2 C Atomic Number Mass Number Atomic Mass and Isotopes
... Atoms have no overall electrical charge so, an atom must have as many electrons as there are ...
... Atoms have no overall electrical charge so, an atom must have as many electrons as there are ...
Tendencies of ionic/atomic radii in the periodic table
... Tendencies of ionic and atomic radii in the periodic table Tendencies: 1. The atomic radii increase down a group (e.g. first group 157 – 272 pm) and within the s and p blocks, decrease from left to right across a period (e.g. second period 157 – 64 pm). 2. The atomic radii for elements following the ...
... Tendencies of ionic and atomic radii in the periodic table Tendencies: 1. The atomic radii increase down a group (e.g. first group 157 – 272 pm) and within the s and p blocks, decrease from left to right across a period (e.g. second period 157 – 64 pm). 2. The atomic radii for elements following the ...
Atoms, Elements, and the Periodic Table (Chapter 2)
... Z = atomic number of an element = # protons in nucleus e.g., carbon is atomic number 6 -- all carbon atoms have 6 protons A = mass number (often omitted) = # protons + # neutrons Y = charge (on an ion) = # protons - # electrons isotopes - atoms of the same element with different mass numbers e.g., ...
... Z = atomic number of an element = # protons in nucleus e.g., carbon is atomic number 6 -- all carbon atoms have 6 protons A = mass number (often omitted) = # protons + # neutrons Y = charge (on an ion) = # protons - # electrons isotopes - atoms of the same element with different mass numbers e.g., ...
Chapt2
... Z = atomic number of an element = # protons in nucleus e.g., carbon is atomic number 6 -- all carbon atoms have 6 protons A = mass number (often omitted) = # protons + # neutrons Y = charge (on an ion) = # protons - # electrons isotopes - atoms of the same element with different mass numbers e.g., ...
... Z = atomic number of an element = # protons in nucleus e.g., carbon is atomic number 6 -- all carbon atoms have 6 protons A = mass number (often omitted) = # protons + # neutrons Y = charge (on an ion) = # protons - # electrons isotopes - atoms of the same element with different mass numbers e.g., ...
Adv review key
... _Group/Family 15_7. Name of the chemical family containing Nitrogen _P,As,Sb,Bi__8. Name of another element in the same family with Nitrogen _Li,Be,B,C,O,F,Ne____9. Name of another element in the same period with Nitrogen Ionic bonding A) Electrons are transferred between atoms B) Valence electrons- ...
... _Group/Family 15_7. Name of the chemical family containing Nitrogen _P,As,Sb,Bi__8. Name of another element in the same family with Nitrogen _Li,Be,B,C,O,F,Ne____9. Name of another element in the same period with Nitrogen Ionic bonding A) Electrons are transferred between atoms B) Valence electrons- ...
APS 1st semester exam review 2016
... _Group/Family 15_7. Name of the chemical family containing Nitrogen _P,As,Sb,Bi__8. Name of another element in the same family with Nitrogen _Li,Be,B,C,O,F,Ne____9. Name of another element in the same period with Nitrogen Ionic bonding A) Electrons are transferred between atoms B) Valence electrons- ...
... _Group/Family 15_7. Name of the chemical family containing Nitrogen _P,As,Sb,Bi__8. Name of another element in the same family with Nitrogen _Li,Be,B,C,O,F,Ne____9. Name of another element in the same period with Nitrogen Ionic bonding A) Electrons are transferred between atoms B) Valence electrons- ...
chapter 4 - Elkhorn Valley Schools
... He thought atoms had different shapes and sizes He thought they were indivisible and indestructible “atomists” – people who followed his beliefs ...
... He thought atoms had different shapes and sizes He thought they were indivisible and indestructible “atomists” – people who followed his beliefs ...
Miss Pang`s 2012 Review
... Which of the following statements explains this similarity in chemical properties? A) B) C) D) ...
... Which of the following statements explains this similarity in chemical properties? A) B) C) D) ...
Fundamentals Fall Final Review
... 20. Isotopes of a given element have the same number of __________, but different number of ____________. 21. Know how to calculate the number of protons, neutrons and electrons in an atom when given its isotope mass and atomic number. As an example: Iron (Fe) has an atomic number of 26. An isotope ...
... 20. Isotopes of a given element have the same number of __________, but different number of ____________. 21. Know how to calculate the number of protons, neutrons and electrons in an atom when given its isotope mass and atomic number. As an example: Iron (Fe) has an atomic number of 26. An isotope ...
Honors Chemistry
... mass / kilogram time / second volume density chemical property physical property malleability ductility conductivity reactivity phase state solid liquid gas melting / freezing evaporating / condensing mixture solution substance homogeneous heterogeneous element compound atom molecule formula unit di ...
... mass / kilogram time / second volume density chemical property physical property malleability ductility conductivity reactivity phase state solid liquid gas melting / freezing evaporating / condensing mixture solution substance homogeneous heterogeneous element compound atom molecule formula unit di ...
Chemistry--Chapter 5: Atomic Structure and the Periodic Table
... The number of ________________(13) in the nucleus of an atom is the atomic ________________(14) of that element. Because atoms are electrically neutral, the number of protons and ________________(15) in an atom are equal. The sum of the ________________(16) and neutrons is the mass number. Atoms of ...
... The number of ________________(13) in the nucleus of an atom is the atomic ________________(14) of that element. Because atoms are electrically neutral, the number of protons and ________________(15) in an atom are equal. The sum of the ________________(16) and neutrons is the mass number. Atoms of ...
chem 4 outline for exam 1
... Identify the three principal components (subatomic particles) of the atom, stating their electrical charges and relative masses. Describe the general arrangement of subatomic particles in the atom. Given the atomic number and mass number of an atom, state the number of protons, electrons, and neutro ...
... Identify the three principal components (subatomic particles) of the atom, stating their electrical charges and relative masses. Describe the general arrangement of subatomic particles in the atom. Given the atomic number and mass number of an atom, state the number of protons, electrons, and neutro ...
AM-1 Power point - Moline High School
... Ion-Charged atom due to the loss or gain of electrons If an atom gains electrons, becomes negatively charged (anion) If an atom loses electrons, becomes positively charged ...
... Ion-Charged atom due to the loss or gain of electrons If an atom gains electrons, becomes negatively charged (anion) If an atom loses electrons, becomes positively charged ...
... Everything around us is made up of atoms. Atoms are one of the smallest units of matter. An atom is too small to see directly through a microscope. The smallest speck that can be seen under an ordinary microscope contains more than ten billion atoms. An atom is more that a million times smaller than ...
Chapter 4
... The periodic table helps determine electron arrangement Horizontal rows (L - R) in the periodic table are called periods ...
... The periodic table helps determine electron arrangement Horizontal rows (L - R) in the periodic table are called periods ...
Units 3 and 4 Revision
... Q4. Explain why the metal elements in group 1 are (a) called the alkali metals. (b) stored under oil. Q5. What happens to the melting point of the elements in group 7 (the halogens) as you go the group? Answers:- Q3. Lithium. Q4. (a) The elements in group 1 react with water to form an ...
... Q4. Explain why the metal elements in group 1 are (a) called the alkali metals. (b) stored under oil. Q5. What happens to the melting point of the elements in group 7 (the halogens) as you go the group? Answers:- Q3. Lithium. Q4. (a) The elements in group 1 react with water to form an ...
Chapter 4 Atomic Structure
... identical. Atoms of any one element are different from those of any other element. ...
... identical. Atoms of any one element are different from those of any other element. ...
IPS Unit 8 – Periodic Table Review Worksheet
... 7. An element is matter that is composed of one type of (atom/quark). 8. The unit of measurement used for atomic particles is the (atom size/atomic mass unit). 9. Atoms of the same element that have different numbers of neutrons are called (isotopes/electron clouds). 10. In the periodic table, eleme ...
... 7. An element is matter that is composed of one type of (atom/quark). 8. The unit of measurement used for atomic particles is the (atom size/atomic mass unit). 9. Atoms of the same element that have different numbers of neutrons are called (isotopes/electron clouds). 10. In the periodic table, eleme ...
atomic number
... tendency of an atom to attract electrons to itself, which is affected by both its atomic number and the distance that its valence electrons reside from the charged nucleus. ...
... tendency of an atom to attract electrons to itself, which is affected by both its atomic number and the distance that its valence electrons reside from the charged nucleus. ...
Document
... Chapter 4 Practice Test – Answer Key Use the table below to answer the following three questions: ...
... Chapter 4 Practice Test – Answer Key Use the table below to answer the following three questions: ...
Chemical Element
... Before chemistry became a science, alchemists had designed arcane symbols for both metals and common compounds. These were however used as abbreviations in diagrams or procedures; there was no concept of atoms combining to form molecules. With his advances in the atomic theory of matter, John Dalton ...
... Before chemistry became a science, alchemists had designed arcane symbols for both metals and common compounds. These were however used as abbreviations in diagrams or procedures; there was no concept of atoms combining to form molecules. With his advances in the atomic theory of matter, John Dalton ...
PowerPoint - Models of the Atom
... • Rutherford shot alpha () particles at gold foil. Most particles passed through. So, atoms are mostly empty. Some positive -particles deflected or bounced back! Thus, a “nucleus” is positive & holds most of an atom’s mass. ...
... • Rutherford shot alpha () particles at gold foil. Most particles passed through. So, atoms are mostly empty. Some positive -particles deflected or bounced back! Thus, a “nucleus” is positive & holds most of an atom’s mass. ...
Unit 2 Review for Test
... 45. Name the primary use of the type of macromolecule which is a source of energy. 46. Name the macromolecule which is the primary component in cellular membranes. 47. Name the macromolecule whose function includes structural contributions, communication, and defense against disease. 48. Proteins ar ...
... 45. Name the primary use of the type of macromolecule which is a source of energy. 46. Name the macromolecule which is the primary component in cellular membranes. 47. Name the macromolecule whose function includes structural contributions, communication, and defense against disease. 48. Proteins ar ...