Periodic Table Practice 11/29

Size: px
Start display at page:

Download "Periodic Table Practice 11/29"

Transcription

1 Periodic Table Practice 11/29 1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the number of oxidation states 2. Which list of elements consists of a metal, a metalloid, and a nonmetal? A) Li, Na, Rb B) Cr, Mo, W C) Sn, Si, C D) O, S, Te 3. Which list includes elements with the most similar chemical properties? A) Br, Ga, Hg B) Cr, Pb, Xe C) O, S, Se D) N, O, F 4. The elements in Group 2 are classified as A) metals B) metalloids C) nonmetals D) noble gases 5. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have A) fewer valence electrons B) more valence electrons C) fewer electron shells D) more electron shells 6. Which statement identifies the element arsenic? A) Arsenic has an atomic number of 33. B) Arsenic has a melting point of 84 K. C) An atom of arsenic in the ground state has eight valence electrons. D) An atom of arsenic in the ground state has a radius of 146 pm. 7. Which statement explains why sulfur is classified as a Group 16 element? A) A sulfur atom has 6 valence electrons. B) A sulfur atom has 16 neutrons. C) Sulfur is a yellow solid at STP. D) Sulfur reacts with most metals. 8. Which substance can be decomposed by chemical means? A) tungsten B) antimony C) krypton D) methane 9. Element X is a solid that is brittle, lacks luster,and has six valence electrons. In which group on the Periodic Table would element X be found? A) 1 B) 2 C) 15 D) Which element is an alkali metal? A) hydrogen B) calcium C) sodium D) zinc 11. Most of the groups in the Periodic Table of the Elements contain A) nonmetals, only B) metals, only C) nonmetals and metals D) metals and metalloids 12. Which of the following Period 4 elements has the most metallic characteristics? A) Ca B) Ge C) As D) Br 13. Which Group 15 element exists as a diatomic molecule at STP? A) phosphorus B) nitrogen C) bismuth D) arsenic 14. In which set do the elements exhibit the most similar chemical properties? A) N, O, and F B) Hg, Br, and Rn C) Li, Na and K D) Al, Si and P 15. As the elements in Group 15 are considered in order of increasing atomic number, which sequence in properties occurs? A) nonmetal metalloid metal B) metalloid metal nonmetal C) metal metalloid nonmetal D) metal nonmetal metalloid 16. All of the atoms of the elements in Period 2 have the same number of A) protons B) neutrons C) valence electrons D) occupied energy levels (shells) Page 1

2 17. The observed regularities in the properties of elements are periodic functions of their A) atomic numbers B) mass numbers C) oxidation states D) non-valence electrons 18. Five cubes of iron are tested in a laboratory. The tests and the results are shown in the table below. Which tests demonstrate chemical properties? A) 1, 3, and 4 B) 1, 3, and 5 C) 2 and 4 D) 2 and Which property can be defined as the ability of a substance to be hammered into thin sheets? A) conductivity B) malleability C) melting point D) solubility 20. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a A) metal B) metalloid C) noble gas D) nonmetal 21. Which element is a liquid at 305 K and 1.0 atmosphere? A) magnesium B) fluorine C) gallium D) iodine 22. Which two characteristics are associated with metals? A) low first ionization energy and low electronegativity B) low first ionization energy and high electronegativity C) high first ionization energy and low electronegativity D) high first ionization energy and high electronegativity 23. Which element is malleable and can conduct electricity in the solid phase? A) iodine B) phosphorus C) sulfur D) tin 24. Which substance can not be decomposed by ordinary chemical means? A) methane B) mercury C) ethanol D) ammonia 25. The elements located in the lower left corner of the Periodic Table are classified as A) metals B) nonmetals C) metalloids D) noble gases 26. What is a property of most metals? A) They tend to gain electrons easily when bonding. B) They tend to lose electrons easily when bonding. C) They are poor conductors of heat. D) They are poor conductors of electricity. Page 2

3 27. The element in Period 4 and Group 1 of the Periodic Table would be classified as a A) metal B) metalloid C) nonmetal D) noble gas 28. Which of the following Group 15 elements has the greatest metallic character? A) nitrogen B) phosphorus C) antimony D) bismuth 29. At STP, graphite and diamond are two solid forms of carbon. Which statement explains why these two forms of carbon differ in hardness? A) Graphite and diamond have different ionic radii. B) Graphite and diamond have different molecular structures. C) Graphite is a metal, but diamond is a nonmetal. D) Graphite is a good conductor of electricity, but diamond is a poor conductor of electricity. 30. Which list of symbols represents nonmetals, only? A) B, Al, Ga B) Li, Be, B C) C, Si, Ge D) P, S, Cl 31. Which two gases can not be broken down by chemical means? A) CO and He B) CO and NH3 C) Xe and He D) Xe and NH3 32. Which phrase describes the molecular structure and properties of two solid forms of carbon, diamond and graphite? A) the same molecular structures and the same properties B) the same molecular structures and different properties C) different molecular structures and the same properties D) different molecular structures and different properties 33. Which particle diagram represents the arrangement of F2 molecules in a sample of fluorine at 95 K and standard pressure? A) B) C) D) 34. What are two properties of most nonmetals? A) high ionization energy and poor electrical conductivity B) high ionization energy and good electrical conductivity C) low ionization energy and poor electrical conductivity D) low ionization energy and good electrical conductivity 35. Which is a property of most nonmetallic solids? A) high thermal conductivity B) high electrical conductivity C) brittleness D) malleability 36. Which element is least likely to undergo a chemical reaction? A) lithium B) carbon C) flourine D) neon 37. Which statement explains why neon is a Group 18 element? A) Neon is a gas at STP. B) Neon has a low melting point. C) Neon atoms have a stable valence electron configuration. D) Neon atoms have two electrons in the first shell. Page 3

4 38. Which group in the Periodic Table contains elements that are all monatomic gases at STP? A) 15 B) 16 C) 17 D) Which element has both metallic and nonmetallic properties? A) Rb B) Rn C) Si D) Sr 40. Which list of elements consists of metalloids, only? A) B, Al, Ga B) C, N, P C) O, S, Se D) Si, Ge, As 41. Which isotopic notation identifies a metalloid that is matched with the corresponding number of protons in each of its atoms? A) 24 Mg and 12 protons B) 28 Si and 14 protons C) 75 As and 75 protons D) 80 Br and 80 protons 42. Which element is a liquid at STP? A) bromine B) cesium C) francium D) iodine 43. Nuclei of U-238 atoms are A) stable and spontaneously absorb alpha particles B) stable and spontaneously emit alpha particles C) unstable and spontaneously absorb alpha particles D) unstable and spontaneously emit alpha particles 44. At STP, a 7.49-gram sample of an element has a volume of 1.65 cubic centimeters. The sample is most likely A) Ta B) Tc C) Te D) Ti 45. Solid samples of the element phosphorus can be white, black, or red in color. The variations in color are due to different A) atomic masses B) molecular structures C) ionization energies D) nuclear charges 46. Which statement correctly describes two forms of oxygen, O2 and O3? A) They have identical molecular structures and identical properties. B) They have identical molecular structures and different properties. C) They have different molecular structures and identical properties. D) They have different molecular structures and different properties. 47. Which Lewis electron-dot diagram represents a nitrogen atom in the ground state? A) B) C) D) 48. Which Lewis electron-dot diagram is correct for a S 2 ion? A) B) C) D) 49. What is represented by the dots in a Lewis electron-dot diagram of an atom of an element in Period 2 of the Periodic Table? A) the number of neutrons in the atom B) the number of protons in the atom C) the number of valence electrons in the atom D) the total number of electrons in the atom 50. The number of valence electrons in each atom of an element affects the element's A) chemical properties B) number of isotopes C) decay mode D) half-life 51. Aqueous solutions of compounds containing element X are blue. Element X could be A) carbon B) copper C) sodium D) sulfur Page 4

5 52. An element with a partially filled d sublevel in the ground state is classified as A) a halogen B) a transition metal C) an alkali metal D) an alkaline earth metal 53. Which set of properties is most characteristic of transition elements? A) colorless ions in solution, multiple positive oxidation states B) colorless ions in solution, multiple negative oxidation states C) colored ions in solution, multiple positive oxidation states D) colored ions in solution, multiple negative oxidation states 54. What occurs when a magnesium atom becomes a magnesium ion? A) Electrons are gained and the oxidation number increases. B) Electrons are gained and the oxidation number decreases. C) Electrons are lost and the oxidation number increases. D) Electrons are lost and the oxidation number decreases. 55. What is the number of electrons in an Al 3+ ion? A) 10 B) 13 C) 3 D) When an atom of lithium loses an electron, the atom becomes a A) negative ion with a radius smaller than the radius of the atom B) negative ion with a radius larger than the radius of the atom C) positive ion with a radius smaller than the radius of the atom D) positive ion with a radius larger than the radius of the atom 57. What can be concluded if an ion of an element is smaller than an atom of the same element? A) The ion is negatively charged because it has fewer electrons than the atom. B) The ion is negatively charged because it has more electrons than the atom. C) The ion is positively charged because it has fewer electrons than the atom. D) The ion is positively charged because it has more electrons than the atom. 58. What is the total number of electrons in a S 2 ion? A) 10 B) 14 C) 16 D) Which ion has the smallest radius? A) B) C) D) 60. As the elements is Period 3 are considered in order of increasing atomic number, there is a general decrease in A) atomic mass B) atomic radius C) electronegativity D) first ionization energy 61. Which grouping of circles, when considered in order from the top to the bottom, best represents the relative size of the atoms of Li, Na, K, and Rb, respectively? A) B) C) D) 62. Which list of elements is arranged in order of increasing electronegativity? A) Be, Mg, Ca B) F, Cl, Br C) K, Ca, Sc D) Li, Na, K Page 5

6 63. Which statement describes the general trends in electronegativity and atomic radius as the elements in Period 2 are considered in order from left to right? A) Both electronegativity and atomic radius increase. B) Both electronegativity and atomic radius decrease. C) Electronegativity increases and atomic radius decreases. D) Electronegativity decreases and atomic radius increases. 64. Which statement describes the general trends in electronegativity and first ionization energy as the elements in Period 3 are considered in order from Na to Cl? A) Electronegativity increases, and first ionization energy decreases. B) Electronegativity decreases, and first ionization energy increases. C) Electronegativity and first ionization energy both increase. D) Electronegativity and first ionization energy both decrease. 65. Which atom has the weakest attraction for electrons in a chemical bond? A) a boron atom B) a calcium atom C) a fluorine atom D) a nitrogen atom 66. As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally A) decreases B) increases C) remains the same 67. The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as A) first ionization energy B) activation energy C) conductivity D) electronegativity 68. As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to A) decreasing radius and decreasing shielding effect B) decreasing radius and increasing shielding effect C) increasing radius and decreasing shielding effect D) increasing radius and increasing shielding effect 69. Which element has atoms that can form halide ions? A) iodine B) silver C) strontium D) xenon 70. When the elements in Group 1 are considered in order from top to bottom, each successive element at standard pressure has A) a higher melting point and a higher boiling point B) a higher melting point and a lower boiling point C) a lower melting point and a higher boiling point D) a lower melting point and a lower boiling point 71. Which phrase describes a compound that consists of two elements? A) a mixture in which the elements are in a variable proportion B) a mixture in which the elements are in a fixed proportion C) a substance in which the elements are chemically combined in a variable proportion D) a substance in which the elements are chemically combined in a fixed proportion 72. Which statement explains why water is classified as a compound? A) Water can be broken down by chemical means. B) Water is a liquid at room temperature. C) Water has a heat of fusion of 334 J/g. D) Water is a poor conductor of electricity. Page 6

7 73. Base your answer to the following question on the information below. Given: Samples of Na, Ar, As, Rb Which two of the given elements have the most similar chemical properties? 74. Base your answer to the following question on the information below and on your knowledge of chemistry. Potassium phosphate, K3PO4, is a source of dietary potassium found in a popular cereal. According to the Nutrition-Facts label shown on the boxes of this brand of cereal, the accepted value for a one-cup serving of this cereal is 170 milligrams of potassium. The minimum daily requirement of potassium is 3500 milligrams for an adult human. Identify the noble gas whose atoms have the same electron configuration as a potassium ion. Base your answers to questions 75 and 76 on the information below and on your knowledge of chemistry. Some properties of the element sodium are listed below. is a soft, silver-colored metal melts at a temperature of 371 K oxidizes easily in the presence of air forms compounds with nonmetallic elements in nature forms sodium chloride in the presence of chlorine gas 75. Convert the melting point of sodium to degrees Celsius. 76. Identify one chemical property of sodium from this list. Page 7

8 77. Base your answer to the following question on the information below and on your knowledge of chemistry. The Lewis electron-dot diagrams for three substances are shown below. Identify the noble gas that has atoms with the same electron configuration as the positive ion represented in diagram 1, when both the atoms and the ion are in the ground state. Base your answers to questions 78 through 80 on the information below and on your knowledge of chemistry. There are six elements in Group 14 on the Periodic Table. One of these elements has the symbol Uuq, which is a temporary, systematic symbol. This element is now known as flerovium. 78. State the expected number of valence electrons in an atom of the element flerovium in the ground state. 79. Explain, in terms of electron shells, why each successive element in Group 14 has a larger atomic radius, as the elements are considered in order of increasing atomic number. 80. Identify an element in Group 14 that is classified as a metalloid. Page 8

1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on

1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on 1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the number of oxidation states 2.

More information

Practice Periodic Table Review

Practice Periodic Table Review Practice Periodic Table Review Name 1. An electron will emit energy in quanta when its energy state changes from 4p to A) 5s B) 5p C) 3s D) 6p 2. Which electron configuration represents an atom in the

More information

1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass

1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass 1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the

More information

1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass

1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass 1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the

More information

Name: Teacher: Gerraputa

Name: Teacher: Gerraputa Name: Teacher: Gerraputa 1. Which list of elements contains a metal, a metalloid, and a nonmetal? 1. Ag, Si, I 2 3.K, Cu, Br 2 2. Ge, As, Ne 4.S, Cl 2, Ar 2. The elements on the Periodic Table are arranged

More information

Periodic Table Practice Questions

Periodic Table Practice Questions Periodic Table Practice Questions 1. Elements in the Periodic Table are arranged according to their (1) atomic number (3) relative activity (2) atomic mass (4) relative size 2. Elements in a given period

More information

Unit 4 - Periodic Table Exam Name: PRACTICE QUESTIONS Date: 2/23/2016

Unit 4 - Periodic Table Exam Name: PRACTICE QUESTIONS Date: 2/23/2016 Name: PRACTICE QUESTIONS Date: 2/23/2016 1. Which pair of symbols represents a metalloid and a noble gas? 1) Si and Bi 2) As and Ar 3) Ge and Te 4) Ne and Xe 2. What determines the order of placement of

More information

Regents review Atomic & periodic

Regents review Atomic & periodic 2011-2012 1. The diagram below represents the nucleus of an atom. What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9

More information

Periodic Table Workbook

Periodic Table Workbook Key Ideas: The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order

More information

HSVD Ms. Chang Page 1

HSVD Ms. Chang Page 1 Name: Chemistry, PERIODIC TABLE 1. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) noble gas (2) metalloid (3) metal (4) nonmetal 2. Which

More information

Name PRACTICE Unit 3: Periodic Table

Name PRACTICE Unit 3: Periodic Table 1. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have (1) fewer valence electrons (2) more valence electrons (3) fewer electron shells (4) more electron shells 2. On the

More information

The Atom/Periodic Table After School Regents Review Practice

The Atom/Periodic Table After School Regents Review Practice 1. An ion that consists of 7 protons, 9 neutrons, and 10 electrons has a net charge of A) 2 B) 2+ C) 3+ D) 3 2. The mass of a proton is approximately equal to the mass of A) an electron B) a neutron C)

More information

Test Review # 4. Chemistry: Form TR4-5A 6 S S S

Test Review # 4. Chemistry: Form TR4-5A 6 S S S Chemistry: Form TR4-5A REVIEW Name Date Period Test Review # 4 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing the symbol, the atomic mass,

More information

Regan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period

Regan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally

More information

Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table

Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Focus Questions for the unit... How has the modern view of the atom changed over time? How does a chemist use symbols and notation to communicate

More information

Regan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period

Regan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally

More information

Part A. Answer all questions in this part.

Part A. Answer all questions in this part. Part A Directions (1-20): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.

More information

Name: 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron

Name: 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron Chemistry Section Name: MID TERM STUDY GUIDE Date: A. Multiple Choice. 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron

More information

A) 12 u C) K, Ca, Sc C) An electron has a negative charge and is located outside the nucleus. C) number of valence electrons

A) 12 u C) K, Ca, Sc C) An electron has a negative charge and is located outside the nucleus. C) number of valence electrons 1. An atom that contains six protons, six neutrons, and six electrons has a mass of approximately A) 12 u B) 12 g C) 18 u D) 18 g 2. What is the correct Lewis electron-dot structure for the compound magnesium

More information

Exam Electrons and Periodic Table

Exam Electrons and Periodic Table 1-20 multiple choice. Answer on scantron. 21-25 short response. Answer on exam paper. All questions are 4 points each. 1. Which term is defined as the region in an atom where an electron is most likely

More information

Practice Packet Unit: 5 Periodic Table

Practice Packet Unit: 5 Periodic Table Regents Chemistry: Practice Packet Unit: 5 Periodic Table 1 VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help

More information

A) first electron shell D) are located in orbitals outside the nucleus A) 2-3 D) 18 A) K and Na C) a mixture C) Sb2O5

A) first electron shell D) are located in orbitals outside the nucleus A) 2-3 D) 18 A) K and Na C) a mixture C) Sb2O5 1. In a calcium atom in the ground state, the electrons that possess the least amount of energy are located in the A) first electron shell B) second electron shell C) third electron shell D) fourth electron

More information

Note that the protons and neutrons are each almost 2,000 times more massive than an electron; What is the approximate diameter of an atom?

Note that the protons and neutrons are each almost 2,000 times more massive than an electron; What is the approximate diameter of an atom? Atomic Structure and the Periodic Table Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on

More information

2/15/2013. Chapter 6 6.1

2/15/2013. Chapter 6 6.1 Chapter 6 In a self-service store, the products are grouped according to similar characteristics. With a logical classification system, finding and comparing products is easy. You will learn how elements

More information

Unit 2: The Periodic Table

Unit 2: The Periodic Table Unit 2: The Periodic Table The following pages are practice questions for this unit, and will be submitted for homework! You must complete: Unit Vocabulary ALL QUESTIONS What Group Am I? ALL QUESTIONS

More information

Chapter 4 Atoms Practice Problems

Chapter 4 Atoms Practice Problems Chapter 4 Atoms Practice Problems 1) The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons. 2) Which of the following is a

More information

Organizing the Periodic Table

Organizing the Periodic Table Organizing the Periodic Table How did chemists begin to organize the known elements? Chemists used the properties of the elements to sort them into groups. The Organizers JW Dobereiner grouped the elements

More information

Chapter 2 Atoms and the Periodic Table

Chapter 2 Atoms and the Periodic Table Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.

More information

Name 2/14 Bonding Page 1

Name 2/14 Bonding Page 1 Bonding Page 1 Name 2/14 1. Which formula represents an ionic compound? A) NaCl B) N2O C) HCl D) H2O 2. Which type of bond results when one or more valence electrons are transferred from one atom to another?

More information

Physical Science Study Guide

Physical Science Study Guide Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table

More information

11. The bright-line spectra produced by four elements are represented in the diagram below.

11. The bright-line spectra produced by four elements are represented in the diagram below. 1. Which substance can not be broken down by a chemical change? A) ammonia B) ethanol C) propanal D) zirconium 2. Which particle has no charge? A) electron B) neutron C) positron D) proton 3. Which phrase

More information

Test Review # 4. Chemistry: Form TR4-9A

Test Review # 4. Chemistry: Form TR4-9A Chemistry: Form TR4-9A REVIEW Name Date Period Test Review # 4 Location of electrons. Electrons are in regions of the atom known as orbitals, which are found in subdivisions of the principal energy levels

More information

5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons

5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons 1. Which substance can be decomposed by a chemical change? (A) beryllium (B) boron (C) methanol (D) magnesium 2. The particles in a crystalline solid are arranged (A) randomly and far apart (B) randomly

More information

Part I Assignment: Electron Configurations and the Periodic Table

Part I Assignment: Electron Configurations and the Periodic Table Chapter 11 The Periodic Table Part I Assignment: Electron Configurations and the Periodic Table Use your periodic table and your new knowledge of how it works with electron configurations to write complete

More information

Homework Packet Unit 2. b. Al 3+, F, Na +, Mg 2+, O 2

Homework Packet Unit 2. b. Al 3+, F, Na +, Mg 2+, O 2 Name Period Homework Packet Unit 2 1. Which of the following is the correct empirical formula for a compound that has 37.5% C, 12.6% H, and 49.9% O? (A) C 2 H 4 O (B) CH 4 O 2 (C) CH 5 O 2 (D) CH 4 O (E)

More information

Full file at

Full file at 16 Chapter 2: Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element. a.

More information

Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements

Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain

More information

Bonding Mrs. Pugliese. Name March 02, 2011

Bonding Mrs. Pugliese. Name March 02, 2011 Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest

More information

Test Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.

Test Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles. Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1

More information

Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass

Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Elemental Properties Review Worksheet Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Periodic Table 1. List the element symbols for the following

More information

Chapter 2: Atoms and the Periodic Table

Chapter 2: Atoms and the Periodic Table 1. Which element is a nonmetal? A) K B) Co C) Br D) Al Ans: C Difficulty: Easy 2. Which element is a metal? A) Li B) Si C) Cl D) Ar E) More than one of the elements above are metals. 3. Which element is

More information

Ch. 3 Answer Key. O can be broken down to form two atoms of H and 1 atom of O. Hydrogen and oxygen are elements.

Ch. 3 Answer Key. O can be broken down to form two atoms of H and 1 atom of O. Hydrogen and oxygen are elements. Ch. 3 Answer Key 1. The Greeks believed that all matter is made of elements. We currently believe the same thing. However, the Greeks believed that there were 4 elements: earth, water, air and fire. Instead,

More information

Periodic Table of Elements

Periodic Table of Elements Periodic Table of Elements chlorine nitrogen helium gold oxygen silver mercury hydrogen neodymium sodium niobium carbon Elements Science has come along way since Aristotle s theory of Air, Water, Fire,

More information

Searching for an Organizing Principle. Searching for an Organizing Principle. How did chemists begin to organize the known elements?

Searching for an Organizing Principle. Searching for an Organizing Principle. How did chemists begin to organize the known elements? Searching for an Organizing Principle Searching for an Organizing Principle How did chemists begin to organize the known elements? Searching for an Organizing Principle A few elements, including copper,

More information

Chemistry B11 Chapter 3 Atoms

Chemistry B11 Chapter 3 Atoms Chapter 3 Atoms Element: is a substance that consists of identical atoms (hydrogen, oxygen, and Iron). 116 elements are known (88 occur in nature and chemist have made the others in the lab). Compound:

More information

Part A Unit-based exercise

Part A Unit-based exercise Topic 2 Microscopic World I / Microscopic World (Combined Science) Part A Unit-based exercise Unit 5 Atomic structure Fill in the blanks 1 atoms 2 solids; liquids; gases 3 metals; metalloids; non-metals

More information

Identify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom

Identify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom Semester Review What happens to electronegativity down a group? electrons for aluminum Identify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom Circle

More information

A sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature.

A sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature. Semester Review A sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature. 1.83 g/l Describe what defines an element s

More information

Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements

Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain

More information

Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions

Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements Multiple Choice Questions 1) In a chemical reaction, matter is neither created or destroyed. Which law does this refer to? A) Law

More information

Chemistry Study Guide

Chemistry Study Guide Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion

More information

Name Date Class ORGANIZING THE ELEMENTS

Name Date Class ORGANIZING THE ELEMENTS 6.1 ORGANIZING THE ELEMENTS Section Review Objectives Explain how elements are organized in a periodic table Compare early and modern periodic tables Identify three broad classes of elements Vocabulary

More information

Note Taking Guide: Episode 401. arranged elements by. predicted of missing. discovered that each has a unique. arranged elements by

Note Taking Guide: Episode 401. arranged elements by. predicted of missing. discovered that each has a unique. arranged elements by Note Taking Guide: Episode 401 Dmitri Mendeleev: arranged elements by. predicted of missing. Henry Moseley: discovered that each has a unique. arranged elements by. now all elements fit into place based

More information

Advanced Chemistry. Mrs. Klingaman. Chapter 5: Name:

Advanced Chemistry. Mrs. Klingaman. Chapter 5: Name: Advanced Chemistry Mrs. Klingaman Chapter 5: The Periodic Law Name: _ Mods: Chapter 5: The Periodic Law Reading Guide 5.1 History of the Periodic Table (pgs. 125-129) 1) What did Dimitri Mendeleev notice

More information

Unit 02 Review: Atomic Theory and Periodic Table Review

Unit 02 Review: Atomic Theory and Periodic Table Review Practice Multiple Choice Questions Unit 02 Review: Atomic Theory and Periodic Table Review 1. The number of neutrons in an atom of radioactive C 14 is: a) 6 c) 8 b) 12 d) 14 2. When a radioactive nucleus

More information

UNIT (2) ATOMS AND ELEMENTS

UNIT (2) ATOMS AND ELEMENTS UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In nature, sulfur is most commonly found in. 1) A) pure elemental sulfur B) H2S C) sulfuric

More information

Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals

More information

Name Midterm Review Date

Name Midterm Review Date Name Midterm Review Date 1. In which process does a solid change directly into a vapor? A) sublimation B) deposition C) condensation D) solidification 2. What is the molecular formula of a compound that

More information

2. Which of the following salts form coloured solutions when dissolved in water? I. Atomic radius II. Melting point III.

2. Which of the following salts form coloured solutions when dissolved in water? I. Atomic radius II. Melting point III. 1. Which pair of elements reacts most readily? A. Li + Br 2 B. Li + Cl 2 C. K + Br 2 D. K + Cl 2 2. Which of the following salts form coloured solutions when dissolved in water? I. ScCl 3 II. FeCl 3 III.

More information

UNIT 5.1. Types of bonds

UNIT 5.1. Types of bonds UNIT 5.1 Types of bonds REVIEW OF VALENCE ELECTRONS Valence electrons are electrons in the outmost shell (energy level). They are the electrons available for bonding. Group 1 (alkali metals) have 1 valence

More information

CHAPTER NOTES CHAPTER 14. Chemical Periodicity

CHAPTER NOTES CHAPTER 14. Chemical Periodicity Goals : To gain an understanding of : 1. Electron configurations 2. Periodicity. CHAPTER NOTES CHAPTER 14 Chemical Periodicity The periodic law states that when the elements are arranged according to increasing

More information

Chemistry CRT Study Guide First Quarter

Chemistry CRT Study Guide First Quarter Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry

More information

Chapter 2: Atoms and the Periodic Table

Chapter 2: Atoms and the Periodic Table 1. Which element is a nonmetal? A) K B) Co C) Br D) Al Ans: C Difficulty: Easy 2. Which element is a metal? A) Li B) Si C) Cl D) Ar E) More than one of the elements above is a metal. Ans: A Difficulty:

More information

6.3 Classifying Elements with the Periodic Table

6.3 Classifying Elements with the Periodic Table 6.3 Classifying Elements with the Periodic Table The Periodic Table was developed by scientists to organize elements in such a way as to make sense of the growing information about their properties. The

More information

Questions 1 to 58 must be answered on the Scantron sheets.

Questions 1 to 58 must be answered on the Scantron sheets. Questions 1 to 58 must be answered on the Scantron sheets. Base your answers to questions 1 to 5 on the heating curve for a pure substance that is shown below. 1. The freezing point of the substance is

More information

Chapter 2: Atoms. 2.1 (a) NaClO3 (b) AlF (a) The mass number is = 31. (b) The mass number is = 222.

Chapter 2: Atoms. 2.1 (a) NaClO3 (b) AlF (a) The mass number is = 31. (b) The mass number is = 222. 2.1 (a) NaClO3 (b) AlF3 2.2 (a) The mass number is 15 + 16 = 31. (b) The mass number is 86 + 136 = 222. 2.3 (a) The element has 15 protons, making it phosphorus (P); its symbol is 31 P 15. (b) The element

More information

Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements

Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain

More information

084f39de - Page 1. Name: 1) An example of a binary compound is A) potassium chlorate B) potassium chloride C) ammonium chloride D) ammonium chlorate

084f39de - Page 1. Name: 1) An example of a binary compound is A) potassium chlorate B) potassium chloride C) ammonium chloride D) ammonium chlorate Name: 1) An example of a binary compound is A) potassium chlorate B) potassium chloride C) ammonium chloride D) ammonium chlorate 2) What is the chemical formula for nitrogen (I) oxide? NO 3) What is the

More information

Unit 3. Atoms and molecules

Unit 3. Atoms and molecules Unit 3. Atoms and molecules Index. s and compounds...2.. Dalton's Atomic theory...2 2.-The atom...2 3.-Atomic number and mass number...2 4.-Isotopes, atomic mass unit and atomic mass...3 5.- configuration...3

More information

Unit 2 Review Please note that this does not start on question 1.

Unit 2 Review Please note that this does not start on question 1. Unit 2 Review Please note that this does not start on question 1. 21. Of the three particles; protons, neutrons, and electrons, which one(s) are responsible for most of the mass of an atom? a) the protons

More information

Discovery of Elements. Dmitri Mendeleev Stanislao Canizzaro (1860) Modern Periodic Table. Henry Moseley. PT Background Information

Discovery of Elements. Dmitri Mendeleev Stanislao Canizzaro (1860) Modern Periodic Table. Henry Moseley. PT Background Information Discovery of Elements Development of the Periodic Table Chapter 5 Honors Chemistry 412 At the end of the 1700 s, only 30 elements had been isolated Included most currency metals and some nonmetals New

More information

Electronic Structure and Bonding Review

Electronic Structure and Bonding Review Name: Band: Date: Electronic Structure and Bonding Review 1. For electrons: a. What is the relative charge? b. What is the relative mass? c. What is the symbol? d. Where are they located in the modern

More information

Bonding Practice Problems

Bonding Practice Problems NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which

More information

Chapter 3-1. proton positive nucleus 1 amu neutron zero nucleus 1 amu electron negative on energy levels around the nucleus very small

Chapter 3-1. proton positive nucleus 1 amu neutron zero nucleus 1 amu electron negative on energy levels around the nucleus very small Chapter 3-1 Sub-atomic Charge Location Mass Particle proton positive nucleus 1 amu neutron zero nucleus 1 amu electron negative on energy levels around the nucleus very small The most mass of the atom

More information

Honors Chemistry Unit 4 ( )

Honors Chemistry Unit 4 ( ) Honors Chemistry Unit 4 (2017-2018) Families (research and present) Metals/nonmetals Trends o Atomic radius o Electronegativity o Ionization energy o Metallic and nonmetallic character Review Ions Oxidation

More information

Honors Chemistry - Unit 4 Bonding Part I

Honors Chemistry - Unit 4 Bonding Part I Honors Chemistry - Unit 4 Bonding Part I Unit 4 Packet - Page 1 of 8 Vocab Due: Quiz Date(s): Test Date: UT Quest Due: Bonding Vocabulary: see separate handout assignment OBJECTIVES: Chapters 4-8 Be able

More information

b. Na. d. So. 1 A basketball has more mass than a golf ball because:

b. Na. d. So. 1 A basketball has more mass than a golf ball because: Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the

More information

Name: Midterm Review Date:

Name: Midterm Review Date: Name: Midterm Review Date: 1. Which statement concerning elements is true? A) Different elements must have different numbers of isotopes. B) Different elements must have different numbers of neutrons.

More information

5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d.

5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d. 1 c E = h 1. Sodium and potassium have similar properties because they have the same a. atomic radii. c. number of valence electrons. b. ionization energy. d. electronegativity. 2. Electrons must be added

More information

Chapter 2: Atoms. 2.1 (a) NaClO 3 (b) AlF (a) The mass number is = 31. (b) The mass number is = 222.

Chapter 2: Atoms. 2.1 (a) NaClO 3 (b) AlF (a) The mass number is = 31. (b) The mass number is = 222. 2.1 (a) NaClO 3 (b) AlF 3 2.2 (a) The mass number is 15 + 16 = 31. (b) The mass number is 86 + 136 = 222. 2.3 (a) The element has 15 protons, making it phosphorus (P); its symbol is 31 P 15. (b) The element

More information

MODULE-21 TRENDS IN THE MODERN PERIODIC TABLE

MODULE-21 TRENDS IN THE MODERN PERIODIC TABLE MODULE-21 TRENDS IN THE MODERN PERIODIC TABLE Valency is defined as the number of electrons an atom requires to lose, gain, or share in order to complete its valence shell to attain the stable noble gas

More information

1 Arranging the Elements

1 Arranging the Elements CHAPTER 11 1 Arranging the Elements SECTION The Periodic Table BEFORE YOU READ After you read this section, you should be able to answer these questions: How are elements arranged on the periodic table?

More information

CHAPTER 6 The Periodic Table

CHAPTER 6 The Periodic Table CHAPTER 6 The Periodic Table 6.1 Organizing the Elements Mendeleev: listed the elements in order of increasing atomic mass and in vertical columns according to their properties. Left blank spaces for undiscovered

More information

Unit 5. The Periodic Table

Unit 5. The Periodic Table Unit 5 The Periodic Table I. Development of Periodic Table Periodic law: when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern.

More information

Bonding Practice Exam

Bonding Practice Exam Bonding Practice Exam Matching Match each item with the correct statement below. a. halide ion e. valence electron b. octet rule f. coordination number c. ionic bond g. metallic bond d. electron dot structure

More information

-discovered set of patterns that applied to all elements published 1st periodic table. -wrote properties of each on note cards (density, color)

-discovered set of patterns that applied to all elements published 1st periodic table. -wrote properties of each on note cards (density, color) Dmitri Mendeleev -discovered set of patterns that applied to all elements -1869 published 1st periodic table -total of 63 elements discovered -wrote properties of each on note cards (density, color) -noticed

More information

Periodic Trends. Slide 1 / 102. Slide 2 / 102. Slide 3 / 102. AP Chemistry. The Periodic Law. New Jersey Center for Teaching and Learning

Periodic Trends. Slide 1 / 102. Slide 2 / 102. Slide 3 / 102. AP Chemistry. The Periodic Law. New Jersey Center for Teaching and Learning New Jersey Center for Teaching and Learning Slide 1 / 102 Progressive Science Initiative This material is made freely available at www.njctl.org and is intended for the non-commercial use of students and

More information

Mendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the

Mendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the Periodic Table Mendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the very stable copper, in the same family.

More information

Nihal İKİZOĞLU. MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements) kimyaakademi.com 1

Nihal İKİZOĞLU. MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements) kimyaakademi.com 1 MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements) kimyaakademi.com 1 PERIODS: Period number = Number of basic energy levels = The principal quantum number The horizontal lines

More information

MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements)

MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements) MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements) 1 PERIODS: Period number = Number of basic energy levels = The principal quantum number The horizontal lines in the periodic system

More information

Introduction: Pure Substances and. Mixtures, Elements and Compounds, Measurements and Units

Introduction: Pure Substances and. Mixtures, Elements and Compounds, Measurements and Units 1 Chemistry-2 Introduction: Pure Substances and Mixtures, Elements and Compounds, Measurements and Units 2 Properties of Matter Property that, which can be observed or measured. Intensive or Extensive:

More information

7. What is the likeliest oxidation number of an element located in Period 3 and Group 16? a. +2 b. +3 c. -3 d The amount of energy required to

7. What is the likeliest oxidation number of an element located in Period 3 and Group 16? a. +2 b. +3 c. -3 d The amount of energy required to 1. Which of the following is the most important factor in determining the properties of an element? a. Atomic mass b. Atomic radius c. Periodic table position d. Electron configuration 2. Similar properties

More information

Name Date Class THE PERIODIC TABLE

Name Date Class THE PERIODIC TABLE Name Date Class 6 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155 160) This section describes the development of the periodic table and explains the periodic law. It also describes the

More information

The Periodic Table & Formation of Ions

The Periodic Table & Formation of Ions The Periodic Table & Formation of Ions Development of the Periodic Table Mendeleev: Considered to be the father of the periodic table Arranged elements by increasing atomic mass Placed elements with similar

More information

Chapter 6: The Periodic Table

Chapter 6: The Periodic Table Chapter 6: The Periodic Table Name: Per: Test date: In-Class Quiz: Moodle Quiz: preap Learning Objectives Trace the historical development of the periodic table Identify the major groups and key features

More information

What is the smallest particle of the element gold (Au) that can still be classified as gold? A. atom B. molecule C. neutron D.

What is the smallest particle of the element gold (Au) that can still be classified as gold? A. atom B. molecule C. neutron D. Use the Periodic Table of Elements to answer the following question(s). Which sentence about the periodic table of elements is true? A. All elements in period 2 are metals. B. All elements in group 18

More information

End of Semester 1 Review

End of Semester 1 Review Name: ate: 1. In the modern Periodic Table, the elements are arranged in order of increasing. atomic number. mass number. oxidation number. valence number 5. Which element within any given period of the

More information

STRUCTURE AND BONDING

STRUCTURE AND BONDING NAME SCHOOL INDEX NUMBER DATE 1. 1989 Q 6 STRUCTURE AND BONDING The table below gives the distance between atoms (bond lengths) in halogen molecules and the energies required to break the bonds (bond energies)

More information

Developing the Periodic Table

Developing the Periodic Table Developing the Periodic Table Early Element Classification Mendeleev s First Periodic Table Mendeleev s First Periodic Table Mendeleev s Periodic Table Arranged by increasing atomic mass Some elements

More information