Praxis Middle School Science-The Mole and Chemical Bonding Flashcards

1
Q

mole

A

that number whose mass in grams is numerically equal to the atomic mass, molecular mass, or formula mass of the substance

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2
Q

why do we have the mole?

A

a single atom or molecule weighs so little that it cannot be measured using a balance in the lab.

it is useful to have a system that permits a large number of chemical particles to be described as one unit.

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3
Q

avogrado’s number

A

the number of atoms, ions, molecules or anything else in one molecule, or 6.02 x 10^23

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4
Q

law of definite proportions (law of constant composition)

A

a pure compound, whatever its source, always contains definite or constant proportions of the elements by mass

it is a fixed composition

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5
Q

mixture

A

a material that can be separated by physical means into two or more substances

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6
Q

mixtures are classified into two types

A
  1. heterogeneous mixture: a mixture that consists of physically distinct parts, each with different properties. ex: chex mix.
  2. homogeneous mixture: (solution) a mixture that is uniform in its properties throughout a given sample.
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7
Q

formula

A

a shorthand that uses symbols and subscripts to show what is in a compound.

the letter symbols tell us what elements are involved.

the number signs tell us how many of each element are involved.

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8
Q

reacants

A

are found on the left side of the equation

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9
Q

products

A

found on the right side of the equation

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10
Q

chemical reaction

A

a chemical event in which one or more substances are formed.

energy is released. energy release can be slow or rapid.

ex: rapid= fireworks
slowly= the tarnishing of a spoon

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11
Q

chemical equilibrium

A

state reached when the quantities of reactants and products are no longer shifting, but the reaction may still proceed with equal forward and backward reaction

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12
Q

example of chemical equilibrium

A

C + O2 –> CO2

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13
Q

no matter is ever _________ or ________ in a chemical reaction.

A

gained or lost

therefore, the chemical equation must be balanced

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14
Q

ionic compounds are named with the ____ first

A

cation

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15
Q

cation

A

positive ion

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16
Q

nearly all cations in inorganic chemistry are

A

monatomic, meaning they consist of just one atom and are formed from a metal ion.

17
Q

anion

A

negative ion

named and written last

they’re formed from nonmetallic elements and are named by replacing the end of the element’s name with the suffix –ide.

18
Q

oxoanions

A

contain one element in combination with oxygen

end in the suffix –ate.

19
Q

water molecules often occupy positions within

A

the lattice of an ionic crystal, called hydrates.

20
Q

molecular compounds

A

compounds (usually composed entirely of nonmetals) making up molecules with a neutral charge

they’re named by placing the less electronegative atom first.

the suffix –ide is added to the second, more electronegative atom

21
Q

prefixes indicating numbers

A
1- mono
2- di
3- tri
4- tetra
5- penta
6- hexa
7- hepta
8- octa
9- nona
10- deca
22
Q

hydrocarbons

A

the simplest organic compounds, containing only carbon and hydrogen

23
Q

alkanes

A

a hydrocarbon compound containing only single bonds

24
Q

saturated

A

describing a hydrocarbon like an alkane that has the maximum number of hydrogen atoms possible for its carbon backbone

25
unsaturated
describing a hydrocarbon like an alkene that has fewer than the maximum number of hydrogen atoms possible
26
alkenes
also called olefins, are hydrocarbons that contain one or more double bonds.
27
alkynes
hydrocarbons that contain one or more triple bonds.
28
alkelynes
hydrocarbons with double and triple bonds.
29
aromatic hydrocarbons
hydrocarbons that structurally are related to benzene or made of benzene molecules fused together called arenes all atoms lie in the same plane, they are flat. electrons are free to migrate throughout the molecule
30
hydrogen bond
the weakest of the three types of chemical bonds formed when one electronegative atom shares a hydrogen atom with another electronegative atom ex: water bonding with ammona (NH3)
31
valence electrons
outermost electrons they are involved in the bonding process they determine the properties of the element
32
chemical bonds are formed when
atoms with incomplete valence shells share or completely transfer their valence electrons
33
condensed structural formulas
a representation of a chemical compound: the elemental atoms and their sub/superscripts ex: ethanol is CH3CH2OH
34
line angle drawings
a representation of a chemical compound: angled lines that intersect and terminate with the designated elements
35
lewis dot structure
a method for keeping track of each atom's valence electrons in a molecule