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Practice Multiple Choice Questions for the Chemistry Final Exam
... Who was the schoolmaster who studied chemistry and proposed an atomic theory? a) John Dalton b) Jons Berzehus c) Robert Brown d) Dmitri Mendeleev ...
... Who was the schoolmaster who studied chemistry and proposed an atomic theory? a) John Dalton b) Jons Berzehus c) Robert Brown d) Dmitri Mendeleev ...
atomic number
... If there are vacancies, the atom is reactive/unstable If there are no vacancies, the atom is nonreactive/stable If the vacancies are filled due to bonding, the molecule is stable ...
... If there are vacancies, the atom is reactive/unstable If there are no vacancies, the atom is nonreactive/stable If the vacancies are filled due to bonding, the molecule is stable ...
Early atomic theory • The Greek philosophers (400 BC) –Democritus
... • A third particle would go undiscovered for some time, although lth h it wass predicted p di t d to t exist xist by Lord Rutherford in 1920. ...
... • A third particle would go undiscovered for some time, although lth h it wass predicted p di t d to t exist xist by Lord Rutherford in 1920. ...
I - Chemistry-at-PA
... e. alike in number of electrons. c. different in number of electrons. 9) According to Democritus’s ideas about “atomos” which one of the following is TRUE? a. Atomos are divisible. b. Atomos are hard dense spheres c. Atomos have varying density – they are heterogeneous. d. Changes in matter are due ...
... e. alike in number of electrons. c. different in number of electrons. 9) According to Democritus’s ideas about “atomos” which one of the following is TRUE? a. Atomos are divisible. b. Atomos are hard dense spheres c. Atomos have varying density – they are heterogeneous. d. Changes in matter are due ...
Review
... 1. All hydrogen atoms contain one _____________________. However, like many naturally occurring elements, hydrogen can contain different numbers of _______________________. _________ types of hydrogen atoms are known. a. The most common type is sometimes called _______________________. Its nucleus h ...
... 1. All hydrogen atoms contain one _____________________. However, like many naturally occurring elements, hydrogen can contain different numbers of _______________________. _________ types of hydrogen atoms are known. a. The most common type is sometimes called _______________________. Its nucleus h ...
Name: Per: Date: Unit 1. Materials: Formulating Matter B. Periodic
... B. Periodic Trends. How can the periodic table be used to help explain and predict the properties of chemical elements? More than 100 chemical elements have been discovered and explored. Of those, a small number are considered highly prized and used for coins, jewelry, and art. Why are some more val ...
... B. Periodic Trends. How can the periodic table be used to help explain and predict the properties of chemical elements? More than 100 chemical elements have been discovered and explored. Of those, a small number are considered highly prized and used for coins, jewelry, and art. Why are some more val ...
chapter5
... People can go up a ladder by going from rung to rung the way electrons in an atom can go from energy level to energy level. A person can never stand between the rungs of a ladder and electrons must always be at a specific energy level as well (and not between them). In order for a person to go from ...
... People can go up a ladder by going from rung to rung the way electrons in an atom can go from energy level to energy level. A person can never stand between the rungs of a ladder and electrons must always be at a specific energy level as well (and not between them). In order for a person to go from ...
All matter is made of atoms.
... The negative electrons remain associated with the nucleus because they are attracted to the positively charged protons. Also, because electrical charges that are alike (such as two negative charges) repel each other, electrons remain spread out in the electron cloud. Neutral atoms have no overall el ...
... The negative electrons remain associated with the nucleus because they are attracted to the positively charged protons. Also, because electrical charges that are alike (such as two negative charges) repel each other, electrons remain spread out in the electron cloud. Neutral atoms have no overall el ...
chapter 4
... You CAN do this. Work out the example if you are stuck. It’s like this: Carbon is made up of 98.89% Carbon-12 & 1.11% Carbon-13 Its atomic mass would be (12amu•0.9889)+(13.03amu•0.0111) = 12.011 amu ...
... You CAN do this. Work out the example if you are stuck. It’s like this: Carbon is made up of 98.89% Carbon-12 & 1.11% Carbon-13 Its atomic mass would be (12amu•0.9889)+(13.03amu•0.0111) = 12.011 amu ...
Inside the Atom
... repel each other Rather strong nuclear forces hold the protons together only when they are closely packed as they are in the nucleus of the atom ...
... repel each other Rather strong nuclear forces hold the protons together only when they are closely packed as they are in the nucleus of the atom ...
Atoms- Building Blocks TG quark.qxd
... holds the atom together. There are different types of atoms with different numbers of protons, neutrons, and electrons. They are called elements. An electrically neutral atom has the same number of protons and electrons. Usually an atom has the same number of protons and neutrons but when it has mor ...
... holds the atom together. There are different types of atoms with different numbers of protons, neutrons, and electrons. They are called elements. An electrically neutral atom has the same number of protons and electrons. Usually an atom has the same number of protons and neutrons but when it has mor ...
Concepts to know for the Unit 3 test
... Concepts to know for the Unit 3 test: 1. Summarize the major experimental evidence that led to the development of various atomic models, both historical and current. 2. Evaluate the limitations of using models to describe atoms. a. Aristotle: a. WRONG, four elements – earth, air, water, fire b. Demo ...
... Concepts to know for the Unit 3 test: 1. Summarize the major experimental evidence that led to the development of various atomic models, both historical and current. 2. Evaluate the limitations of using models to describe atoms. a. Aristotle: a. WRONG, four elements – earth, air, water, fire b. Demo ...
Atomic structure and the periodic tabl
... and with most of the mass in the nucleus. A suggested teaching sequence for the beginning of the GCSE course would be to first discuss how the modern model of the atom developed over time as scientists rejected earlier models and proposed new ones to fit the currently available evidence. Stages in t ...
... and with most of the mass in the nucleus. A suggested teaching sequence for the beginning of the GCSE course would be to first discuss how the modern model of the atom developed over time as scientists rejected earlier models and proposed new ones to fit the currently available evidence. Stages in t ...
Click here to Ch 3.2_ Atoms_Structure
... • Because atomic radii are so small, they are expressed using a unit that is more convenient for the sizes of atoms. • This unit is the picometer, pm. ...
... • Because atomic radii are so small, they are expressed using a unit that is more convenient for the sizes of atoms. • This unit is the picometer, pm. ...
10/2/2013 1 10 Modern Atomic Theory and the Periodic Table
... rules for filling electrons can be developed. Guidelines for filling electrons: 1. Only up to two electrons can occupy an orbital. 2. Electron will occupy lower energy orbitals first. Orbital energies: s < p < d < f for a given n value. 3. Each orbital in a sublevel must contain an electron before a ...
... rules for filling electrons can be developed. Guidelines for filling electrons: 1. Only up to two electrons can occupy an orbital. 2. Electron will occupy lower energy orbitals first. Orbital energies: s < p < d < f for a given n value. 3. Each orbital in a sublevel must contain an electron before a ...
AP Chemistry Chapter 3 – The Structure of the Atom was the early
... To know the maximum amount of electrons that could be in any principal quantum level (and the number of elements that could be represented) use the formula 2n2 if n=1, then _____________________ electrons will fit if n=4, then _____________________ electrons will fit ...
... To know the maximum amount of electrons that could be in any principal quantum level (and the number of elements that could be represented) use the formula 2n2 if n=1, then _____________________ electrons will fit if n=4, then _____________________ electrons will fit ...
Test Review Chapter 1
... 1. The law of conservation of mass follows from the concept that a. atoms are indivisible. b. atoms of different elements have different properties. c. matter is composed of atoms. d. atoms can be destroyed in chemical reactions. 2. According to the law of definite proportions, any two samples of KC ...
... 1. The law of conservation of mass follows from the concept that a. atoms are indivisible. b. atoms of different elements have different properties. c. matter is composed of atoms. d. atoms can be destroyed in chemical reactions. 2. According to the law of definite proportions, any two samples of KC ...
File
... C) atomic numbers of the naturally occurring isotopes of that element D) atomic masses of the naturally occurring isotopes of that element 25. The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (shown as percents) produces this average mass? A) 50% 12C and 50% 13C B) 50% 35Cl a ...
... C) atomic numbers of the naturally occurring isotopes of that element D) atomic masses of the naturally occurring isotopes of that element 25. The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (shown as percents) produces this average mass? A) 50% 12C and 50% 13C B) 50% 35Cl a ...
Early View of the Elements Democritus Metallurgy
... 1) matter could be broken down into indivisible bits called atomos: modern-day “atoms” 2) different atoms made different materials 3) combining different atoms made new materials Science 9 – Unit B (Chemistry) – Section 2.1 ...
... 1) matter could be broken down into indivisible bits called atomos: modern-day “atoms” 2) different atoms made different materials 3) combining different atoms made new materials Science 9 – Unit B (Chemistry) – Section 2.1 ...
Atoms and - 4LTR Press
... hy does an element or compound have the properties it has? Why does one element or compound undergo a change that another element or compound will not undergo? Inanimate matter behaves the way it does because of the nature of its parts. The use of atoms to represent these parts dates back to about 4 ...
... hy does an element or compound have the properties it has? Why does one element or compound undergo a change that another element or compound will not undergo? Inanimate matter behaves the way it does because of the nature of its parts. The use of atoms to represent these parts dates back to about 4 ...
Periodic Table: Why the repetition
... •Particles come in discrete chunks that can be counted. That is, they are quantized. They carry energy as kinetic energy which is infinitely adjustable. •Waves do not come in discrete chunk but instead are continuous and thus are not countable like particles. They are not quantized. They have wavele ...
... •Particles come in discrete chunks that can be counted. That is, they are quantized. They carry energy as kinetic energy which is infinitely adjustable. •Waves do not come in discrete chunk but instead are continuous and thus are not countable like particles. They are not quantized. They have wavele ...
Periodic table
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.