Chemistry Chapter 3 Test

Front 1

describe scientists' discoveries toward and the progression of atomic theory

Back 1

-democritus suggested existence of atoms
-no evidence existed
-dalton proposed atomic theory with scientific basis

Front 2

list daltons postulates of the atomic theory of matter and compare to mdoern atomic theory

Back 2

A. Elements are made of tiny particles called atoms
B. Atoms cannot be divided
C. All atoms of an element are exactly alike
D. Atoms of different elements combine to form compounds
EVIDENCE TO FALSITY OF B AND C: law of conservation of mass

Front 3

explain the model of the atom as proposed by rutherford

Back 3

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Front 4

*know symbols of elements*

Back 4

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Front 5

*know how to apply the law of conservation of mass to various situations*

Back 5

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Front 6

*determine the number of protons, neutrons and electrons using the complete symbol, mass number, atmic number, and net charge of an atom or ion*

Back 6

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Front 7

*write a complete atomic symbol from given information

Back 7

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Front 8

*name locate and identify properties of various groups (families) on the periodic table

Back 8

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Front 9

*identify groups on the periodic table using the two common numbering systems*

Back 9

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Front 10

*using periodic table, identify elements as metals, nonmetals, or mellatoids, and describe properties*

Back 10

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Front 11

describe the formation of cations and anions, locate the pattern of ionic charge on the periodic table

Back 11

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Front 12

describe the history of the periodic table, and explain how the current periodic table is arranged

Back 12

-used to be a mess; no organization of elements
-chemistry did not make sense
-difficult to find information
-elements are put in rows by increasing atomic number
-horizontal rows are called periods and are labeled from 1 to 7
-the vertical columns are called groups are labeled from 1 to 18

Front 13

actinides

Back 13

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Front 14

alkali metals

Back 14

-1st column on the periodic table (group 1); not including hydrogen
-very reactive metals, always combined with something else in nature
-soft enough to cut with a butter knife

Front 15

alkaline earth metals

Back 15

-second column on the periodic table (group 2)
-reactive metals that are always combined with nonmetals in nature
-several of these elements are important mineral nutrients

Front 16

anoin

Back 16

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Front 17

atom

Back 17

-an ion is an atom that has gained or lost electrons
-the charge will show how many protons or electrons the ion has
-the number of protons in an element never changes
-it is the electrons that increase or decrease

Front 18

atomic mass

Back 18

-also called atomic weight
-larger value in each box of the table
-average of mass numbers for that element
-amount of each isotope that exists is calculated in this average

Front 19

atomic mass unit

Back 19

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Front 20

atomic number

Back 20

-number of protons of that element (top left/right corner)
-listed for each box on the periodic table
-remains the same for each element

Front 21

atomic symbol

Back 21

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Front 22

cathode ray tube

Back 22

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Front 23

cation

Back 23

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Front 24

chemical formula

Back 24

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Front 25

complete atomic symbol

Back 25

-complete symbols communicate much information about an atom or ion
-upper left or right corner; mass number tells protons and neutrons together

Front 26

conservation of mass

Back 26

-in any process, the mass of all reactants must equal the mass of all products

Front 27

electron

Back 27

-negative charge
-very small mass 0.0006 amu
-same number of electrons as protons in a neutral atom

Front 28

group (family)

Back 28

-have similar chemical and physical properties
-have the same number of valence electrons
-will form the same kind of ions
-families can be one column or several

Front 29

halogens

Back 29

-elements in group 17
-very reactive, volatile, diatomic nonmetals
-always found combined with other elements in nature
-used as disinfectants and to strengthen teeth

Front 30

ion

Back 30

-an atom that has gained or lost electrons
-number of protons never changes
-the electrons decrease or increase

Front 31

isotope

Back 31

-atoms of the same element with different number of neutrons
-same element if they have the same number of protons
-they have the same number of protons
-will have different mass numbers

Front 32

lanthanides

Back 32

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Front 33

law of definite proportions

Back 33

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Front 34

mass number

Back 34

-the total number of protons and neutrons in the nucleus of the atom = #protons + #neutrons = mass number
-not on the periodic table - you must find it yourself
-formula can also be used to calculate the number of neutrons in the atom

Front 35

metal

Back 35

-conductors of heat and electricity
-malleable solids
-ductile
-lustrous (shiny)
-high melting and boiling points
-located to left of stair-step line

Front 36

metalloid (semimetal)

Back 36

-elements that lie in contact with stair-step line (except al
-show a mixture of metallic and non metallic properties

Front 37

molecule

Back 37

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Front 38

net charge

Back 38

-helps determine protons and electrons

Front 39

neutron

Back 39

-no charge
-mass of 1 amu
-all neutrons are identical to each other

Front 40

noble gases

Back 40

-elements in group 18
-very unreactive, monatomic gases
-used in lighted "neon" signs
-used in blimps to fix the hindenberg problem
-have a full valence shell

Front 41

non metal

Back 41

-insulators
-brittle solids and gases
-dull
-low melting and boiling points
-located to right of stair-step

Front 42

nucleus

Back 42

-very small and dense
-contains protons and neutrons
-contains most of the atom's amss
-overall positive charge

Front 43

period

Back 43

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Front 44

proton

Back 44

-positively charged
-mass of 1 amu
-the number of protons determines the identity of the element
-all protons are identical to each other

Front 45

transition metals

Back 45

-elements in groups 3-12
-less reactive harder metals
-includes metals used in jewelry and construction
-metals used "as metal"

Front 46

boron family

Back 46

-elements in group 13
-aluminum metal was once rare and expensive not a "disposable metal"

Front 47

carbon family

Back 47

-elements in group 14
-contains elements important to life and computers
-carbon is the basis for an entire branch of chemistry
-silicon and germanium are important semiconductors

Front 48

nitrongen family

Back 48

-elements in group 15
-nitrogen makes up 3/4 of the atmosphere
-nitrogen and phosporus are both important in living things
-most of the world's nitrogen is not available to living things
-the red stuff on teh tip of matches is phosphorus

Front 49

oxygen family or chalcogens

Back 49

-elements in group 16
-oxygen is necessary for respiration
-many things that stink, contain sulfur

Front 50

electron cloud

Back 50

-surrounds the nucelus
-has energy levels
-lower energy levels are closer to the nucleus
-number shells from inside out - lowest number is closest to the nucleus/theclosest inside
-negatively charged
-occupies most of the atom's space
-most of its space is empty

Front 51

electrons in the electron cloud

Back 51

-move randomly within their energy level
-act like fan blades to occupy the empty space
-each energy level hold a maximum number of electrons

Front 52

electrons ont eh move

Back 52

-atoms will gain or lose electrons to get to a full outer energy level
-negative ions form by gaining electrons
-positive ions form by losing electrons
-atoms will gain, lose, or share electrons to get a full outer energy level (typically 8 electrons - full octet)

Front 53

democritus

Back 53

-first to propose existence of atoms; philosopher

Front 54

boyle

Back 54

-defined element through experiment; if he could break down he knew the substance wasn't an element

Front 55

lavoisier

Back 55

-proposed law of conservation of mass; everything must weight the same before and after

Front 56

dalton

Back 56

-came up with the atoic theory and listed 4 things he thought described atoms

Front 57

thomsen

Back 57

-discovered electron and came up with the plum pudding model of the atom

Front 58

rutherford

Back 58

-did the gold foil experiment - 99% went through (atom is mostly empty space) but some were deflected by the nucleus; figured it had to be very small and dense an positively charged; came up with a model that we know today is not true

Front 59

mendeleev

Back 59

-sorted out the periodic table
-left spaces for future elements

Front 60

moseley

Back 60

-proved atomic weight was insignificant - resorted periodic table by atomic # - discovered the proton (atomic weight wasn't as good as atomic #)