The Atom
... mass #’s (or simply, • Because of this, they have different _________ masses different ___________.) • Isotopes are the same element, but the atoms weigh a different neutrons amount because of the # of ______________. Examples---> (1) Carbon-12 & Carbon-13 (2) Chlorine-35 & Chlorine-37 (The # shown ...
... mass #’s (or simply, • Because of this, they have different _________ masses different ___________.) • Isotopes are the same element, but the atoms weigh a different neutrons amount because of the # of ______________. Examples---> (1) Carbon-12 & Carbon-13 (2) Chlorine-35 & Chlorine-37 (The # shown ...
Unit 3 Notes, Practice, and Review
... 19. The atomic number is unique for every element. It also tells the number of protons in that element. Every element on the periodic table has a unique number of protons. It’s like an element’s Social Security Number. 20. Atomic number is the number of protons and electrons in an atom. To get the n ...
... 19. The atomic number is unique for every element. It also tells the number of protons in that element. Every element on the periodic table has a unique number of protons. It’s like an element’s Social Security Number. 20. Atomic number is the number of protons and electrons in an atom. To get the n ...
Unit 4 Day 1 Intro to Atom
... the nucleus (protons or neutrons) are very rare. They only take place in nuclear processes such as: radioactive decay nuclear bombs nuclear reactors. ...
... the nucleus (protons or neutrons) are very rare. They only take place in nuclear processes such as: radioactive decay nuclear bombs nuclear reactors. ...
the electron configuration notes
... nucleus – leaving lots of empty space Later experiments showed a nucleus of + charged protons and neutrally charged neutrons, surrounded by – charged ...
... nucleus – leaving lots of empty space Later experiments showed a nucleus of + charged protons and neutrally charged neutrons, surrounded by – charged ...
Electrons #2
... nucleus – leaving lots of empty space Later experiments showed a nucleus of + charged protons and neutrally charged neutrons, surrounded by – charged ...
... nucleus – leaving lots of empty space Later experiments showed a nucleus of + charged protons and neutrally charged neutrons, surrounded by – charged ...
2013 The Periodic Table
... nonmetals the greater the tendency to gain/share electrons, the more reactive the nonmetal is. ...
... nonmetals the greater the tendency to gain/share electrons, the more reactive the nonmetal is. ...
Ch 4 Powerpoint
... Elements are able to be subdivided into smaller and smaller particles – these are the atoms, and they still have properties of that element If you could line up 100,000,000 copper atoms in a single file, they would be approximately 1 cm long Despite their small size, individual atoms are observa ...
... Elements are able to be subdivided into smaller and smaller particles – these are the atoms, and they still have properties of that element If you could line up 100,000,000 copper atoms in a single file, they would be approximately 1 cm long Despite their small size, individual atoms are observa ...
File
... This means that the number of neutrons = Mass number – Atomic number Example The atomic number of fluorine is 9 and its mass number is 19. How many (i) protons, (ii) electrons and (iii) neutrons does a neutral fluorine atom have? (i) 9 protons, (ii) 9 electrons (same number as the number of protons) ...
... This means that the number of neutrons = Mass number – Atomic number Example The atomic number of fluorine is 9 and its mass number is 19. How many (i) protons, (ii) electrons and (iii) neutrons does a neutral fluorine atom have? (i) 9 protons, (ii) 9 electrons (same number as the number of protons) ...
Chapter 4
... In 1919, Rutherford fine-tuned his concept of the nucleus, stating that it contained positively charged subatomic particles equal to but opposite that of an electron (+1 charge)—proton. In 1932, Rutherford & his co-worker, James Chadwick, concluded that the nucleus contained yet another subatomic ...
... In 1919, Rutherford fine-tuned his concept of the nucleus, stating that it contained positively charged subatomic particles equal to but opposite that of an electron (+1 charge)—proton. In 1932, Rutherford & his co-worker, James Chadwick, concluded that the nucleus contained yet another subatomic ...
Masterton and Hurley - Chapter 6
... • It is impossible to specify the exact position of an electron at a given instant • We can only specify the probability of finding an electron in a particular region of space ...
... • It is impossible to specify the exact position of an electron at a given instant • We can only specify the probability of finding an electron in a particular region of space ...
Periodic Table - personals.okan.edu.tr
... • The more easily an atom loses its electrons, the more it tends to have a metallic character. • Ionization Energy (I) is the quantity of energy a gaseous atom must absorb so that an electron is stripped from the atom. The electron is the one most loosely held. • First ionization energy (I1), is the ...
... • The more easily an atom loses its electrons, the more it tends to have a metallic character. • Ionization Energy (I) is the quantity of energy a gaseous atom must absorb so that an electron is stripped from the atom. The electron is the one most loosely held. • First ionization energy (I1), is the ...
The Structure of the Atom- Chapter 4, 3
... Nuclear chemistry is the study of the changes of the NUCLEUS of an atom. Nuclear Reactions involve changes within the nucleus where as chemical reactions involve the loss, gain or sharing of electrons. ...
... Nuclear chemistry is the study of the changes of the NUCLEUS of an atom. Nuclear Reactions involve changes within the nucleus where as chemical reactions involve the loss, gain or sharing of electrons. ...
Sample Questions Sample Questions Standard Atomic Notation
... 17 number. The number of protons is 17, the number of electrons is 17 and the number of neutrons is 18. • 23Na 23 is the atomic mass, 11 is the atomic 11 number. The number of protons is 11, the ...
... 17 number. The number of protons is 17, the number of electrons is 17 and the number of neutrons is 18. • 23Na 23 is the atomic mass, 11 is the atomic 11 number. The number of protons is 11, the ...
CH 6: The Periodic Table
... periodic table because as you travel up a group, there are fewer energy levels on the atom. • Atomic radius decreases as you travel left to right across the periodic table because the number of protons in the nucleus increases. • As the number of protons increases, the nucleus pulls the electrons cl ...
... periodic table because as you travel up a group, there are fewer energy levels on the atom. • Atomic radius decreases as you travel left to right across the periodic table because the number of protons in the nucleus increases. • As the number of protons increases, the nucleus pulls the electrons cl ...
Atoms, Molecules, and Ions Chemistry Timeline #1
... Ernest Rutherford: Existence of the nucleus, and its relative size Meitner & Fermi: Sustained nuclear fission Ernest Lawrence: The cyclotron and trans-uranium elements ...
... Ernest Rutherford: Existence of the nucleus, and its relative size Meitner & Fermi: Sustained nuclear fission Ernest Lawrence: The cyclotron and trans-uranium elements ...
Document
... Lewis Dot Diagram shows only the element symbol and the VALENCE ELECTRONS. Bohr Model: “energy shells” replaced by Quantum mechanical model Explain how Bohr’s model of the atom incorporated Plank’s idea of quantization. The difference between a line spectrum and a continuous spectrum was the evidenc ...
... Lewis Dot Diagram shows only the element symbol and the VALENCE ELECTRONS. Bohr Model: “energy shells” replaced by Quantum mechanical model Explain how Bohr’s model of the atom incorporated Plank’s idea of quantization. The difference between a line spectrum and a continuous spectrum was the evidenc ...
1.What is the overall charge of an ion that has 12 protons
... spectrum of a mixture formed from at least two of these elements: ...
... spectrum of a mixture formed from at least two of these elements: ...
Part B: Periodic Trends
... 12. ATOMIC RADIUS of P vs. IONIC RADIUS of P 13. ATOMIC RADIUS of O vs. IONIC RADIUS of O ...
... 12. ATOMIC RADIUS of P vs. IONIC RADIUS of P 13. ATOMIC RADIUS of O vs. IONIC RADIUS of O ...
Atomic Theory Review
... Ionic compound charges 1. Which is a positive ion: A cation or an anion? 2. What is the charge of zinc in Zn3(PO4)2? 3. What is the charge on the iron atom in FePO4? 4. What is the name of FePO4? 5. What is the name of FeP? 6. Which of the following is incorrect? a) Sulfate is SO32- b) nitrate is a ...
... Ionic compound charges 1. Which is a positive ion: A cation or an anion? 2. What is the charge of zinc in Zn3(PO4)2? 3. What is the charge on the iron atom in FePO4? 4. What is the name of FePO4? 5. What is the name of FeP? 6. Which of the following is incorrect? a) Sulfate is SO32- b) nitrate is a ...
File - Johnson
... • Each element is composed of extremely small particles called atoms • All atoms of a given element are identical, but they differ from those of any other element • Atoms are neither created nor destroyed in any chemical rxn • A given compound always has the same relative numbers and kinds of atoms ...
... • Each element is composed of extremely small particles called atoms • All atoms of a given element are identical, but they differ from those of any other element • Atoms are neither created nor destroyed in any chemical rxn • A given compound always has the same relative numbers and kinds of atoms ...
chemistry basics - Menifee County Schools
... • By the 1700’s nearly all chemists had accepted the modern definition of an element as a particle that is indivisible • It was also understood at that time that elements combine to form compounds that are different in their properties than the elements that composed them – However, these understan ...
... • By the 1700’s nearly all chemists had accepted the modern definition of an element as a particle that is indivisible • It was also understood at that time that elements combine to form compounds that are different in their properties than the elements that composed them – However, these understan ...
Rule of Solid Solubility
... • Positive deviation of the enthalpy of mixing and consequently limited solid solubility may be predicted from known atomic properties. ...
... • Positive deviation of the enthalpy of mixing and consequently limited solid solubility may be predicted from known atomic properties. ...
