Fundamentals of Chemistry
... elements are chemically very active, some are not very active, and others are inert. • Group I has 1 valence electron, which makes it easy to loose that electron. Group VIIA has seven valence electrons and it only needs to gain one electron to become stable. • The more stable the resulting molecules ...
... elements are chemically very active, some are not very active, and others are inert. • Group I has 1 valence electron, which makes it easy to loose that electron. Group VIIA has seven valence electrons and it only needs to gain one electron to become stable. • The more stable the resulting molecules ...
Electrochemistry
... A. Any chemical process in which electrons are transferred from one atom to another is an _________-__________ reaction. 1. The name for this type of reaction is often shortened to what is called a ________ reaction. 2. A species _____ _________ when _______ (LEO). A species _____ ________ when ____ ...
... A. Any chemical process in which electrons are transferred from one atom to another is an _________-__________ reaction. 1. The name for this type of reaction is often shortened to what is called a ________ reaction. 2. A species _____ _________ when _______ (LEO). A species _____ ________ when ____ ...
File
... Thomson did experiments on the beams of particles in his tube. They were attracted to a positive charge, so Thomson correctly concluded that they must be negatively charged themselves. Other experiments showed that it would take about 2000 electrons to weigh the same as the lightest atom, hydrogen. ...
... Thomson did experiments on the beams of particles in his tube. They were attracted to a positive charge, so Thomson correctly concluded that they must be negatively charged themselves. Other experiments showed that it would take about 2000 electrons to weigh the same as the lightest atom, hydrogen. ...
Atomic Nature of Matter
... The isotopes of hydrogen are unique in that they are each commonly referred to by a unique name instead of the common chemical element name. Hydrogen-1 is almost always referred to as hydrogen, but the term protium is infrequently used also. Hydrogen-2 is commonly called deuterium and symbolized 21D ...
... The isotopes of hydrogen are unique in that they are each commonly referred to by a unique name instead of the common chemical element name. Hydrogen-1 is almost always referred to as hydrogen, but the term protium is infrequently used also. Hydrogen-2 is commonly called deuterium and symbolized 21D ...
Name: (1 of 2) Math Set # 13 Protons,
... The number of protons is ALWAYS the same for an atom of a specific element. Germanium ALWAYS has 32 protons. If you add a proton it is no longer Germanium but becomes Arsenic. ...
... The number of protons is ALWAYS the same for an atom of a specific element. Germanium ALWAYS has 32 protons. If you add a proton it is no longer Germanium but becomes Arsenic. ...
Document
... Mass is not gained or lost in a chemical reaction. Proposed by Antoine Lavoisier in 1787. What would happen to the mass reading if the reaction was done without the balloon (an open system)? ...
... Mass is not gained or lost in a chemical reaction. Proposed by Antoine Lavoisier in 1787. What would happen to the mass reading if the reaction was done without the balloon (an open system)? ...
Ch 30 Nuclear Physics
... from radioactive decay. Therefore if any lead-204 is present we know that the other three lead isotopes are also present and we know their ratios. ...
... from radioactive decay. Therefore if any lead-204 is present we know that the other three lead isotopes are also present and we know their ratios. ...
What Are Atoms, and Why Do They Join Together?
... neutrons in the nucleus of an element may vary. Most oxygen atoms have seven neutrons, but some may have slightly more or less neutrons. You cannot tell what element an atom is just by the number of neutrons. The mass of an electron is much less than the mass of a proton or neutron, and it would tak ...
... neutrons in the nucleus of an element may vary. Most oxygen atoms have seven neutrons, but some may have slightly more or less neutrons. You cannot tell what element an atom is just by the number of neutrons. The mass of an electron is much less than the mass of a proton or neutron, and it would tak ...
Electrons
... 4. The oxidation number of hydrogen is____except when it is bonded to metals in binary compounds. In these cases, its oxidation number is____. 5. Group 1 metals are____, Group 2 metals are____and fluorine is always____. 6. The sum of the oxidation numbers of all the atoms in a molecule or ion is eq ...
... 4. The oxidation number of hydrogen is____except when it is bonded to metals in binary compounds. In these cases, its oxidation number is____. 5. Group 1 metals are____, Group 2 metals are____and fluorine is always____. 6. The sum of the oxidation numbers of all the atoms in a molecule or ion is eq ...
8.3 Metals - UNSW Chemistry
... – atomic spectra could not be explained by the Nuclear Atomic model. Relative Atomic Sizes Atomic radius is a measure of the distance between an atomic nucleus and the outermost electron (the valence electron). It is extremely difficult to measure this distance, and thus a variety of measures of ato ...
... – atomic spectra could not be explained by the Nuclear Atomic model. Relative Atomic Sizes Atomic radius is a measure of the distance between an atomic nucleus and the outermost electron (the valence electron). It is extremely difficult to measure this distance, and thus a variety of measures of ato ...
Chapter 18: The Representative Elements
... configuration is ns2np2 (n is the period number). The half filled orbital allows this group to straddle between metal and non metal. The heavier elements of the group are more likely to keep their s electrons and can have oxidation numbers of +2 or +4. ...
... configuration is ns2np2 (n is the period number). The half filled orbital allows this group to straddle between metal and non metal. The heavier elements of the group are more likely to keep their s electrons and can have oxidation numbers of +2 or +4. ...
19 Chapter
... Because the numbers of neutrons in the isotopes are different, the mass numbers are also different. • You use the name of the element followed by the mass number of the isotope to identify each isotope: boron10 and boron-11. ...
... Because the numbers of neutrons in the isotopes are different, the mass numbers are also different. • You use the name of the element followed by the mass number of the isotope to identify each isotope: boron10 and boron-11. ...
Chapter 18: The Representative Elements The Representative
... number). In its elemental state, all halogens atoms combine to form diatomic molecules (ex. F2,I2,…). With the exception of F, the halogens can also lose valence electrons and their oxidation states can range from -1 to +7. Chapter 18: The Representative Elements ...
... number). In its elemental state, all halogens atoms combine to form diatomic molecules (ex. F2,I2,…). With the exception of F, the halogens can also lose valence electrons and their oxidation states can range from -1 to +7. Chapter 18: The Representative Elements ...
Chapter 4 Atoms and Elements
... 1. Most of the atom’s mass and all of its positive charge are contained in a small core called the nucleus. 2. Most of the volume of the atom is empty space through which the tiny, negatively charged electrons are dispersed. 3. The number of negatively charged electrons outside the nucleus is equal ...
... 1. Most of the atom’s mass and all of its positive charge are contained in a small core called the nucleus. 2. Most of the volume of the atom is empty space through which the tiny, negatively charged electrons are dispersed. 3. The number of negatively charged electrons outside the nucleus is equal ...
Essential Question: What type of model did Thompson ,Rutherford
... Said that electrons are found in specific circular pathways (energy levels or orbits) around the nucleus Every possible orbit has a fixed amount of electrons Lowest energy is found in the energy level closest to the nucleus Electrons can jump from electrons level to electron level therefore electron ...
... Said that electrons are found in specific circular pathways (energy levels or orbits) around the nucleus Every possible orbit has a fixed amount of electrons Lowest energy is found in the energy level closest to the nucleus Electrons can jump from electrons level to electron level therefore electron ...
Chapter 2 Atoms and Elements
... The nucleus has essentially the entire mass of the atom the electrons weigh so little they give practically no mass to the atom The nucleus is positively charged the amount of positive charge balances the negative charge of the electrons The electrons are dispersed in the empty space of the atom ...
... The nucleus has essentially the entire mass of the atom the electrons weigh so little they give practically no mass to the atom The nucleus is positively charged the amount of positive charge balances the negative charge of the electrons The electrons are dispersed in the empty space of the atom ...
Chapter 2 Atoms and Elements
... The nucleus has essentially the entire mass of the atom the electrons weigh so little they give practically no mass to the atom The nucleus is positively charged the amount of positive charge balances the negative charge of the electrons The electrons are dispersed in the empty space of the atom ...
... The nucleus has essentially the entire mass of the atom the electrons weigh so little they give practically no mass to the atom The nucleus is positively charged the amount of positive charge balances the negative charge of the electrons The electrons are dispersed in the empty space of the atom ...
Electron - cloudfront.net
... element consists of atoms. Atoms are tiny particles which are indivisible by chemical means. ...
... element consists of atoms. Atoms are tiny particles which are indivisible by chemical means. ...
Masses of Atoms - Pelham City Schools
... Because the numbers of neutrons in the isotopes are different, the mass numbers are also different. • You use the name of the element followed by the mass number of the isotope to identify each isotope: boron10 and boron-11. ...
... Because the numbers of neutrons in the isotopes are different, the mass numbers are also different. • You use the name of the element followed by the mass number of the isotope to identify each isotope: boron10 and boron-11. ...
Chapter 17 notes
... Because the numbers of neutrons in the isotopes are different, the mass numbers are also different. • You use the name of the element followed by the mass number of the isotope to identify each isotope: boron10 and boron-11. ...
... Because the numbers of neutrons in the isotopes are different, the mass numbers are also different. • You use the name of the element followed by the mass number of the isotope to identify each isotope: boron10 and boron-11. ...
Chapter 4, 5, 6 - Campbell County Schools
... Target 2 - Identify the atomic number and the atomic mass of all elements and explain what they mean. A. All of the elements are listed on the ___________________________ of Elements. B. Elements are different kinds of atoms with a name, symbol, and unique properties. C. The Periodic Table lists the ...
... Target 2 - Identify the atomic number and the atomic mass of all elements and explain what they mean. A. All of the elements are listed on the ___________________________ of Elements. B. Elements are different kinds of atoms with a name, symbol, and unique properties. C. The Periodic Table lists the ...
Which of the following statements correctly describes the relative
... Which of the following statements accurately describes the locations of the three subatomic particles that make up an atom? ...
... Which of the following statements accurately describes the locations of the three subatomic particles that make up an atom? ...
Ch 04 AtomicStructure
... A. The actual mass of an electron is very large compared to the actual mass of a proton. B. The actual masses of atoms are very small and difficult to work with. C. The number of subatomic particles in atoms of different elements varies. D. The actual masses of protons, electrons, and neutrons are n ...
... A. The actual mass of an electron is very large compared to the actual mass of a proton. B. The actual masses of atoms are very small and difficult to work with. C. The number of subatomic particles in atoms of different elements varies. D. The actual masses of protons, electrons, and neutrons are n ...
Chapter 3 Notes
... Light is a small part of all the radiation (something that spreads from a source) called electromagnetic radiation. Electromagnetic radiation is energy in the form of waves (of electric and magnetic fields). Electromagnetic radiation includes radio waves, microwaves, infrared, visible light, X-rays ...
... Light is a small part of all the radiation (something that spreads from a source) called electromagnetic radiation. Electromagnetic radiation is energy in the form of waves (of electric and magnetic fields). Electromagnetic radiation includes radio waves, microwaves, infrared, visible light, X-rays ...