mixture?

(1) C2H5OH (l) (2) C2H5OH (aq) (3) C2H5OH (g) (4) C2H5OH (s)

4. Which material is a mixture?

(1) water (2) air (3) methane (4) magnesium

5. Tetrachloromethane, CCl4, is classified as a

(1) compound because the atoms of the elements are combined in a fixed proportion (2) compound because the atoms of the elements are combined in a proportion that varies (3) mixture because the atoms of the elements are combined in a fixed proportion (4) mixture because the atoms of the elements are combined in a proportion that varies

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Separating Mixtures: Basic techniques

Different separation techniques must be used with mixtures because of their varying compositions.

TECHNIQUE #1: CRYSTALLIZATION/EVAPORATION Real Life Example: ROCK CANDY! BACKGROUND INFORMATION: Beaker 1 represents a homogenous mixture of sugar water that was created by dissolving sugar into water. A piece of string was left inside the mixture and the beaker was left out until all the water had evaporated. The result was that we made rock candy on a string!

QUESTIONS: Please answer all questions in complete sentences. 1. What is the rock candy made out of? How do you know?

2. hat do you think happened to the sugar water mixture that allowed for the rock candy to form? Describe the process.

TECHNIQUE #2: FILTRATION Real Life Example: SEPARATING NOODLES FROM WATER! BACKGROUND INFORMATION: Pasta noodles were cooked in salt water (salt is known to bring out the flavors in pasta). The pasta noodles were separated from the salt water using a filter.

QUESTIONS: Please answer all questions in complete sentences. 1. When the pasta noodles were cooking in salt water, both homogeneous and

heterogeneous mixtures were present. What was the homogeneous mixture? What was the heterogeneous mixture? How do you know?

2. hat ended up in the beaker after you separated the pasta noodle/salt water mixture? 3. s filtration better for separating homogeneous mixtures or heterogeneous mixture? Defend your answer.

Given a mixture of sand and water, state one process that can be used to separate water from the sand.

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Lab Throwback Looking at the set up to the right, which separation technique would this be used for? Explain your answer.

Which mixture can be separated by using the equipment shown in the diagram?

(1) NaCl (aq) and SiO2 (s) (2) NaCl (aq) and C6H12O6 (aq) (3) CO2 (aq) and NaCl (aq) (4) CO2 (aq) and C6H12O6 (aq)

DRILL POINTS! 3/8 points available

1. A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolved. Which statement best describes the resulting mixture? (1) The mixture is homogeneous and can be separated by filtration. (2) The mixture is homogeneous and cannot be separated by filtration. (3) The mixture is heterogeneous and can be separated by filtration. (4) The mixture is heterogeneous and cannot be separated by filtration.

2. Recovering the salt from a mixture of salt and water could best be accomplished by

(1) evaporation (2) filtration (3) paper chromatography (4) density determination

3. At room temperature, a mixture of sand and water can be separated by

(1) ionization (2) combustion (3) filtration (4) sublimation

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Lesson #3 – How are the states/phases of matter held together?

All matter may exist in three possible states of matter: SOLID, LIQUID or GAS. INTERMOLECULAR FORCES are the forces between the atoms of matter.

Based on this diagram… a) Which state of matter has the STRONGEST intermolecular forces? How do you know? b) Which state of matter has the WEAKEST intermolecular forces? How do you know?

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Standard temperature and Pressure

STP = Standard Temperature and Pressure When conditions are NORMAL. Nothing out of the ordinary is happening.

Find on Table A.

Standard Temperature: ___________________

Standard Pressure: ____________________

A substance has a melting point of 230 K and a boiling point of 769 K.

What state of matter is this substance in:

a) 300 K ___________________

b) 100 K __________________

c) 1000 K __________________ -----------------------------------------------------------------------------------------------

d) 500 K ___________________

e) STP ____________________

DRILL POINTS! 4 points available 1. Which statement best describes the shape and volume of Al(s), an aluminum cylinder at STP?

(1) It has a definite shape and a definite volume. (2) It has a definite shape and no definite volume. (3) It has no definite shape and a definite volume. (4) It has no definite shape and no definite volume.

Base your answers to questions 2- 4 on the diagram of a molecule of nitrogen shown below.

= one molecule of nitrogen (N2)

2. Draw a particle model that shows at 3. Draw a particle model that shows at

least six molecules of nitrogen gas, N2 (g). [1] least six molecules of liquid nitrogen, N2 (l). [1]

4. Describe, in terms of particle arrangement, the difference between nitrogen gas and liquid nitrogen. [1]

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__LESSON #4 – How can you describe matter?

Property: a characteristic of a substance that can be observed There are both physical and chemical properties that can be observed.

PROPERTY PHYSICAL PROPERTIES CHEMICAL PROPERTIES

DEFINITION

3-4 EXAMPLES

DENSITY: is a very important physical property.

This property DOES NOT change regardless of how much you have of the substance. Densities of all elements can be found on Table S. Density unit of measure: g/cm3

Ms. Green found a gold ring at a flea market, but wanted to know for sure it is was real. She brings it to you. After you divide the mass of the ring by its volume, you figure out that the density of this particular ring is 22.6 g/cm3. What do you tell Ms. Green?

Check for Understanding

A 10.0 cm3 sample of copper has a mass of 89.6 g. What is the density of copper?

Mass known: __________________

Volume known: ________________

DRILL POINTS! 4 points available 1. If an iron (Fe) sample has a mass of 15.9 g and a density of 7.87 g/cm3. Determine the volume of this particular sample.

2. A large sample of solid calcium sulfate is crushed into smaller pieces for testing. Which two physical properties are the same for both the large sample and the one of the smaller pieces? (1) Mass and density

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(2) Mass and volume (3) Melting point and density (4) Melting point and volume

3. Compared to the physical and chemical properties of the compound NO2, the compound N2O has

(1) Different physical properties and different chemical properties (2) Different physical properties and the same chemical properties (3) The same physical properties and different chemical properties (4) The same physical properties and the same chemical properties

4. Which statement describes a chemical property that can be used to distinguish between compound A and compound B? (1) A is a blue solid, and B is a white solid. (2) A does not corrode in acid, and B does corrode in acid. (3) A has a high melting point, and B has a low melting point. (4) A dissolves in water, and B does not dissolve in water.

__sson #5 – What products are made from physical and chemical changes?

PHYSICAL V. CHEMICAL CHANGES

Physical changes do NOT change the identity of the substance. Phase changes are Physical changes. SOLID LIQUID GAS

Chemical changes DO alter the identity of the substance.

Ch emical changes produce a NEW SUBSTANCE

Frankie said that when water evaporates into water vapor, that is an example of a chemical change. Do you agree or disagree? Explain.

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DRILL POINTS! 4 points available In an investigation, a dripless wax candle is massed and then lighted. As the candle burns, a small amount of liquid wax forms near the flame. After 10 minutes, the candle’s flame is extinguished and the candle is allowed to cool. The cooled candle is massed. 1. Identify one physical change that takes place in this investigation. [1] 2. State one observation that indicates a chemical change has occurred in this investigation. [1] 3. Which change results in the formation of different substances? (1) Burning of propane (3) Deposition of CO2(g) (2) Melting of NaCl(s) (4) Solidification of water

4. Given the particle diagram representing four molecules of a substance:

Which particle diagram best represents this same substance after a physical change has taken place?

_______________________________________________________________________________________________

Lesson #6 – How is the periodic table divided? The periodic table is arranged according to increasing ATOMIC NUMBER. Elements with similar properties occupy the same area of the table.

Metals and Nonmetals

Li

3

He

2

C

6

N

7

O

8

F

9

Ne

10

Na

11

B

5

Be

4

H

1

Al

13

Si

14

P

15

S

16

Cl

17

Ar

18

K

19

Ca

20

Sc

21

Ti

22

V

23

Cr

24

Mn

25

Fe

26

Co

27

Ni

28

Cu

29

Zn

30

Ga

31

Ge

32

As

33

Se

34

Br

35

Kr

36

Rb

37

Sr

38

Y

39

Zr

40

Nb

41

Mo

42

Tc

43

Ru

44

Rh

45

Pd

46

Ag

47

Cd

48

In

49

Sn

50

Sb

51

Te

52

I

53

Xe

54

Cs

55

Ba

56

Hf

72

Ta

73

W

74

Re

75

Os

76

Ir

77

Pt

78

Au

79

Hg

80

Tl

81

Pb

82

Bi

83

Po

84

At

85

Rn

86

Fr

87

Ra

88

Rf

104

Db

105

Sg

106

Bh

107

Hs

108

Mt

109

Mg

12

Ce

58

Pr

59

Nd

60

Pm

61

Sm

62

Eu

63

Gd

64

Tb

65

Dy

66

Ho

67

Er

68

Tm

69

Yb

70

Lu

71

Th

90

Pa

91

U

92

Np

93

Pu

94

Am

95

Cm

96

Bk

97

Cf

98

Es

99

Fm

100

Md

101

No

102

Lr

103

La

57

Ac

89

1

2

3

4

5

6

7

*

W

METALS

Nonmetals

Metalloids

Describe where most metal elements can be found on the periodic table. Most nonmetals with the exception of what element can be found on the upper right-hand corner of the table? List the metalloid elements:

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CHARACTERISTICS OF METALS, METALLOIDS AND NONMETALS

Non-Metals Metalloids Metals

Groups and Periods:

Term Definition How many are there are on the periodic table?

Group A column of the periodic table

Period A row of the periodic table

Which member of group 13 is found in the second period? (1) Be (2) Mg (3) B (4) Al

DRILL POINTS! 6 points available 1. Which element is ductile and conducts heat?

(1) Ag (3) Ne (2) F (4) Si

2. Which list of elements contains a metal, a metalloid, and a nonmetal?

(1) Zn, C, N (3) Si, Li, Sn (2) F, Cl, Br (4) Pt, Ge, F

3. Most of the elements in the Periodic Table are classified as

(1)Metalloids (3) Nonmetals (2) Noble gases (4) Metals

4. Which element is classified as a non-metal?

(1) Be (3) Al (2) Si (4) Cl

5. Which element is a metal that is in the liquid phase at STP? (1) Bromine (2) Cobalt (3) Hydrogen (4) Mercury

6. Which list of elements consists of a metal, a metalloid, and a nonmetal?

(1) Li, Na, Rb (3) Sn, Si, C (2) Cr, Mo, W (4) O, S, Te

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Lesson #7 – How has the structure of the atom evolved? Many atomic models existed as scientists discovered more information about the atom.

The atom is the smallest unit of matter.

Rutherford’s Gold Foil experiment contributed 2 important ideas of the atom BASED on the EVIDENCE he OBSERVED. RUTHERFORD OBSERVED…

THEREFORE, RUTHERFORD CONCLUDED…

1. Most alpha particles went straight through.

1.

2.

2. That there is a dense POSITIVELY charged NUCLEUS.

DRILL POINTS! 6 points available 1. Which sequence represents a correct order of historical developments leading to the modern model of the atom

(1) the atom is a hard sphere most of the atom is empty space electrons exist in orbitals outside the nucleus (2) the atom is a hard sphere electrons exist in orbitals outside the nucleus most of the atom is empty space (3) most of the atom is empty space electrons exist in orbitals outside the nucleus most of the atom is empty

space (4) most of the atom is empty space the atom is a hard sphere electrons exist in orbitals outside the nucleus

Plum-pudding Rutherford Bohr Wave-mechanical

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2. According to the wave-mechanical model of the atom, electrons in an atom (1) are mostly likely found in the excited state (2) have a positive charge (3) are located in orbitals outside the nucleus (4) travel in defined circles

. Which statement correctly describes the charge of the nucleus and the charge of the electron cloud of an atom?

(1) The nucleus is positive and the electron cloud is positive. (2) The nucleus is positive and the electron cloud is negative. (3) The nucleus is negative and the electron cloud is positive. (4) The nucleus is negative and the electron cloud is negative.

. Which group of atomic models is listed in historical order from earliest to the most recent?

(1) Hard-sphere model, wave-mechanical model, electron-shell model (2) Hard-sphere model, electron-shell model, wave mechanical model (3) Electron-shell model, wave-mechanical model, hard-sphere model (4) Electron-shell model, hard-sphere model, wave-mechanical model

5. Which of these phrases best describes our current understanding of the atom?

(1) A positive nucleus surrounded by a hard negative shell (2) A positive nucleus surrounded by a cloud of negative charges (3) A hard sphere with positive particles uniformly embedded (4) A hard sphere with negative particles uniformly embedded

6. In Rutherford’s gold foil experiments, some alpha particles were deflected from their original paths but most passed with no deflection. Which statement about gold atoms is supported by these experimental observations?

(1) Gold atoms consist mostly of empty space. (2) Gold atoms are similar to alpha particles. (3) Alpha particles and gold nuclei have opposite charges (4) Alpha particles are more dense than gold atoms.

__________________________________________________________________________________________________

Lesson #8 – How do the subatomic particles of the atom differ?

Every atom has three subatomic particles: Protons, Neutrons and Electrons

Atomic Number is the # of protons an atom has. # of protons NEVER CHANGES of the ATOM CHANGES.

The charge of the atom is ALWAYS neutral. (# of protons = # of neutrons) The charge of the nucleus is ALWAYS positive. (Protons +neutrons = POSITIVE)

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The periodic table is listed in order of increasing? (CIRCLE ONE) ATOMIC NUMBER MASS NUMBER

1. What is the atomic symbol represented above?______ 2. What element is this? ____________ 3. What is the atomic number? ________ 4. What is the mass number if there are 7 neutrons? __________ 8 neutrons? _______________ 5. How many protons does nitrogen have? _______ 6. How many electrons does nitrogen have? ______ 8. What kind of charge does nitrogen have? ______

DRILL POINTS! 5/7 points available 1. Which particles have approximately the same mass?

(1) An electron and an alpha particle (2) An electron and a proton (3) A neutron and an alpha particle (4) A neutron and a proton

2. An atom of any element must contain (1) An equal number of protons and neutrons (2) An equal number of protons and electrons (3) More electrons than neutrons (4) More electrons than protons

3. What is the number of electrons in an atom that has 3 protons and 4 neutrons? (1) 1 (3) 3 (2) 7 (4) 4

4. Each diagram to the right represents the nucleus of a different atom. Which diagrams represent nuclei of the same element? (1) D and E, only (2) D, E, and Q (3) Q and R, only (4) Q, R, and E

5. Which subatomic particles are located in the nucleus of a neon atom?

(1) electrons and positrons (2) electrons and neutrons (3) protons and neutrons (4) protons and electrons

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ISOTOPES

ISOTOPE: When versions of an atom exist with a DIFFERENT # of NEUTRONs in the nucleus The average mass of an atom is calculated by multiplying the mass (g) of each isotope by its percent abundance (%)

How to calculate average atomic mass:

QUESTION HOW TO SOLVE IT!

Calculate the average atomic mass of boron.

Calculate the atomic mass of copper.

Predict whether you think the answer will be closer to 63 or 65: __________________ Now solve: Atomic Mass = ___________________________ g/ mol

DRILL POINTS! 2/7 points available

1. What whole number do you predict

the atomic mass of sulfur to be closest to? ________________ 2. Show the numerical setup for calculating

the average atomic mass of sulfur.

AVERAGE ATOMIC MASS = (mass of A)( % abundance of A in ratio form) + (mass of B)(% abundance of B in ratio form) +..

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BOOTCAMP Free Response and Math!

Use the picture on the right to answer the following questions:

1. Which diagram depicts only one compound composed of atoms of element X and element Z? Explain.

2. Which diagram depicts a mixture of diatomic elements X and element Z? Explain.

3. Which diagram depicts a mixture that contains different compounds of element X and element Z? Explain.

4. Explain, in terms of protons and neutrons, why U-235 and U-238 are different isotopes of uranium. [1] Protons: Neutrons:

5. State one conclusion about atomic structure based on the observation that almost all alpha particles passed straight through the foil. [1]

6. Explain why an atom is considered to be neutral in charge but the nucleus of an atom is positively charge.

[1] 7. Explain why the atomic mass only accounts for protons and neutrons. [1]

8. If an object has a mass of 3.0 grams and has a volume of 2 mL (2 cm3), what is the density of the object?