Questions and Answers
What is the average atomic mass given in the content?
35.45 amu
What is the percent abundance of boron-11?
80%
The mass of boron-11 is ______ amu.
11.009306
The mass of boron-10 is ______ amu.
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What equation is used to calculate average atomic mass using isotopes?
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How do the percentages of the isotopes relate to each other?
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How many protons are in an atom of sodium?
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How many electrons are in an atom of bromine?
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How many electrons are in an atom of nickel?
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How many protons are in an atom of radon?
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How many neutrons are in an atom of potassium-40?
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How is the atomic number related to the number of protons in an atom?
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How is the mass number of an atom related to the number of neutrons?
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How many protons, electrons, and neutrons are in an atom of copper-63?
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An atom has a mass number of 14 and 6 electrons. How many protons and neutrons does it have?
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An atom has 40 electrons and 51 neutrons. What is its mass number, and how many protons does it have?
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What does the top number in isotope notation represent?
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What does the bottom number in isotope notation represent?
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How many protons and neutrons are in ¹⁸₉F?
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How many protons and neutrons are in ²⁵₁₁ Na?
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What is the isotope notation for an atom of carbon-12?
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What is the isotope notation for an atom of chlorine-37?
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What is the name of Ar?
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How does an ion differ from an atom of the same element with regard to the numbers of subatomic particles?
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When two atoms or ions have the same number of electrons, they're said to be __________.
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When an ion has a positive charge, how do the numbers of subatomic particles differ?
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When an ion has a negative charge, how do the numbers of subatomic particles differ?
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How many protons and electrons does ⁴⁰₂₀C²⁺ have?
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How many protons and electrons does ¹³¹₅₃I¹⁻ have?
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How many protons and electrons does ³⁰₁₃Al³⁺ have?
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How many protons and electrons does ³³P ³⁻ have?
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What is the isotope notation for an ion of silver-109 with a charge of positive 1?
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What is the isotope notation for an ion of sulfur-34 with a charge of negative 2?
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How many protons, neutrons, and electrons are in ⁵²Cr ⁶⁺?
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How many protons, neutrons, and electrons are in ⁶²Ni ³⁺?
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What is the name of the premise that one electron fills each orbital in a subshell until all orbitals contain one electron?
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What rule or principle describes the order in which electrons fill orbitals?
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What is the maximum number of electrons that can be in the f orbitals?
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What is the maximum number of electrons that can be in the p orbitals?
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What is the electron configuration of carbon?
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What is the electron configuration of magnesium?
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What is the electron configuration of argon?
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What is the electron configuration of bromine?
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What is the electron configuration of zirconium?
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What is the expected electron configuration of plutonium?
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Which quantum number describes the spin of the electron?
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Which quantum number describes the average distance between the nucleus and the orbital?
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Which quantum number describes how the various orbitals are oriented in space?
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Which quantum number describes the shape of the orbital?
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What are the possible values for the spin quantum number?
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The decimal numbers in the blocks of the periodic table represent the __________.
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What is the average atomic mass of lithium that is 7.59% lithium-6 and 92.41% lithium-7?
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Study Notes
Atomic Structure
- Sodium (Na) has 11 protons, equal to its atomic number.
- Bromine (Br) has 35 protons and 35 electrons, making it a neutral atom.
- Nickel (Ni) contains 28 electrons, matching its 28 protons.
- Radon (Rn) has 86 protons as its atomic number indicates.
Neutrons and Isotopes
- Potassium-40 has 21 neutrons calculated by subtracting its atomic number (19) from its mass number (40).
- Copper-63 has 29 protons, 29 electrons, and 34 neutrons (63 - 29).
- An atom with a mass number of 14 and 6 electrons has 6 protons and 8 neutrons (14 - 6).
- An atom with 40 electrons and 51 neutrons has a mass number of 91, revealing it has 40 protons.
Isotope Notation
- The top number in isotope notation represents the mass number.
- The bottom number represents the number of protons (atomic number).
- ¹⁸₉F has 9 protons and 9 neutrons (18 - 9).
- ²⁵₁₁Na has 11 protons and 14 neutrons (25 - 11).
- Carbon-12 is denoted as ¹²₆C in isotope notation.
Ions and Charges
- Ions differ from neutral atoms by having unequal numbers of protons and electrons.
- Isoelectronic refers to atoms/ions having the same number of electrons.
- A positively charged ion has more protons than electrons; a negatively charged ion has more electrons than protons.
Subatomic Particles in Ions
- ⁴⁰₂₀C²⁺ has 20 protons and 18 electrons (20 - 2 due to charge).
- ¹³¹₅₃I¹⁻ has 53 protons and 54 electrons (53 + 1 due to charge).
- ³⁰₁₃Al³⁺ contains 13 protons and 10 electrons (13 - 3 due to charge).
- ³³P³⁻ has 15 protons and 18 electrons (15 + 3 due to charge).
Electron Configuration
- Hund's rule states each orbital in a subshell fills singly before pairing starts.
- The Aufbau principle dictates the order in which electrons fill orbitals based on energy levels.
- Maximum electrons in f orbitals: 14; in p orbitals: 6.
- Carbon’s electron configuration is 1s²2s²2p², totaling 6 electrons.
Average Atomic Mass
- Average atomic mass is calculated using relative abundances and isotopic masses.
- Lithium's average atomic mass calculated from isotopes is 6.940 amu.
- Chlorine's average atomic mass calculated from isotopes is 35.45 amu.
- Percent abundance for boron-11 when given average atomic mass involves creating and solving a related equation.
Quantum Numbers
- The spin quantum number (s) describes an electron's spin direction.
- The principal quantum number (n) indicates average distance from nucleus to orbital.
- The magnetic quantum number (ml) describes orientation of orbitals in space.
- The angular momentum quantum number (l) describes the shape of the orbital.
- Spin quantum number values are -1/2 and 1/2, indicating two spin directions.
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Description
This quiz focuses on the concepts of average atomic mass, specifically related to boron isotopes. You will be tested on the percent abundance of boron-11, the masses of boron-10 and boron-11, and the equation used to calculate average atomic mass using isotopes. Additionally, you'll explore how the percentages of isotopes relate to each other.