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Name:___________________________________ Mrs. Bonanno Honors Chemistry Pearl River High School Unit 6 – The Atom Vocabulary: Atom:____________________________________________________________________________________ Nucleus:__________________________________________________________________________________ Neutrons:_________________________________________________________________________________ Protons:__________________________________________________________________________________ Electrons:_________________________________________________________________________________ Nucleons:_________________________________________________________________________________ Atomic Mass:______________________________________________________________________________ Atomic Number:____________________________________________________________________________ Isotopes:__________________________________________________________________________________ Ground State:______________________________________________________________________________ Excited State:______________________________________________________________________________ Ions:_____________________________________________________________________________________ Bright line Spectra:__________________________________________________________________________ 1 Do Now 1 Do Now 5 Do Now 2 Do Now 6 Do Now 3 Do Now 7 Do Now 4 Do Now 8 2 Do Now 9 Do Now 12 Do Now 10 Do Now 13 Do Now 11 Do Now 14 3 1) Subatomic Particles a) All atoms are composed of a _______________, _____________, _________________ charged nucleus that is surrounded by a _________________________ occupied by __________________. b) The nucleus contains ____________________. There are two types of nucleons: i) Protons = ___________________________ ii) Neutrons =__________________________ c) Electrons: i) Occupy the space __________________________________ ii) Have a charge equal to, but opposite of, a proton. (1) Therefore, an electron is _________________________ charged. d) Diagram an atom: a) Elements on the Periodic Table: a) Atomic Number:_______________________________________________ b) Atomic Mass:_________________________________________________ c) Examples: Carbon Flourine Oxygen 2) Atomic Mass Unit a) The mass of a proton is only ____________________________________ b) Since the mass is so small we use a different scale called ____________________________________, to represent mass. c) Protons: i) The mass of a proton = _________________________ 4 d) Neutrons: i) The mass of a neutron is approximately the same as a proton so its mass is _____________ e) Electrons: i) Much ____________ massive than a proton or neutron. ii) Its mass is only ____________ amu f) Selected Subatomic Particles: Particle Charge Mass Location Symbol Proton Neutron Electron Practice Questions: 1) The atomic number of any atom is equal to the number of 1. neutrons in the atom, only 2. protons in the atom, only 3. neutrons plus protons in the atoms 4. protons plus electrons in the atom 2) What is the symbol for an atom containing 20 protons and 22 neutrons? 1. 2. 3. 4. 3) Which statement best describes an electron? 1. It has a smaller mass than a proton and a negative charge. 2. It has a smaller mass than a proton and a positive charge. 3. It has a greater mass than a proton and a negative charge. 4. It has a greater mass than a proton and a positive charge. 4) What is the mass number of an atom which contains 28 protons, 28 electrons and 34 neutrons? 1. 28 2. 56 3. 62 4. 90 5 5) What is the total number of electrons present in an atom of 1. 27 2. 32 3. 39 4. 86 ? 6) How many protons are in the nucleus of an atom of beryllium? 1. 5 2. 2 3. 9 4. 4 7) Which particles account for most of the mass of the atom? 1. protons and neutrons 2. protons and electrons 3. neutrons and electrons 4. neutrons and positrons 8) Compared to the entire atom, the nucleus of the atom is 1. smaller and contains most of the atom’s mass 2. smaller and contains little of the atom’s mass 3. larger and contains most of the atom’s mass 4. larger and contains little of the atom’s mass 9) An electron has a charge of 1. −1 and the same mass as a proton 2. +1 and the same mass as a proton 3. −1 and a smaller mass than a proton 4. +1 and a smaller mass than a proton 10) Which species contains only 12 nucleons in the nucleus? 1. 2. 3. 4. 11) Which particle has a mass of approximately one atomic mass unit and a unit positive charge? 1. a neutron 2. a proton 3. a beta particle 4. an alpha particle 12) What is the total number of neutrons in an atom of 1. 82 2. 125 3. 207 4. 289 ? 6 Atom # Protons # Neutrons # Electrons Mass Number Atomic Number Nuclear Charge # Nucleons Sb C Mg Pb Pt F Ba Bi Cm Si 7 3) Isotopes a) ___________________ of a given element must contain the _____________ number of protons. b) However, the number of ______________________________________ i) Isotopes: Atoms of the ________________________ that have different numbers of _____________ (1) Therefore, isotopes have different _____________ numbers! (2) Isotopes of Hydrogen: Particle Protons Protium 1 Neutrons Symbol 1 amu Deuterium Tritium Mass Number 1 1 2 amu 2 c) Identifying Isotopes i) Isotopes are written by using elements ________________ and its _________________________ C-13 Cl – 37 Na - 22 d) Atomic Masses i) In order to determine the atomic mass of an element, you must ______________________________ of all the _____________________ of that ________________________ ii) Examples: 1) Carbon has ________________________ occurring stable isotopes. Most carbon atoms, 98.89%, are C-12 while the remaining 1.108% are C-13. What is the atomic mass of carbon? 8 2) Example: Base your answer on the data table, which shows three isotopes of neon. Based on natural abundances, what is the average atomic mass of neon? 3) Naturally occurring elemental carbon is a mixture of isotopes. The percent composition of the two most abundant isotopes is listed below. 98.93% of the carbon atoms have a mass of 12.00 atomic mass units. 1.07% of the carbon atoms have a mass of 13.00 atomic mass units. What is the average atomic mass of carbon? 4) Atoms of the same element that have different numbers of neutrons are classified as 1. charged atoms 2. charged nuclei 3. isomers 4. isotopes 5) All the isotopes of a given atom have 1. the same mass number and the same atomic number 2. the same mass number but different atomic numbers 3. different mass numbers but the same atomic number 4. different mass numbers and different atomic numbers 6) The atomic mass of an element is defined as the weighted average mass of that element’s 1. most abundant isotope 2. least abundant isotope 3. naturally occuring isotopes 4. radioactive isotopes 9 7) An atom that contains 8 protons, 8 electrons, and 9 neutrons has 1. an atomic number of 9 2. an atomic number of 16 3. a mass number of 17 4. a mass number of 25 8) Which two atoms are isotopes? 1. 2. and and 3. and 4. and 9) Neutral atoms of 35Cl and 37Cl differ with respect to their number of 1. electrons 2. protons 3. neutrons 4. positrons 10) What is the structure of a krypton-85 atom? 1. 49 electrons, 49 protons, and 85 neutrons 2. 49 electrons, 49 protons, and 49 neutrons 3. 36 electrons, 36 protons, and 85 neutrons 4. 36 electrons, 36 protons, and 49 neutrons 11) An atom of carbon-14 contains 1. 8 protons, 6 neutrons and 6 electrons 2. 6 protons, 6 neutrons and 8 electrons 3. 6 protons, 8 neutrons and 8 electrons 4. 6 protons, 8 neutrons and 6 electrons 10 Complete the following sentences: 1. Atoms are composed of ________________, _________________, and ________________. 2. The ________________ & ______________ are located in the nucleus, while the _____________ are outside of the nucleus. 3. Atoms are mostly ___________________________. 4. The number of protons is referred to as the __________________ for the atom. 5. All atoms of the same element have the same number of __________________. 6. Isotopes have the same number of ___________________, but a different number of ____________________. 7. The mass number of an element is the total number of ________________ & _________________. 8. Why is the atomic mass of an element given in decimal form in the periodic table? ________________________________________________ 11 Determining the number of electrons: a) Neutral atom ii) The number of protons is exactly _______________ to the number of electrons. iii) So the number of ________________ is the same as the _______________ number. b) Charged Atom = Ion i) Ion = charged particles created when an atom____________________________ electrons, giving it a charge!!! ii) Ions are written with a __________ and the _____________________ that were removed or gained. iii) If the charge is positive, electrons were ____________________ (1) ______________________ always lose their electrons! So metals always have a ____ charge. (a) Examples: iv) If the charge is negative, electrons were ____________________ (1) ____________________ always gain electrons! So nonmetals always have a ______ charge. (a) Examples: Practice: 1) The total number of electrons in a neutral atom of every element is always equal to the atom’s 1. mass number 2. number of neutrons 3. number of protons 4. number of nucleons 2) What is the total number of electrons in a Cu+ ion? 1. 28 2. 29 3. 30 4. 36 3) What is the total number of protons in the nucleus of an F− ion? 1. 8 2. 9 3. 10 4. 11 4) An ion with 5 protons, 6 neutrons, and a charge of 3+ has an atomic number of 1. 5 2. 6 3. 8 4. 11 5) As a Ca atom undergoes oxidation to Ca2+, the number of neutrons in its nucleus 1. decreases 2. increases 3. remains the same 12 c) Location of Electrons (Based on Wave Mechanical Model) c) Electrons are found in the _______________ around the nucleus called ____________________ d) Orbitals are arranged by energy levels, each containing a ________________________________ i) The first orbital is called the __________________________ (1) The first energy level contains a maximum of __________________ ii) The second orbital is called the ________________________ (1) The second energy level contains a maximum of _______________ iii) The third orbital is called the __________________________ (1) The third energy level contains a maximum of _________________ iv) The fourth orbital is called the _________________________ (1) The fourth energy level contains a maximum of ________________ d) Electron Configuration i) Tells how many electrons an atom of a specific element has. ii) Listed on the periodic table for each element on the bottom left corner. iii) Listed in order of energy levels (1) Example: 13 iv) The outer most electrons are called the valence electrons (1) Example: Na v. S Determine the electron configuration for the following ions: a. B+ ____________________ b. Cl- ____________________ c. Ca2+____________________ d. O3- ____________________ Practice Questions 1) Which electron configuration is correct for a sodium ion? 1. 2–7 2. 2–8 3. 2–8–1 4. 2–8–2 2) A particle of matter contains six protons, seven neutrons, and six electrons. This particle must be a 1. neutral carbon atom 2. neutral nitrogen atom 3. positively charged carbon ion 4. positively charged nitrogen ion 3) Compared to an element of calcium-40, an atom of potassium-39 contains fewer 1. protons 2. neutrons 3. occupied sublevels 4. occupied principal energy levels 4) Which particle contains the greatest number of electrons? 1. Na 2. Na+ 3. F 4. F- 14 e) Ground and Excited States c) Electrons are able to gain or lose energy which allows them to move to different energy levels. i) How it works: (1) Electrons __________________________, allowing it to move to a higher energy level. (2) Electrons __________________________, allowing them to move down to a lower energy level. (a) The energy given off could be infrared, ultraviolet, or visible light. d) Ground State i) When electrons occupy the __________________________, it is in the ground state. e) Excited State i) Electrons may _______________________ and temporarily move to a _____________ energy level. (1) This could be due to _____________________________________________ (2) This unstable state is called the ______________________________ ii) After the electron quickly returns to the _______________________, it ____________ the same amount of energy it absorbed. (1) The energy given off is _________________________ that humans can see. (a) Although the light appears as ________________, it is actually composed of many ___________________ having different __________________ iii) Bright Line Spectra (1) A tool used to ____________________________ into narrow lines of color called the _____________________________ (2) This information about the bright line spectra is used to __________________________ 15 Practice Problems: 1) The bright-line spectra for three elements and a mixture of elements are shown below. Identify all the elements in the mixture. 2) Base your answer to this question on the information below. In a laboratory, a glass tube is filled with hydrogen gas at a very low pressure. When a scientist applies a high voltage between metal electrodes in the tube, light is emitted. The scientist analyzes the light with a spectroscope and observes four distinct spectral lines. The table below gives the color, frequency, and energy for each of the four spectral lines. The unit for frequency is hertz, Hz. Explain, in terms of subatomic particles and energy states, why light is emitted by the hydrogen gas. 16 Electron Configurations: Describe how _____________________ are arranged around the nucleus. Important because it helps us predict ________________________________ Learn the following pattern: Auf Bau Principle: Standard electron configuration: Examples: o Hydrogen: o Helium: o Lithium: o Boron: 17 o Neon: o Magnesium: o Sulfur: o Calcium: o Nickel: o Bromine: Orbital Diagrams: Hund’s Rule: Examples: o Carbon o Silicon o Iron 18