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chem 100 final > unit two > Flashcards

unit two Flashcards

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1
Q

solid that forms when two solutions are mixed

A

precipitate

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2
Q

what is a double replacement precipitate reaction

A

AX + BY → AY + BX

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3
Q

chemical particle present in greatest abundance in solution, ionized

A

major species

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4
Q

chemical particle present in lesser abundance in the solution, unionized

A

minor species

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5
Q

equation that replaces the formulas of the dissolved substances with the major species in solution

A

total ionic equation

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6
Q

ionic equation from which all spectators have been removed

A

net ionic equation

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7
Q

how to write the net ionic equation

A

write balanced conventional equation, then write total ionic equation, then remove the spectator ions

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8
Q

reaction where electrons are transferred from one species to another

A

single replacement oxidation reaction

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9
Q

Species that loses electrons is said to be

A

oxidized

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10
Q

Species that gains electrons is said to be

A

reduced

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11
Q

what is a single replacement reaction

A

A + BX → AX + B

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12
Q

reaction where the element that gets replaced undergoes a change in its oxidation state (loses or gains electrons)

A

redox reaction

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13
Q

lists metal elements and hydrogen in order of reactivity in a single-replacement redox reaction

A

activity series

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14
Q

a number assigned to each element in a species that reflects its oxidation state, and is used to keep track of electrons

A

oxidation number

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15
Q

the Oxidation number of each atom in any elemental substance is:

A

zero

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16
Q

the oxidation number of a monatomic ion is the:

A

same as the charge of the ion

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17
Q

oxidation number of combined oxygen is

A

-2

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18
Q

oxidation number of combined hydrogen is

A

+1

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19
Q

the sum of the oxidation numbers of all atoms in a molecule or polyatomic ion is :

A

equal to the charge on the species

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20
Q

reaction where acid and base react to yield water, which is neutral, that is neither an acid nor a base.

A

neutralization reaction

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21
Q

energy in the form of electric and magnetic waves that propagate (move) in space

A

electromagnetic radiation

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22
Q

em radiation spectrum from lowest to highest frequency

A

Radio waves
Microwaves
Infrared
Visible light
Ultraviolet
X-Ray
Gamma Rays

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23
Q

em radiation spectrum from shortest to longest wavelength

A

gamma rays, x ray, ultraviolet, visible light, infrared, microwaves, radio waves

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24
Q

Energy released by the electron in the form of a massless packet of electromagnetic radiation

A

photon

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25
Q

movement of an electron between orbits

A

quantum jump/leap

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26
Q

the four quantum numbers that describe electron energy levels in an atom:

A

principal energy level, sublevel, orbital, and number of electrons in an orbital

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27
Q

mathematically described region in space around a nucleus in which there is a high probability of finding an electron

A

orbitals

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28
Q

the s sublevel has _ orbitals

A

1

29
Q

the p sublevel has _ orbitals

A

3

30
Q

the d sublevel has _ orbitals

A

5

31
Q

the f sublevel has _ orbitals

A

7

32
Q

concept that limits the population of any orbital to two electrons

A

pauli exclusion principle

33
Q

the distribution of electrons among the orbitals of the atom of the element

A

electron configuration of an element

34
Q

the symbol of the element is surrounded by a number of dots that matches the number of valence electrons.

A

lewis/electron dot symbol

35
Q

highest-energy s and p electrons in an atom which determines bonding characteristics of an element

A

valence electron

36
Q

how to determine number of valence electrons

A

group number, for main group elements only

37
Q

elements that have the same number of electrons in the highest energy level (outermost shell)

A

group(s)

38
Q

elements that use the same highest energy level (outermost shell of electrons)

A

period

39
Q

how to write electron configuration

A

Find elements in the periodic table, identify and write the configuration of the highest occupied energy sublevel.
To the left of what is written, list all lower-energy sublevels in order of increasing energy
For each filled lower-energy sublevel, write as a superscript the number of electrons that fill that sublevel
Confirm that the total number of electrons is the same as the atom number.
As we hit the transition metals region of the PT, interruptions appear at 3d electrons.

40
Q

on the PT atom size decreases from

A

left to right

41
Q

on the PT atom size increases from top to bottom

A

top to bottom

42
Q

Energy required to remove a second electron from the 1+ ion of an element

A

second ionization energy

43
Q

energy required to remove an electron from an ion with a 2+ charge

A

third ionization energy

44
Q

elements with similar chemical properties due to similar valence electron configuration appear in the same group of the table

A

chemical families

45
Q

unreactive elemental gases appearing in 8A of the periodic table

A

noble gas

46
Q

Belong to group 1A of the periodic table

A

alkali metals

47
Q

in forming bonds, atoms seek to have 8 electrons in their outermost shell

A

octet rule

48
Q

positively charged ion

A

cation

49
Q

negatively charged ion

A

anion

50
Q

cations are _

A

metals

51
Q

anions are _

A

nonmetals

52
Q

chemical bond between two or more nonmetal atoms that share one or more pair of electrons to make a molecular compound

A

covalent bond

53
Q

what is the representation that uses an electron dot symbol is used to show the bonding arrangement between atoms in a molecule

A

lewis diagram

54
Q

unshared electron pairs

A

lone pair

55
Q

the ability of an atom of that element in a molecule to attract bonding electron pairs to itself

A

electronegativity of an element

56
Q

bonding electrons are shared equally between the two nuclei

A

nonpolar bond

57
Q

bonding electrons that are shared unequally between the two nuclei

A

bonding electrons are shared equally between the two nuclei

58
Q

bonding that involves transfer of electrons

A

ionic bonding

59
Q

how to Determine if a single-replacement reaction occurs using the activity series.

A

Basically read the activity series chart up and down, anything below an element can be replaced by the element above it

60
Q

what shape are the orbitals

A

s: spherical, p: dumbbell, d: butterfly idk

61
Q

what shape is the s orbital

A

spherical

62
Q

2 things, 2 bonding groups, 180 degrees

A

linear linear

63
Q

3 things, 3 bonding groups, 120 degrees

A

trigonal planar trigonal planar

64
Q

3 things, 2 bonding groups, less than 120

A

trigonal planar bent

65
Q

4 things, 4 bonding groups, 109.5

A

tetrahedral tetrahedral

66
Q

4 things, 3 bonding groups, less than 109.5

A

tetrahedral trigonal pyramidal

67
Q

4 things, 2 bonding groups, less than 109.5

A

tetrahedral bent

68
Q
A

chem 100 final (4 decks)

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