SCI 3101 Test IV MULTIPLE CHOICE. 1) The sky is blue because air
... D) Atomic mass, 99 amu; Technetium (Tc) 15) Why are the atomic masses listed in the periodic table not whole numbers? A) The atomic masses are average atomic masses. B) Scientists have yet to make the precise measurements. C) That would be too much of a coincidence. D) Today's instruments are able t ...
... D) Atomic mass, 99 amu; Technetium (Tc) 15) Why are the atomic masses listed in the periodic table not whole numbers? A) The atomic masses are average atomic masses. B) Scientists have yet to make the precise measurements. C) That would be too much of a coincidence. D) Today's instruments are able t ...
chemistry final - Madison Public Schools
... A. oxygen supports the burning of paper. B. oxygen reacts with sulfur to form sulfur dioxide C. oxygen has a density of 1.43 grams/ liter ...
... A. oxygen supports the burning of paper. B. oxygen reacts with sulfur to form sulfur dioxide C. oxygen has a density of 1.43 grams/ liter ...
Document
... 5. Know the locations and label the names for the following groups: 1, 2, 3-12, 13, 14, ...
... 5. Know the locations and label the names for the following groups: 1, 2, 3-12, 13, 14, ...
Key
... a) The orbitals b and c depicted above are what type? b) Which orbital would likely have the highest ionization energy? Question 14 4 Points ...
... a) The orbitals b and c depicted above are what type? b) Which orbital would likely have the highest ionization energy? Question 14 4 Points ...
Chapter 2 Notes
... 1. molecules- 2 or more atoms combined; atoms share electrons in the outermost portion of their electron clouds; example: (H2O) 2. compounds- when 2 or more substances combine chemically; has properties different from the properties of each of the elements in it; example: water (H2O) 3. chemical pro ...
... 1. molecules- 2 or more atoms combined; atoms share electrons in the outermost portion of their electron clouds; example: (H2O) 2. compounds- when 2 or more substances combine chemically; has properties different from the properties of each of the elements in it; example: water (H2O) 3. chemical pro ...
STUDY GUIDE for DIGESTION and NUTRITION
... Check off the box once you have studied and understand the concept ...
... Check off the box once you have studied and understand the concept ...
Advanced Placement (AP) Chemistry 2012 – 2013 Ramsay High
... the AP Chemistry Exam. Material once learned must be remembered all year long. Once materials have been covered, students are expected to retain information for use throughout the course. The laboratory requirements are met by requiring students to complete laboratory work during the school day, an ...
... the AP Chemistry Exam. Material once learned must be remembered all year long. Once materials have been covered, students are expected to retain information for use throughout the course. The laboratory requirements are met by requiring students to complete laboratory work during the school day, an ...
FE Review Chemistry - UTSA College of Engineering
... • Element: a substance only composed of one type of atom • Isotope: element with the same number of protons but different atomic masses ...
... • Element: a substance only composed of one type of atom • Isotope: element with the same number of protons but different atomic masses ...
Name: (1 of 2) Math Set # 13 Protons,
... now has a charge. For example, if a hydrogen atom has one proton (+) and one electron (-‐) the two charges cancel each other out. When the electron is lost the hydrogen atom is only a ...
... now has a charge. For example, if a hydrogen atom has one proton (+) and one electron (-‐) the two charges cancel each other out. When the electron is lost the hydrogen atom is only a ...
Exam Review - hrsbstaff.ednet.ns.ca
... The reaction of solutions of ammonium phosphate and barium nitrate gives a precipitate of barium phosphate. The equation that best represents this statement is a) 2(NH4)3PO4(s) + 3Ba(NO3)2(aq) → Ba3(PO4)2(aq) + 6NH4NO3(s). b) 2(NH4)3PO4(aq) + 3Ba(NO3)2(aq) → Ba3(PO4)2(s) + 6NH4NO3(aq). c) 2(NH4)3PO4 ...
... The reaction of solutions of ammonium phosphate and barium nitrate gives a precipitate of barium phosphate. The equation that best represents this statement is a) 2(NH4)3PO4(s) + 3Ba(NO3)2(aq) → Ba3(PO4)2(aq) + 6NH4NO3(s). b) 2(NH4)3PO4(aq) + 3Ba(NO3)2(aq) → Ba3(PO4)2(s) + 6NH4NO3(aq). c) 2(NH4)3PO4 ...
SCH 3U - othsmath
... 2) Going down a group, a new energy level is added with each subsequent atom, ensuring the valence electrons are moved further and further from the nucleus. This increases the shielding provided by non-valence electrons, decreases the ENC (even though the number of protons in the nucleus is increasi ...
... 2) Going down a group, a new energy level is added with each subsequent atom, ensuring the valence electrons are moved further and further from the nucleus. This increases the shielding provided by non-valence electrons, decreases the ENC (even though the number of protons in the nucleus is increasi ...
Introduction to Molecular Orbital Theory... in the molecular orbital
... Although the Lewis structure and molecular orbital models of oxygen yield the same bond order, there is an important difference between these models. The electrons in the Lewis structure are all paired, but therecould be unpaired electrons in the molecular orbital description of a molecule. As a res ...
... Although the Lewis structure and molecular orbital models of oxygen yield the same bond order, there is an important difference between these models. The electrons in the Lewis structure are all paired, but therecould be unpaired electrons in the molecular orbital description of a molecule. As a res ...
Name: Date: Period: Who is the Father of Atomic Theory? What
... 9. Why do elements in a group have similar chemical properties? 10. What can the number of valence electrons tell us about and element? 11. What is the most reactive group on the periodic table? The least? ...
... 9. Why do elements in a group have similar chemical properties? 10. What can the number of valence electrons tell us about and element? 11. What is the most reactive group on the periodic table? The least? ...
notes and handout
... from the valence electrons (#1 above). Arrange these around the atoms until all of them satisfy the octet rule: Remember, ALL elements EXCEPT hydrogen want eight electrons around them, total. Hydrogen only wants two electrons. Let's do an example: CO2 Note: Each of the numbers below correspond to ...
... from the valence electrons (#1 above). Arrange these around the atoms until all of them satisfy the octet rule: Remember, ALL elements EXCEPT hydrogen want eight electrons around them, total. Hydrogen only wants two electrons. Let's do an example: CO2 Note: Each of the numbers below correspond to ...
Name: Midterm Review (Part II) Fill in the blanks (Chapter 6.1 – 6.3
... Describe the trends in the atomic size of elements within groups? (Increase/Decrease down a group?) Describe the trends in the atomic size of elements across periods in the periodic table? (Increase/Decrease across the period?) Which element has the largest radius? Lithium, Sodium, Rubidium, Cesium ...
... Describe the trends in the atomic size of elements within groups? (Increase/Decrease down a group?) Describe the trends in the atomic size of elements across periods in the periodic table? (Increase/Decrease across the period?) Which element has the largest radius? Lithium, Sodium, Rubidium, Cesium ...
Answers to practice questions
... Standard 1.1 Analyze the structure of atoms and ions. _____ 1. As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is believed to be true? A) A model in which the protons, electrons and neutrons are evenly distributed throughout the volume of the atom. B) A model ...
... Standard 1.1 Analyze the structure of atoms and ions. _____ 1. As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is believed to be true? A) A model in which the protons, electrons and neutrons are evenly distributed throughout the volume of the atom. B) A model ...
CHEM 481. Assignment 0. Review of General Chemistry. Answers
... 27. What is Heisenberg’s uncertainty principle? Explain how it applies to our modern view of atomic structure. Heisenberg concluded that it was impossible to fix both the position of an electron in an atom and its energy with any degree of certainty. One way to understand this principle is that the ...
... 27. What is Heisenberg’s uncertainty principle? Explain how it applies to our modern view of atomic structure. Heisenberg concluded that it was impossible to fix both the position of an electron in an atom and its energy with any degree of certainty. One way to understand this principle is that the ...
Answers to Assignment #1
... 27. What is Heisenberg’s uncertainty principle? Explain how it applies to our modern view of atomic structure. Heisenberg concluded that it was impossible to fix both the position of an electron in an atom and its energy with any degree of certainty. One way to understand this principle is that the ...
... 27. What is Heisenberg’s uncertainty principle? Explain how it applies to our modern view of atomic structure. Heisenberg concluded that it was impossible to fix both the position of an electron in an atom and its energy with any degree of certainty. One way to understand this principle is that the ...
chapter 1 - Revsworld
... Which of the following statements is/are correct? I. When heat energy flows from a system to the surroundings, we know that the temperature of the system is greater than that of the surroundings. II. Given the thermochemical equation 4NH3(g) + 5O2(g) ------> 4 NO(g) + 6H2O(g) H = -906 kJ, the therm ...
... Which of the following statements is/are correct? I. When heat energy flows from a system to the surroundings, we know that the temperature of the system is greater than that of the surroundings. II. Given the thermochemical equation 4NH3(g) + 5O2(g) ------> 4 NO(g) + 6H2O(g) H = -906 kJ, the therm ...
Chapter 2
... Every atom has a characteristic total number of covalent bonds that it can form, equal to the number of unpaired electrons in the outermost shell. This bonding capacity is called the atom’s valence. o The valence of hydrogen is 1; oxygen is 2; nitrogen is 3; carbon is 4. o Phosphorus should have a v ...
... Every atom has a characteristic total number of covalent bonds that it can form, equal to the number of unpaired electrons in the outermost shell. This bonding capacity is called the atom’s valence. o The valence of hydrogen is 1; oxygen is 2; nitrogen is 3; carbon is 4. o Phosphorus should have a v ...
Molecular orbital diagram
A molecular orbital diagram, or MO diagram, is a qualitative descriptive tool explaining chemical bonding in molecules in terms of molecular orbital theory in general and the linear combination of atomic orbitals (LCAO) molecular orbital method in particular. A fundamental principle of these theories is that as atoms bond to form molecules, a certain number of atomic orbitals combine to form the same number of molecular orbitals, although the electrons involved may be redistributed among the orbitals. This tool is very well suited for simple diatomic molecules such as dihydrogen, dioxygen, and carbon monoxide but becomes more complex when discussing even comparatively simple polyatomic molecules, such as methane. MO diagrams can explain why some molecules exist and others do not. They can also predict bond strength, as well as the electronic transitions that can take place.