Chapter 02: Atoms and Elements Flashcards

1
Q

Law of conservation of mass

A

Matter is neither created nor destroyed in a chemical reaction

Mass of reactants = mass of products

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2
Q

Law of definite proportions

A

All samples of a given compound have the same proportions of their constituent elements

Water is always H20

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3
Q

Law of multiple proportions

A

Atoms of two or more elements may combine in different ratios, producing various compounds

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4
Q

Subatomic particles

A

Election (e-) - negative charge, mass is minute

Proton (p) - positive charge, mass = 1840x an electron’s

Neutron (n) - neutral particle, GREATEST MASS

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5
Q

Cathode rays

A

Beam of particles, negatively charged

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6
Q

Cathode

A

Negatively charged electrode

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7
Q

Anode

A

Positively charged electrode

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8
Q

Radioactivity

A

Spontaneous emission of particles and/or radiation

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9
Q

Radioactive element

A

Spontaneously emits radiation

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10
Q

Alpha particles

A

Positively charged particles

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11
Q

Beta particles

A

Negatively charged particles

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12
Q

Gamma rays

A

Neutral charge, high-energy radiation

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13
Q

Nuclear theory

A

Nucleus = most of atom’s mass and all of its positive charge

Empty space = most of the atom

of protons = # of electrons, so atoms are neutral

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14
Q

Periodic table

A

Elements are in order of increasing atomic number

Row = period
Column = group/family
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15
Q

Group 1A

A

Alkali metals

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16
Q

Group 2A

A

Alkaline earth metals

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17
Q

Groups XB

A

Transition metals

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18
Q

Groups XB - inserted rows

A

Inner transition metals

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19
Q

Group 7A

20
Q

Group 8A

A

Noble/inert gases

21
Q

Atomic number

A

Z

Number of protons

22
Q

Mass number

A

A

Number of protons + neutrons

23
Q

Chemical symbol

A

X

Chemical abbreviation

24
Q

X-A

A

Chemical-Mass #

25
Molecule
2+ atoms in DEFINITE arrangement, held together by chemical forces
26
Diatomic molecule
2-atom molecule
27
Diatomic molecules in nature (7)
``` Hydrogen (H) Nitrogen (N) Fluorine (F) Oxygen (O) Iodine (I) Chlorine (Cl) Bromine (Br) ``` H + N through F + F down to I "Have No Fear Of Ice Cold Beer"
28
Polyatomic molecule
>2 atom molecule
29
Polyatomic molecules in nature
Phosphorus (P4) Sulfur (S4) Selenium (Se4) (Oxygen (O3)) (remaining 3 Other Nonmetals angled in diatomic molecules N, O, F, Cl, Br
30
Cation
Positively charged ion
31
Anion
Negatively charged ion
32
Monatomic ion
1-atom ion
33
Polyatomic ion
2+ atom ion
34
Main-group/representative elements
A groups | Properties tend to be largely predictable based on location in table
35
Transition elements
B groups | Properties tend to be less predictable simply based on location in table
36
Metals
``` Solids at room temperature (EXCEPT MERCURY, Hg) Lustrous (shiny) Good conductors of heat/electricity Malleable Ductile High melting points, high densities Tends to lose electrons ``` Form ionic compounds with nonmetals Rarely combine with other metals
37
Metals found in free states (3) | "Noble metals"
Silver (Ag) Platinum (Pt) Gold (Au)
38
Nonmetals
``` Not lustrous (shiny) Poor conductors of heat/electricity Not malleable Not ductile Fairly low melting points & densities Tend to gain electrons ``` Form molecular compounds with each other (and metalloids) Form ionic compounds with metals BROMINE (Br) is liquid at room temperature
39
Metalloids
Properties are between metals and nonmetals Some are semiconductors ``` Boron (B) through Astatine (At) EXCLUDING Aluminum (Al) (and Polonium (Po)) ```
40
Transition metals with predictable charge (3)
Silver (Ag) - Group 1B = 1+ charge Zinc (Zn) - Group 2B = 2+ charge Cadmium (Cd) - Group 2B = 2+ charge
41
Atomic mass
amu Mass of an atom Based on carbon-12
42
Average atomic mass
Weighted average of all naturally occurring isotopes of an element Avg = (amu)(% abundance)+(amu)(% abundance)
43
Mass spectrometry
Separates particles according to mass | Used to determine masses of atoms & % abundances
44
1 mole (Avogadro's number)
6.022 x 10^23 objects
45
Molar mass
Mass of 1 mole of atoms of an element, expressed in grams x amu = x g/mol