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Chemistry > ATI 7: Chem Tutor Geek > Flashcards

ATI 7: Chem Tutor Geek Flashcards

1
Q

What determines if a substance is a Solid, Liquid, Gas (2)

A
  1. How far apart the molecules are (within the substance)
  2. How fast these molecules are moving
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2
Q

Do molecules in a solid move?

A

No, but they vibrate

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3
Q

Gas to Solid is called

A

Deposition

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4
Q

Solid to a gas is called

A

Sublimation

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5
Q

As temperature increases the atmospheric pressure……

As temperature decreases the atmospheric pressure….

A

Decreases

Increases

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6
Q

The heating curve includes these phase changes. (3)

A

Melting, vaporization, sublimation

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7
Q

Cooling curve includes these 3 phase changes

A

Condensation, freezing, deposition

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8
Q

Matter can be divided into 2 categories

A

Pure substances & Mixtures

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9
Q

Pure substances can be broken down into (2)

A

Elements & Compounds

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10
Q

_______ is a group of two or more atoms held together by chemical bonds.

________ is a substance which is formed by two or more different types of elements which are united chemically in a fixed proportion.

A

Molecule

Compound

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11
Q

Which subatomic particle has the largest mass

A

Neutron

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12
Q

Any element that is made of 2 atoms in its natural form

A

Diatomic

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13
Q

hydrogen (H), nitrogen (N), oxygen (O), fluorine (F), chlorine (Cl), bromine (Br), and iodine (I).

Are this type of element

A

Diatomic

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14
Q

Groups or families all have a number of valance electrons equal to their group number.

which way on the periodic table do they go?

A

Down

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15
Q

Periods on the table indicate the number of electron orbitals

They go which direction on the table

A

To the right, across

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16
Q

Metals are (cations / anions) in an ionic bond?

Is this positive or negative

A

Cations

Positive

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17
Q

Group 1A are this kind of element?

A

Alkali metals

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18
Q

Group 2A elements are this kind

A

Alkaline earth metals

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19
Q

Group 7A are called

A

Halogens

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20
Q

Group 8A are calles

A

Noble gases

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21
Q

Between group 2 and 13 are

A

Transitional metals

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22
Q

Highly reactive
Form cations with +1 charge

A

Alkali metals

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23
Q

Highly reactive
Form cations with a +2 charge

A

Alkaline Earth metals

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24
Q

This type of element consists of diatomic elements

Forms anions with a negative -1 charge

A

Halogens

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25
Q

Least reactive
Aka “inert gases”

A

Noble Gases

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26
Q

The average number of protons and neutrons for all natural isotopes of an element is called…

Where is it found on the periodic table

A

Atomic mass

Below the atomic symbol

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27
Q

The Elemental Symbol is written how?

A

Top
Mass number (Protons & Neutrons)

Bottom
Atomic number
(Number of protons)

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28
Q

Metals are (least / most) electronegativite

Non-metals are (least/ most) electronegativite

A

Metals: Least
Nonmetals: Most

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29
Q

All diatomic molecules have ____ bonds between the same atoms

A

Covalent

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30
Q

When the difference in electronegativity is greater than or equal to >0.5 this is called a Polar bond.

True or False

A

True

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31
Q

H - H which type of bond?

A

Non polar Covalent

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32
Q

C 2.5 - H 2.1 which type of bond?

A

Covalent

Non-polar

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33
Q

Ca - S type of bond

A

Ionic

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34
Q

O - H type of bond

A

Polar Covalent

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35
Q

How many electrons fit in the 1st - 7th energy level

A

1=2
2=8
3=18
4=32
5=50
6=72
7=98

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36
Q

Xe has an atomic number 54
It is located 8a group and 5th period

Describe where the electrons are located

A

1=2
2=8
3=18
4=18
5=8

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37
Q

2 factors that affect the size of an atom or the “atomic radii”

A
  1. Distance of the electron to the Proton
  2. The amount of protons in the nucleus
38
Q

Distance from center of the nucleus to the outer most electron is called?

A

Atomic radius

39
Q

Atomic radius increases how
Periods
Groups

A

Increases
Periods: Right to Left
Groups: Up to Down

40
Q

Why do atomic radii increase going from up to down on the periodic table?

A

As you go down each Peroid is 1 more electron shell so the radius is bigger due to more shells

41
Q

Why does the atomic radius increase as you go from Right to Left?

A

Right side= Higher atomic number, more protons, protons pull the electrons towards them due to being opposite charges, shrinking the radius.

The left has less protons than the right and has less of a pull towards the negative electrons

42
Q

Which had a larger atomic radius
Cation or regular element

A

Regular element

Due to there being more protons, they pull the electrons in making it smaller

43
Q

Are anions bigger or smaller than their neutral atom?

A

Bigger

Due to the electrons taking up more space

44
Q

_____ is the energy required to remove one or more valance electrons from a gaseous atom

A

Ionization Energy

45
Q

Ionization energy trend in the periodic table is

A

IE increasing going Up
IE increases going Right

46
Q

Ionization energy Exception

Be, Mg,CA are reversed with B,Al,GA
&
N,P,As are reversed with O,S,Se

True or False

47
Q

What is the difference between Electronegativitiy & Ionization Energy?

A

Electronegativity ATTRACTS electrons to form bonds (Covalent)

Ionization energy REMOVES electrons from a gaseous atom

48
Q

What is the most electronegativite atom? Pauling electronegativity scale

although in the Allred-Rochow scale, _____ has the highest electronegativity.)

A

F fluorine

He helium

49
Q

Acids are likely to begin with an H and be attached to a metal

True or False

A

False

A Non metal

Bases have an H attached to a metal

50
Q

Bases are likely to have an OH and/or a metal attached to an H

True or False

51
Q

This theory says that acids release Hydrogen (H+) ions in a solution

Bases release Hydroxide (OH-) ions in a solution

52
Q

This theory states that Acids are Proton donors

Bases are Proton acceptors

A

Bronsted-Lowry

53
Q

Bronsted Lowry

NH³ + H²O —-> NH⁴ + OH-

Which is the Bronsted Lowry Acid / Base

Which is the Conjugated Acid/ Base

A

NH³ Base
H²O Acid

NH⁴+ Acid
OH- Base

54
Q

Hcl —> H+ (+) Cl-

HCl + H²O —> H3O+ (+) Cl-

What type of Acid theory is this?
What is happening here?

A

Hydrochloric Acid is disassocating into hydrogen and chloride

Hydrochloric Acid is disassociate with water to become Hydronime (An Acid)

55
Q

Arrhenius

NaOH —-> Na+ (+) OH-

A

NaOH is arrhenius base

56
Q

HCl + H²O —> H³O+ (+) Cl-
What is happening here?
Is it a strong or weak acid, why?

A

HCl hydrochloric Acid is completely disassocating

Strong acid

57
Q

NaOH —> Na+ (+) OH-

Is this an example of a strong or weak base? Why?

A

Strong
Because it completely disassociates

58
Q

How many vacation days does a nurse get annually?

How many do you get?

A

Nurses receive an average of 26 vacation days.

0

Fuck DK security

59
Q

If a solution has Arrows Going Both Ways “reversible” is it a strong or weak acid/ base

60
Q

Which of the following are a homogeneous mixture

A: milk
B: air
C: blood
D: sand
E: oil and water
F: salt water
G: black coffee

61
Q

Which of the following express a compound

A: NaCl
B: H²
C: H²O
D: NH³
E: F²
F: Mg
G: He
H: CO²

62
Q

Which describes the compound
Electronegativity values given of each

 (3.0)C(2.5)Cl⁴

Polar-covalent
Non polar-covalent
Ionic
Neither

A

Polar-covalent

63
Q

35
Br
79.9

What is the average number of neutrons in bromine

A

44.9

Minus Atomic number (Protons)

From Atomic Mass (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)

64
Q

Odor
Enery change
Gas bubbles
Precipitate formation
Color change

As signs that a ____ has taken place

A

Chemical reaction

65
Q

Does a solid have (high or low) kinetic energy

66
Q

Bronsted-Lowry base is a Proton donor

True or False

A

False

Bronsted Lowry Acid is a Proton donor

67
Q

Which is true

Matter is anything that has mass and volume

Matter is anything that takes up space and has volune

A

Matter is anything that has mass and volume

68
Q

16 -2
O
8

What are the number of protons, electrons, neutrons

A

P=8
N=8
E=10

69
Q

How many of each subatomic particles does Aluminum with a +3 charge have

13
Al
26.982

A

P = 13
N = 14
E = 10

70
Q

What are the SI units for

Time
Length
Mass
Electric current
Thermodynamic temperature
Amount of substance
Luminous intensity

A

Second
Meter
Kilogram
Ampere
Kelvin
Mole
Candela

71
Q

Which of the phase changes requires a loss of heat

Sublimation
Melting
Deposition
Condescending
Freezing

A

Deposition
Condensing
Freezing

72
Q

A cooling curve does this to the molecules in a substance

A

Slows them down

73
Q

A heating curve does this to the molecules in a substance

A

Speeds them up

74
Q

Oxygen with 8 protons, 10 electrons, 8 neutrons is

An anion with a - 2 charge
A Cation with a - 2 charge
An anion with a + 2 charge
A Cation with a + 2 charge

A

An anion with a -2 charge

75
Q

NH3

Acid or base

A

Base

ammonia

76
Q

KOH

Acid or base

A

Base

potassium hydroxide

77
Q

NaHCO3

Acid or base

A

Base

sodium bicarbonate

78
Q

Na2CO3

Acid or base

A

Base

sodium carbonate

79
Q

NaOH

Acid or base

A

Base

sodium hydroxide

80
Q

HNO3
Acid or base

A

nitric acid

81
Q

HCl

Acid or base

A

Acid

Hydrochloric Acid

82
Q

H3PO4

Acid or base

A

Acid

phosphoric acid

83
Q

C2H4O2

Acid or base

A

Acid

acetic acid

84
Q

_____ is the tendency for an atom of a given chemical element to attract shared electrons when forming a chemical bond.

A

Electronegativity

85
Q

Hydrocarbon Bonds

Alkane

Alkenes

Alkyne

A

Alkane (all Single)

Alkenes (Single & atleast 1 double)

Alkyne (Single & atleast 1 triple)

86
Q

Water does not evaporate easily due to which chemical property

A

Hydrogen bonding

87
Q

Gas particles contain a high amount of which type of energy

88
Q

Which form of matter has the most potential energy stored in its bonds

89
Q

Does gas contain bonds and potential energy

A

No, only kinetic energy

90
Q

An element with 10 protons and 11 electrons will have which kind of charge (+1 / -1) and be called (Cation/ Anion)

Chemistry (14 decks)

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