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Chemistry > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

According to Dalton’s Atomic theory Elements are composed of _________.

A

atoms; tiny, hard, unbreakable spheres

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2
Q

According to Dalton’s Atomic theory all atoms of a given element are ___________.

A

identical; atoms of different elements are different, every carbon atom is identical to every other carbon atom, but carbon atoms are different than sulfur atoms

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3
Q

According to Dalton’s Atomic theory atoms combine in _____, __________ ratios to form ________ of ___________

A
  • simple
  • whole number
  • molecules
  • compounds
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4
Q

Atoms combine as whole atoms because…

A

atoms are unbreakable

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5
Q

Each molecule of a compound contains the exact same ______ and ________ of atoms

A
  • types
  • numbers
  • law of constant composition* - i.e. H2O will always contain 2 Hydrogens and 1 Oxygen; Hydrogen peroxide will always have 2 hydrogens and 2 oxygens
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6
Q

According to Dalton’s Atomic theory atoms are not _______ or ________ into another type during a chemical rxn.

A
  • broken
  • changed

*all atoms present before the reaction are present after

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7
Q

According to Dalton’s Atomic theory atoms are not ______ or _______they are just ________

A
  • created
  • destroyed
  • rearranged
  • therefore the total mass will remain the same this is called the law of conservation of mass.
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8
Q

Can atoms change into a different type of atom during a chemical reaction?

A

No, atoms of one element do not change into Adams of another element in a chemical reaction.

Lead cannot be turned into gold via chem. rxn

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9
Q

Scientists such as JJ Thomson and others showed that atom had pieces called __________

A

electrons

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10
Q

Thomson discover about electrons?

A

He discovered that electrons are smaller than atoms and carry a negative charge of 1-

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11
Q

1 e-

A

One electron with a charge of one minus

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12
Q

5 e-

A

Five electrons with a total charge of five minus

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13
Q

Chemical reactions _______atoms.

A

rearrange

CH4 + O2 —–> CO2 + H2O

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14
Q

A (3g) + B (5g) = C + D (?)

A

8g

law of conservation of mass

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15
Q

Two kinds of charge_______and ______.

A

positive

negative

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16
Q

If you have to positively charged magnets will they attract or repel?

A

repel, because like charges repel and opposite charges attract.

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17
Q

an atom has the same number of protons and electrons what is the atom’s charge?

A

the atom is neutral.

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18
Q

If something has no charge, or the same number of charges what is it called?

A

neutral

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19
Q

What are the significant points of Rutherford’s interpretation of the nuclear model?

A
  1. the atom contains a tiny dense center called the nucleus.
  2. The nucleus has essentially the entire mass of the atom.
  3. The nucleus is positively charged.
  4. the electrons move around in the empty space of the atoms surrounding the nucleus.
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20
Q

how much space does the nucleus of an atom take up?

A

1/10 trillionth of the volume of the atom

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21
Q

Trying to contribute to the mass of an atom?

A

Yes but the amount of mass they contribute is so insignificant that they practically give no mass to the atom.

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22
Q

Positively charged particles are called __________.

A

Protons

*Protons have a positive charge of 1+

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23
Q

Who proposed that there was a positively charged particle in the nucleus of an atom that has the same amount of charges an electron?

A

Rutherford

he discovered this based on measurements of the nuclear charge of elements

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24
Q

1p+

A

one proton

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25
Q

5p+

A

five protons

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26
Q

in order for an atom to be neutral it must have the same amount of _______ and _____.

A

protons
electrons

because p+ and e- have the same amount of charge

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27
Q

In addition to the proton Rutherford proposed the existance of another type of subatomic particle in the nucleus called the ___________.

A

neutron

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28
Q

What is the charge of a neutron?

A

neutrons have no charge.

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29
Q

The masses of protons and neutrons are approximately ___________.

A

the same

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30
Q

1n0

A

1 neutron

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31
Q

5n0

A

five neutrons

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32
Q

the nucleus of an atom contains _______ and _______.

A

protons

neutrons

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33
Q

what is the diameter of the nucleus of an atom?

A

10^-13

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34
Q

What are the 3 subatomic particles that make up an atom?

A

proton
neutron
electron

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35
Q

e- move outside the nucleus with an average distance of about 10^-8 cm ….

A

therefore the radius of the atom is about 100,000 times larger than the radius of the nucleus.

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36
Q

AMU

A

atomic mass unit; a common unit to express mass for atoms.

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37
Q

a proton has the mass of

A

~ 1 amu

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38
Q

a neutron has the mass of

A

~ 1 amu

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39
Q

an electron has the mass of

A

~ 0 amu

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40
Q

if the charge of an atom changes the amount of which subatomic particle has changed?

A

the amount of e- because if the amount of p+ changes then the element changes because an atom of a certain element always has the same number of p+

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41
Q

each element has a ___________ number of protons in its nucleus.

A

unique

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42
Q

atomic number

A

the number of protons in the nucleus of an atom

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43
Q

How are the elements on the periodic table of elements arranged?

A

in order of their atomic numbers

44
Q

Each element has a unique ____ and _______.

A

name
symbol

the symbol is made up of one or two letters One capital letter by itself or with a lowercase letter.

45
Q

Z= 11

A

an atom has 11 protons because Z represents atomic number which is the number of protons in an atom.

46
Q

Z

A

atomic #= # of protons

47
Q

What is Z of Boron?

A

5

48
Q

atomic mass

A

the mass of an atom of a chemical element expressed in atomic mass units. It is approximately equivalent to the number of protons and neutrons in the atom (the mass number) or to the average number allowing for the relative abundances of different isotopes.

49
Q

Mendeleev

A
  • organized the elements according to atomic mass
  • while doing this he recognized a repeating pattern of properties
  • Periodic law
  • he used the pattern he discovered to predict the properties of undiscovered elements
50
Q

Periodic law

A

when the elements are arranged in order of increasing relative mass, certain sets of properties recur periodically.

51
Q

What are the 7 metalloids?

A
  1. Boron
  2. Silicon
  3. Germanium
  4. Arsenic
  5. Antimony
  6. Tellurium
  7. Astatine
52
Q

Boron

A

Z = 5
Atomic mass: 10.81 amu
Symbol: B

53
Q

Silicon

A

Z = 14
Atomic mass: 28.09 amu
Symbol: Si

54
Q

Germanium

A

Z = 32
Atomic mass: 72.63 amu
Symbol: Ge

55
Q

Arsenic

A

Z = 33
Atomic mass: 74.92 amu
Symbol: As

56
Q

Antimony

A

Z = 51
Atomic mass: 121.75 amu
Symbol: Sb

57
Q

Tellurium

A

Z = 52
Atomic mass: 127.60 amu
Symbol: Te

58
Q

Astatine

A

Z = 85
Atomic mass: 210 amu
Symbol: At

59
Q

Metals

A
  • solid at 25 degrees Celsius except for mercury
  • reflective shiny surface
  • conducts heat well
  • conducts electricity well
  • malleable
  • ductile
  • loses e- and becomes a cation in chem rxns
  • 75% of elements are metals
  • lower left on the table
60
Q

Nonmetals

A
  • poor conductors of heat and electricity
  • solids are brittle
  • gains electrons in chem. rxns (becomes anions)
  • if already has extra e- it won’t want more
  • upper right on the table except hydrogen
61
Q

Metalloids

A
  • show some properties of metals and nonmetals
  • also known as semi conductors

*ex. silicon (metalloid) is shiny, brittle conducts electricity but does not conduct heat well (semiconductor)

62
Q

In the modern periodic table of elements, how are elements with similar chemical and physical properties grouped?

A

elements with similar chemical and physical properties are grouped in in columns called groups or families

*families are labled by a number and a letter at the top of a column

63
Q

In the modern periodic table of elements rows are called ____________.

A

periods

64
Q

‘A’ groups

A

main group

65
Q

‘B’ group

A

transition elements (all metals)

66
Q

Inner Transition Elements

A

bottom rows

67
Q

Group 1A

A

Alkali metals

  • hydrogen is placed here though it doesn’t belong
  • soft low melting points
  • low density
  • flame test; Li = red, Na = yellow, K = violet
  • very reactive
  • never find uncombined in nature
68
Q

what type of sodium is included in our diet?

A

Na+

69
Q

Why are chemicals reactive?

A

chemicals are reactive when they are unstable, they will react because they are looking for stability; if an element is unreactive it is stable

70
Q

What are the Alkali metals?

A

Lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), francium (Fr)

71
Q

Group 2A

A

Alkaline Earth metals

  • harder than alkali metals
  • higher melting point
  • denser
  • flame tests; Ca = red, Sr = red, Ba = yellow-green
  • reactive but less than corresponding alkali metal
72
Q

What are the Alkaline earth metals?

A

Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba)

73
Q

Group 7A

A

Halogens

  • nonmetals
  • F2 and Cl2 gases; Br2 liquid,; I2 solid
  • all diatomic (more stable as a pair)
  • very reactiveHelium
74
Q

What are the Halogens?

A

Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I)

75
Q

Group 8A

A

Noble gases

  • all gases at room temperature (very low melting and boiling points)
  • very unreactive practically inert
  • very hard to remove e- from or give an e- to.
76
Q

What are the noble gases?

A

Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe)

77
Q

The number of protons determines the _____________.

A

element; all Na atoms have 11 protons

78
Q

In a chemical change the number of protons in an atom does not __________.

A

change

79
Q

electrically charged atoms in a compound are called?

A

ions

+ cation
- anion

80
Q

How do atoms acquire a charge?

A

by gaining or losing e- (NOT PROTONS!)

81
Q

Ion charge =

A

protons - # electrons

82
Q

Cations

A

positive charge
made by losing e-
more protons than e-
usually metals

83
Q

Anions

A

negative charge
made by gaining e-
more e- than protons
usually form from nonmetals

84
Q

Na+

A

sodium ion (cation)

85
Q

What kind of ions do metals form?

A

cations

86
Q

How are cations named?

A

cations are named the same as the metal but with ion added on

87
Q

The charge of a cation can be determined from the _______number on the periodic table.

A

group;

Group 1A —-> 1+, Group 2A —-> 2+ (Al, Ga, In) —–> 3+

88
Q

Na vs. Na +

A

sodium and sodium ion

89
Q

Ca and Ca 2+

A

Calcium and calcium ion

90
Q

nonmetals tend to gain ________.

A

e-

91
Q

How are nonmetals (anions) with a charge named?

A

base name of nonmetal + ide +ion

92
Q

O vs O2-

A

oxygen and Oxide ion

93
Q

Base names for Nonmetals

A 
H: hydr 1-
N: nitr 3-
P: phosph 3-
O: ox 2-
S: sulf 2-
F: fluor 1-
Cl: chlor 1-
Br: brom 1-
Se: selen 2-
I: iod 1-
Te: tellur 2-
94
Q

The charge on an anion can be determined from the group ________ on the _________ -______

A

number
periodic table
*Group 7A —>1-
Group 6A—>2-

95
Q

Isoelectronic

A

different elements with the same number of e-

96
Q

isotope

A

atoms of an element that are the same but have different weights *discovered by Soddy

Identical elements with different masses due to different numbers of neutrons

97
Q

There are 2 isotopes of chlorine found in nature, one that has a mass of about 35 amu and another that weighs 37 amu why is the atomic mass on the periodic table of elements for chlorine 35.45 amu?

A

because there is more Chlorine-35 in nature; The observed mass is a weighted average of the weights of all the naturally occuring atoms

98
Q

How do isotopes differ?

A

Allz isotopes have the same protons but different numbers of neutrons

isotopes of an element have different masses

99
Q

How are isotopes identified?

A

isotopes are identified by their mass numbers (A) Protons+neutrons

100
Q

A

A

mass number (protons+neutrons)

101
Q

Atomic number

A

Z

number of protons

102
Q

Mass number

A

A
whole number
Protons+neutrons

103
Q

isotopic notation

A

Ne-21

104
Q

Atomic Symbol

A/Z X = X-A

A 
A= mass number
Z= atomic number
X= element
105
Q

Atomic mass

A

represents the average mass for each element

found directly beneath element symbol

106
Q

All isotope percentages should equal ________.

A

100%

Chemistry (5 decks)

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