Atoms and the Periodic Table Study Guide
... Electrons 3) What two subatomic particles are responsible for the mass of the atom? ...
... Electrons 3) What two subatomic particles are responsible for the mass of the atom? ...
Notes
... -the number of protons in an atom of an element •all atoms of an element have the same atomic # •written as a subscript next to the element’s symbol •in a neutral atom, the number of protons is equal to the number of electrons (balanced charges). ...
... -the number of protons in an atom of an element •all atoms of an element have the same atomic # •written as a subscript next to the element’s symbol •in a neutral atom, the number of protons is equal to the number of electrons (balanced charges). ...
Worksheet 3.1 People Who Helped Develop the Modern Model of
... Ernest Rutherford: shot alpha particles through thin gold foil to show that the mass of the atom was concentrated in the middle, or nucleus, which is where the proton are. ...
... Ernest Rutherford: shot alpha particles through thin gold foil to show that the mass of the atom was concentrated in the middle, or nucleus, which is where the proton are. ...
Development of the Periodic Table
... ◦ Left blank spaces for elements which were not discovered yet ...
... ◦ Left blank spaces for elements which were not discovered yet ...
Periodic Table and Electrons
... The periodic table is arranged in order of increasing atomic numbers. The names of groups and periods on the periodic chart are alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. Metalloids have properties of metals and nonmetals. They are located between metals and ...
... The periodic table is arranged in order of increasing atomic numbers. The names of groups and periods on the periodic chart are alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. Metalloids have properties of metals and nonmetals. They are located between metals and ...
Chemistry - Spokane Public Schools
... An atom that has lost an electron becomes a positive ion because one of the positive protons in the nucleus is not being cancelled. An atom that has gained an electron becomes a negative ion because it has an extra negative electron that is not being cancelled by any proton. Ions are attracted to ea ...
... An atom that has lost an electron becomes a positive ion because one of the positive protons in the nucleus is not being cancelled. An atom that has gained an electron becomes a negative ion because it has an extra negative electron that is not being cancelled by any proton. Ions are attracted to ea ...
Lecture 1: Basic Concepts: Atoms and Bonding
... an electron than others. Each electron does, however, have a specific energy. Must solve wave equation for specific states! • The combination of the energy and probability gives rise to the current understanding for electron distributions, which are referred to as electron orbitals; these orbital ...
... an electron than others. Each electron does, however, have a specific energy. Must solve wave equation for specific states! • The combination of the energy and probability gives rise to the current understanding for electron distributions, which are referred to as electron orbitals; these orbital ...
Chapter 10_Handouts_6
... The electrons in an atom that have the same principal quantum number n occupy the same shell. The electrons in an atom that have the same orbital quantum number l occupy the same subshell. The larger the value of l, the more electrons the subshell can hold. A shell or subshell that contains its full ...
... The electrons in an atom that have the same principal quantum number n occupy the same shell. The electrons in an atom that have the same orbital quantum number l occupy the same subshell. The larger the value of l, the more electrons the subshell can hold. A shell or subshell that contains its full ...
Section 5.3
... “forced” to gain an electron by the addition of energy: • A + e - + E → A• The energy value is positive. Such ions are unstable, and will lose the electron spontaneously. ...
... “forced” to gain an electron by the addition of energy: • A + e - + E → A• The energy value is positive. Such ions are unstable, and will lose the electron spontaneously. ...
Chapter 10 Handouts_1
... low melting points.They are in group 1. •The alkaline earth metals are less active than the alkali metals. They are in group 2. •The inert gases are inactive nonmetals. They are in group 8 ...
... low melting points.They are in group 1. •The alkaline earth metals are less active than the alkali metals. They are in group 2. •The inert gases are inactive nonmetals. They are in group 8 ...
Chapter 10 Handouts - Bakersfield College
... low melting points.They are in group 1. •The alkaline earth metals are less active than the alkali metals. They are in group 2. •The inert gases are inactive nonmetals. They are in group 8 ...
... low melting points.They are in group 1. •The alkaline earth metals are less active than the alkali metals. They are in group 2. •The inert gases are inactive nonmetals. They are in group 8 ...
sch3u unit 1 test: matter
... 21. Which of the following always indicates that a chemical reaction has taken place? a. production of a gas b. absorption of heat c. change in colour d. appearance of a new substance ...
... 21. Which of the following always indicates that a chemical reaction has taken place? a. production of a gas b. absorption of heat c. change in colour d. appearance of a new substance ...
Atomic Theory: the beginning
... out experiments that allowed him to calculate the charge and mass of an ...
... out experiments that allowed him to calculate the charge and mass of an ...
Chapter One Outline
... The law of constant composition states that a chemical compound always contains the same elements in the same proportions by mass The Modern Atomic Theory ...
... The law of constant composition states that a chemical compound always contains the same elements in the same proportions by mass The Modern Atomic Theory ...
Midterm Review.ppt - Chemistry R: 4(AE)
... • Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms‘ 1. number of principal energy levels 2. number of valence electrons 3. atomic numbers 4. atomic masses ...
... • Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms‘ 1. number of principal energy levels 2. number of valence electrons 3. atomic numbers 4. atomic masses ...
Define:
... 78. Which subatomic particle plays the greatest part in determining the properties of an element? 79. Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant? 80. Consider an element Z that has two ...
... 78. Which subatomic particle plays the greatest part in determining the properties of an element? 79. Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant? 80. Consider an element Z that has two ...
Slide 1
... 20. Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms‘ 1. number of principal energy levels 2. number of valence electrons 3. atomic numbers 4. atomic masses ...
... 20. Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms‘ 1. number of principal energy levels 2. number of valence electrons 3. atomic numbers 4. atomic masses ...
Chapter 2
... understanding of atomic structure. 5. Distinguish between each of the following pairs of terms: a. neutron and proton b. atomic number and mass number c. atomic weight and mass number 6. Explain how the atomic number and mass number of an atom can be used to determine the number of neutrons. 7. Expl ...
... understanding of atomic structure. 5. Distinguish between each of the following pairs of terms: a. neutron and proton b. atomic number and mass number c. atomic weight and mass number 6. Explain how the atomic number and mass number of an atom can be used to determine the number of neutrons. 7. Expl ...
Rules for Naming Elements/Compounds
... • atomic number is the number located in the upper left corner • atomic weight is the number located on the bottom • krypton: ...
... • atomic number is the number located in the upper left corner • atomic weight is the number located on the bottom • krypton: ...
Name Objective 1: Matter and Energy C3H8 + 5O2 → 3CO2 + 4H2O
... 16. Which two compounds contain the same total number of atoms? (8.5D) a. C3H8 and C2H6 b. NO2 and KCl c. 2Li2S and Be4Cl2 d. 2CO and CO2 17. All of the following are indicators of a chemical change except — (8.5E) a. formation of a gas b. change in temperature c. change in the state of matter d. fo ...
... 16. Which two compounds contain the same total number of atoms? (8.5D) a. C3H8 and C2H6 b. NO2 and KCl c. 2Li2S and Be4Cl2 d. 2CO and CO2 17. All of the following are indicators of a chemical change except — (8.5E) a. formation of a gas b. change in temperature c. change in the state of matter d. fo ...
Study Guide.Ch.11and12.tst
... 1. In your own words, write a definition for the term periodic. 2. Compare a period and a group on the periodic table. What information do each of these provide? 3. What property did Mendeleev use to position the elements on the periodic table? How did Henry Mosely rearrange the periodic table? Whic ...
... 1. In your own words, write a definition for the term periodic. 2. Compare a period and a group on the periodic table. What information do each of these provide? 3. What property did Mendeleev use to position the elements on the periodic table? How did Henry Mosely rearrange the periodic table? Whic ...
Atomic Models
... - studied the ratios of elements in chemical reactions and came up with a theory about atoms Dalton’s Atomic Theory (text p. 63) 1. All matter consists of atoms which are tiny, _________________ particles of an element and cannot be ______________________________ 2. Atoms from one element are ______ ...
... - studied the ratios of elements in chemical reactions and came up with a theory about atoms Dalton’s Atomic Theory (text p. 63) 1. All matter consists of atoms which are tiny, _________________ particles of an element and cannot be ______________________________ 2. Atoms from one element are ______ ...
Periodic table
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The periodic table is a tabular arrangement of the chemical elements, ordered by their atomic number (number of protons in the nucleus), electron configurations, and recurring chemical properties. The table also shows four rectangular blocks: s-, p- d- and f-block. In general, within one row (period) the elements are metals on the lefthand side, and non-metals on the righthand side.The rows of the table are called periods; the columns are called groups. Six groups (columns) have names as well as numbers: for example, group 17 elements are the halogens; and group 18, the noble gases. The periodic table can be used to derive relationships between the properties of the elements, and predict the properties of new elements yet to be discovered or synthesized. The periodic table provides a useful framework for analyzing chemical behavior, and is widely used in chemistry and other sciences.Although precursors exist, Dmitri Mendeleev is generally credited with the publication, in 1869, of the first widely recognized periodic table. He developed his table to illustrate periodic trends in the properties of the then-known elements. Mendeleev also predicted some properties of then-unknown elements that would be expected to fill gaps in this table. Most of his predictions were proved correct when the elements in question were subsequently discovered. Mendeleev's periodic table has since been expanded and refined with the discovery or synthesis of further new elements and the development of new theoretical models to explain chemical behavior.All elements from atomic numbers 1 (hydrogen) to 118 (ununoctium) have been discovered or reportedly synthesized, with elements 113, 115, 117, and 118 having yet to be confirmed. The first 94 elements exist naturally, although some are found only in trace amounts and were synthesized in laboratories before being found in nature. Elements with atomic numbers from 95 to 118 have only been synthesized in laboratories. It has been shown that einsteinium and fermium once occurred in nature but currently do not. Synthesis of elements having higher atomic numbers is being pursued. Numerous synthetic radionuclides of naturally occurring elements have also been produced in laboratories.