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Chemestry > CH2) Atoms, Molecules, and Ions > Flashcards

CH2) Atoms, Molecules, and Ions Flashcards

1
Q

Structure of Matter

Atoms

A

Composed of electrons, protons and neutrons

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2
Q

The structure of matter

Molecules

A

Combination of atoms

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3
Q

the structure of matter

Ions

A

charged particles

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4
Q

Jhon Dalton and Atomic theory

A
  • Different conbinations produce different compounds
  • Atoms of difference elements have different masses
  • no atom disapears or is changed in chemical reaction
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5
Q

Fundamental laws of matter

3 fundamental laws of matter

A
  • law of conservation of mass
  • lasw of constant composition
  • laws of multiple proportions
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6
Q

Components of the Atom

what are atoms made of? and how do we know that?

A
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7
Q

The elctron and the Atom

A
  • every atom has at least one electron
  • atoms are known that have one hundred or more electrons
  • there is one elctron for each positive charge in an atom
  • electrical neutrality us maintained
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8
Q

The plum-pudding Model

A
  • J.J thomson proposed the atom as a positively charged spehere
  • whithin the spehere are eletrons
  • Plum-pudding or raisin-bread model
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9
Q

Protns and Neutrons- The nucleus

A
  • 1911 Rutherford bombarded of gold foil with a particle (helium atom without electrons)
  • Expected to see the particles pass through the foil
  • Found that some of the aplha particles were deflected by the foil
  • led to the discovery of a region of heavy mass at the center of the atom
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10
Q

Rutherdord’s model

A
  • rutherford’s exoeriment revealed a small, dense core with positive charge
  • electrons are outside this core
  • most of the atom is empty space
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11
Q

Nuclear Particles

1) protons

A
  • mass nearly eqaul to the H atom
  • positive charge
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12
Q

2) Neutrons- Discovered by Chadwick in 1934

A
  • mass slightly greater than that of the proton
  • no charge
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13
Q

Mass and the atom

A
  • more than 99% of the atomic mass is concentrated in the nucleus
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14
Q

Termininology

Atomic number, z

A
  • number of protons in the atom
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15
Q

Mass number, A

A
  • number of protons plus number of neutrons
  • A is the mass number
  • Z is the atomic number
  • X is the chemical sysmbol
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16
Q

Examples

1) An isotope of cobalt(z+27) is used in radiation cancer therapy, it has 33 neutrons, what is its nuclear symbol?

A
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17
Q

Isotopes

A
  • 2 atoms of the same element
  • same atomic number
  • different mass numbers
  • number of neutrons is A minus Z
  • number odf neutrons differs between isotopes
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18
Q

Isotopes of hydrogen

A
  • 1H, 2h, 3h
  • hydrogen, deuterium, tritium
  • different masses
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19
Q

Atomic Masses: The carbon-12 scale

A
  • Unit is the atomic mass unit (amu)
  • Mass of one 12C atom= 12 amu (exactly)
  • Note that 12C and C-12 mean the same thing
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20
Q

Determine Atomic Masses

A
  • can be determined to highly
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21
Q

isotopic abundance

A
  • determine hte mass of an element, we must know the mass
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22
Q

Mass Spectrum of CI

A
  • the mass spectrum is a plot of abundance vs. mass
  • the area under the peak in the mass spectogram gives the isotopic abundance
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23
Q

Carbon

A
  • 12
24
Q

Isotopic Abudance

A
  • determine the mass of an element, we must know the mass of each isotope and the atom perfent of the isitopes (isotopic abundance)
25
Q

Masses of individuals atoms

A
  • many porpouses, relative masses- not sufficient
  • necessary to know the mass of an atom in grams- quatitiy of matter can be determine weighing
  • number that converts the mass of an atom in atomic mass units
26
Q

Examples:
NB. 6.022x10^23=

A

atomic mass in grams

27
Q

Periods and groups

horixzontal rows are periods

A
  • first period is H and He
  • ## Second period is Li-Ne
28
Q
A
29
Q

Blocks in the periodidc table

main groups elements

A

1,2,13-18

30
Q

transition metals

A
  • 3-12
31
Q

post transition metals

A
  • Elements in groups 13-15 to the right of the transition metals
  • Ga, In, Ti, Sn, PB, Bi, Po
32
Q

Groups with common names

group 1:

A

Alkali metals

33
Q

group 2

A

Alkali earths

34
Q

group 3

A

noble or inert gases

35
Q

group 4

A

helogens

36
Q

group 5

A

chalcogenes

37
Q

group 6

A

Pnictogens

38
Q

Importance of group

A

similar chemical properties

39
Q

Mendeleev

A
  • Dmitri mendeleev, 1836-1907
  • ## Arranged elements by chemical properties
40
Q

Metals and nonmetals

A
41
Q

Some elements

A
  • Sulfur (nonmetal), antimony(metalloid) and silver (metal)
42
Q

Molecules

A

2 or more atoms may combine to form a molecule
- atoms involved are often nonmetals
- covalent bonds are strong forces that hold the atoms together

43
Q

Molecular Formulas

A
  • Number of each atom is indicated
44
Q

Structrurals formula

A

show bonding patterns within the molecule

45
Q

Condensed Structural formulas

A

suggest the bonding pattern and highlight specific parts of a molecule. Such as the reactive group of

46
Q

Molecular Elements

A
  • some exist as molecules, including such common ones as oxygen, hydrogen and nitrogen
47
Q

Ions

A
  • when atoms or molecules lose or gain electrons, they form changed particles called ions
  • Na->Na+ +e-
  • O+ 2e- ->O^2-
  • Cation (+)
  • Anions (-)
  • no change in number of protons in the nucleus when an ion forms
48
Q

Polyatomic ions

A
  • groups of atoms may carry a charge; these are polyatomic ions
  • Oh-, hYDROGEN ION
  • NH4+, ammonium ion
49
Q

Ionic Compounds

A
  • Compounds can form between anions and cations
  • Sodium cloride, Nacl
50
Q

forces between ions

A
  • Ionic compounds are hekd together bby strong forces called ionic bonds
  • Electrostatic attraction of + and - for each other
  • compounds are usually solids at room temperature
  • high melting points
  • may be water- soluble
51
Q

Solutions pf inoic compounds

A
  • when and ionic compound dissolves in water, the ions are relaae from each other
  • presence of ions in the solution leads to electrical conductivity
  • strong electrolytes
  • when molecular compounds dissolce in water, no ions are formed
  • without ions, solutions does not conduct
52
Q

Formulas of ionic compounds

A
  • charge balance
  • each positive charge must have a negative charge to balance it
  • ccalsium chloride, CaCl 2
  • Ca2+
  • two Cl- ions are required for charge balance
53
Q

Noble gas connections

A

Atoms close to a noble gas (group18) form ions- conatin same number of electrons as the neighboring noble gas atom
- Applies to Groups 1,2,16 and 17, plus AI (Ai3+) AND N(N3)

54
Q

Cations of transitions and Post-transition metals
- Iron

A

Commonly forms Fe2+ and Fe3+

55
Q

Lead

A
  • commonly forms Pb2+ and Pb4+
56
Q

Polyatomic ions

A

There are only 2 common polyatomic cations
- NH4+ and Hg2^

Chemestry (5 decks)

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