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10th grade > Chem Final Sem 1 > Flashcards

Chem Final Sem 1 Flashcards

1
Q

Creation Mandate: What is it where do you find it

A

What God wants us to do: Create products and solve problems, Weigh the consequences of actions, Seek a balance, Love neighbors

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2
Q

Scientific models: What are they? What are they used for

A

Simplifies something in the world to explain, describe, or represent

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3
Q

When was chemistry first taught as an academic discipline

A

1800

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4
Q

Biblical worldview

A

How someone sees and interprets life using Bible as guide

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5
Q

Quantitative data

A

Data with numbers, measurable

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6
Q

Qualitative data

A

Data without numbers, not measurable

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7
Q

Scientific method

A

Observation
Question
Hypothesis
Experiment
Data collection
Conclusion
Retest

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8
Q

DIfference between theory and hypothesis

A

Hypothesis: Suggested solution to problem, testable, written as if… then, predicts outcome
Theory: Principle formed to explain things already shown in data

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9
Q

Observation

A

What do you see happening

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10
Q

Data

A

Info/fact/stats collected for analysis

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11
Q

You set up an experiment to test the idea that the amount of nitrogen in the soil affects plant growth
What is your hypothesis
What would be the experimental and control group be
What is the dependent and independent variables

A

Hypothesis: If there is a lot of nitrogen, then plant growth improves
Experimental: Soil with a lot of nitrogen
Control: Normal soil
Dependent: Plant growth
Independent: Nitrogen, soil

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12
Q

Ex nihilo

A

Out of nothing

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13
Q

Density formula

A

Mass over volume

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14
Q

Physical property

A

We can measure without changing material into another substance

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15
Q

Chemical property

A

How matter acts when other materials are combined together
How material changes composition when enough energy is added to it

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16
Q

Conductivity

A

Ability of material to transfer heat or electricity between its particles

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17
Q

Ductility

A

Describes how easily materials can be drawn into thin wires

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18
Q

Malleability

A

How easily material can be hammered into shapes

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19
Q

Luster

A

based on whether the mineral is metallic or non-metallic

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20
Q

Physical change
Example: Spoiled milk or cut up paper

A

Change in physical properties
Substance remains same
Start with A end with A
Paper that is cut

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21
Q

Chemical change
Example: Spoiled milk or cut up paper

A

Substance changes
New substance formed
Composed of different particles
Start with A end with B
Spoiled milk

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22
Q

Mixtures: Heterogenous/homogenous/suspensions what are they

A

Hetero/suspension: Parts settle out bc gravity
Homo: Uniform mixture of 2+ pure substances

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23
Q

Diatomic element & Monatomic element & Polyatomic

A

Dia: O2, H2
Mon: Na, Ar
Poly: O3, S8

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24
Q

Polyatomic ion

A

groups of atoms covalently bonded together, but the group of atoms as a whole has a charge

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25
Q

5Fe₂
What is the 5

A

Coefficient: Number in front of formula which tells how many molecules/atoms present

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26
Q

5Fe₂
What is 2

A

Subscript: Number that indicates amnt of atoms/groups of atoms in formula

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27
Q

(Fe₂)₂

A

2 Fe₂

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28
Q

What is an ion

A

Positive or negative charged atom

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29
Q

Entropy

A

Measure of disorder in system

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30
Q

If you burn gasoline will entropy increase or decrease

A

Increase becausethe energy becomes less usable

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31
Q

Kelvin
What is 0 degrees Kelvin known as

A

Basic metric unit of temp
Absolute 0

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32
Q

How do you change from Celcius to Kelvin

A

+273.15 kelvins

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33
Q

Temp 12000k what is that in celsius

A

12000 - 273.15
926.85

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34
Q

Changes of common states of matter

A

Condensation: gas to liquid
Vaporization: liquid to gas
Freezing: liquid to solid
Melting: Solid to liquid
Sublimation: Solid to gas
Deposition: Gas to solid

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35
Q

Metric system
How many grams in 1 kg
How many milligrams in 1g

A

1000g
1000 milligrams

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36
Q

How many kg in 25,600g

A

25.6 kg

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37
Q

Percent error formula

A

|observed value - accepted value| divided by accepted value times 100

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38
Q

Accuracy and precision

A

Accuracy: How close measurement is to exact value
Precision: Indicates how repeatable measurement is

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39
Q

Law of definite composition

A

Every compound is formed of elements combined in specific ratios by mass that are unique for that compound

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40
Q

Electron, proton, neutron what are they
Which weighs the least

A

Subatomic particles
Electron

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41
Q

A number and Z number of atom
What A and Z

A

A: Atomic number
Z: Protons

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42
Q

Niels Bohr what did he propose

A

Concept of principal energy levels that he envisioned as set of circular tracks on which electrons orbited

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43
Q

Heisenberg Uncertainty Priciple

A

Impossible ot know both energy and location of an electron in an atom

44
Q

Pauli exclusion principle

A

No 2 electrons in an atom can have same address

45
Q

Afbau principle

A

Hypothetically electrons orbiting 1 or more atoms fill lowest available energy lvls before filling higher lvls

46
Q

Hund’s rule

A

As electrons fill sublvl, all orbitals receive 1 electron with same spin before they begin to pair

47
Q

4 parts of electrons address

A

N- energy level (1, 2, 3, 4 distance from nucleus)
L- energy orbital or sublevel (s, p, d, f)
M- how sublevel or orbital is arranged in 3D space
S- Spin (electron spin)

48
Q

What is s, p, d, f orbitals/sublvls
what is the maximum number of electrons that can be in each kind sublevel?

A

Sublvls inside principle lvl
S- 2
P- 6
D- 10
F- 14

49
Q

Electron configuration
Ex: Carbon 6

A

How electrons are arranged1s2 2s2 2p2

50
Q

Electron configuration for nitrogen (7 electrons)

A

1s2 2s2 2p3

51
Q

What does [He] mean in electron configuration

A

Helium 1s2

52
Q

Isotopes

A

Elements with different numbers of neutrons

53
Q

Carbon- 12, Carbon- 13 and Carbon- 14 have same number of ___________ and different number of __________

A

Protons
Neutrons

54
Q

Canutium has atomic number of 42 and atomic mass of 98 how many protons and neutrons does it have

A

42 protons
56 neutrons

55
Q

Carbon has 6 electrons. If it loses 1 electron what kind of charge will it have

A

Positive

56
Q

If Carbon gains 1 electron what charge will it have

A

Negaitive

57
Q

PO4 ^-3 is an atom, ion, element, or isotope

A

Ion

58
Q

Wavelength

A

Distance between 2 peaks or troughs in a wave

59
Q

Frequency

A

Number of waves (cycles) per second that pass given point in space

60
Q

What is relationship between frequency and wavelength

A

High frequency -> short wavelength
Small frequency -> long wavelength

61
Q

What are units of frequency and wavelength

A

Hertz

62
Q

What is h in c= hv

A

Wavelength

63
Q

C = 3 x 10^8 m/s and wavelength is 50 m what is frequency

A

3 x 10^8 = 50 v
V = 6 x 10^6 hz

64
Q

What did Newlands discover

A

Law of octaves

65
Q

Law of octaves

A

Connection with atomic mass and chemical properties

66
Q

What did Mendeleev do for creating periodic table

A

Elements arranged by atomic masses
Knew elements not yet discovered
Transition metals
Periodic law

67
Q

Lustrous

A

metallic

68
Q

Alkali metals
How many electrons do they lose or gain

A

Group 1
Very chemically reactive
Metallic and soft physical properties
Sodium, potassium, lithium, rubidium, cesium
Lose 1 electron

69
Q

Alkali earth metals
How many electrons do they lose or gain

A

Group 2
Denser, harder, higher melting points than alkali metals
Typically donate 2 electrons
Magnesium, calcium, strontium, barium, radium
Ex: Military flares, x-rays, bones

70
Q

Halogens

A

Group 17
More color, higher melting point, density
Most reactive out of all nonmetals
Used for halogen lights, bleach and medical uses

71
Q

Noble gases

A

Group 18
Colorless, odorless, tasteless
Rarely react
Used for balloons, diving, neon light

72
Q

Metalloids

A

Characteristics lying between those of metals and nonmetals
Semiconductors
Boron, silicon

73
Q

How does the size of a metal atom compare to its positive ion? Its negative ion?

A

Positive (Cation)- Bigger
Negative (Anion)- Smaller

74
Q

Ionization energy

A

Measures the energy required to remove an outermost electron
Trend- upper right corner

75
Q

Atomic radius

A

Measured using x-ray diffraction. Determined by electron cloud
Trend- lower left corner

76
Q

Ion size

A

Cation-bigger
Anion- smaller

77
Q

Electron affinity

A

measures the energy released when an electron joins an atom
Trend- upper right corner

78
Q

Electronegativity

A

Measure the attraction of bonded atoms to electrons?
Trend- upper right corner

79
Q

Why do atoms form bonds
What part of atom is involved in bonds

A

Lose energy
Gain stability
Valence electron

80
Q

When atoms bond, they want to have enough electrons to become like which family or group of elements

A

Noble gases

81
Q

Polarity of a bond btwn 2 atoms depend on what

A

Electronegativity

82
Q

What does deltaEN mean

A

Electronegativity

83
Q

What kind of bond would exist between Na and F

A

Ionic

84
Q

What is electrostatic force

A

+ and - charges in atoms that attract or repel each other

85
Q

What does the single dash btwn 2 atoms mean

A

2 electrons shared

86
Q

What does double dash btwn 2 atoms mean

A

2 pairs of 2 electrons shared

87
Q

What does triple dash btwn 2 atoms mean

A

3 pairs of 2 electrons shared

88
Q

Electron sea theory

A

All metal atoms in metallic solid contribute valence electronsto form a sea of electrons

89
Q

Which does electron sea theory explain regarding metals

A

Luster, conductivity, ductility

90
Q

Ionic compounds

A

Strong bonds
High melting points
Dense, brittle, hard
Good electron conductors if dissolved/molten

91
Q

Ionic compounds are they good at electrical conductivity

A

Yes

92
Q

Are ionic compounds easily broken as crystals

A

No

93
Q

*Sigma bonds
How are they formed
What is involved in their formation

A

Formed by head-to-head overlapping of atomic orbitals
Single bond

94
Q

Pi bonds
How are they formed
What is involved in their formation

A

The same phase overlap of atomic orbitals along a direction perpendicular to the internuclear axis
Found in double and triple bonds
Weaker than sigma bonds

95
Q

Which bond type is stronger sigma or pi

A

Sigma

96
Q

How many sigma and pi bonds are in
H2O, CH4, N2, HCN, O2

A

H2O- 2 sigma
CH4- 4 Sigma
N2- 1 sigma 2 pi
HCN- 2 sigma 2 pi
O2- 1 sigma 1 pi

97
Q

Which bond would be the strongest single, double, or triple

A

Triple

98
Q

Resonance

A

No single Lewis structure can totally describe how electrons are distributed

99
Q

What makes a good graph

A

Title on top of graph
Labels on x and y axis
Units to go with labels on x and y axis

100
Q

Why do we need to wear eye goggles when working with glass or liquids other than water

A

To protect your eyes

101
Q

Why would you need to wear a lab apron during a lab

A

To protect from chemicals

102
Q

If you have long hair why should you tie it back when working with fire

A

So hair doesn’t catch on fire

103
Q

Why use tongs when working with glass beaker

A

To safely grab very hot items

104
Q

What is purpose of wire gauze

A

Place between beaker or dish and lab burner

105
Q

Inductive vs Deductive reasoning

A

Inductive- Begins with observation
Deductive- Begins with theory

106
Q

Bonds sigma and pi

A

Single- 1 sigma
Double- 1 sigma 1 pi
Triple- 1 sigma 2 pi

10th grade (71 decks)

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