Chem Final Sem 1 Flashcards by Ivana Darmawan

Creation Mandate: What is it where do you find it

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

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

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When was chemistry first taught as an academic discipline

1800

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Biblical worldview

How someone sees and interprets life using Bible as guide

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Quantitative data

Data with numbers, measurable

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Qualitative data

Data without numbers, not measurable

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Scientific method

Observation
Question
Hypothesis
Experiment
Data collection
Conclusion
Retest

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DIfference between theory and hypothesis

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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Observation

What do you see happening

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Data

Info/fact/stats collected for analysis

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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

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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Ex nihilo

Out of nothing

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Density formula

Mass over volume

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Physical property

We can measure without changing material into another substance

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Chemical property

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

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Conductivity

Ability of material to transfer heat or electricity between its particles

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Ductility

Describes how easily materials can be drawn into thin wires

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Malleability

How easily material can be hammered into shapes

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Luster

based on whether the mineral is metallic or non-metallic

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Physical change
Example: Spoiled milk or cut up paper

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

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Chemical change
Example: Spoiled milk or cut up paper

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

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Mixtures: Heterogenous/homogenous/suspensions what are they

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

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Diatomic element & Monatomic element & Polyatomic

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

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Polyatomic ion

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

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5Fe₂ What is the 5

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

5Fe₂ What is 2

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

(Fe₂)₂

2 Fe₂

What is an ion

Positive or negative charged atom

Entropy

Measure of disorder in system

If you burn gasoline will entropy increase or decrease

Increase becausethe energy becomes less usable

Kelvin What is 0 degrees Kelvin known as

Basic metric unit of temp Absolute 0

How do you change from Celcius to Kelvin

+273.15 kelvins

Temp 12000k what is that in celsius

12000 - 273.15 926.85

Changes of common states of matter

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

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

1000g 1000 milligrams

How many kg in 25,600g

25.6 kg

Percent error formula

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

Accuracy and precision

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

Law of definite composition

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

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

Subatomic particles Electron

A number and Z number of atom What A and Z

A: Atomic number Z: Protons

Niels Bohr what did he propose

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

Heisenberg Uncertainty Priciple

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

Pauli exclusion principle

No 2 electrons in an atom can have same address

Afbau principle

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

Hund's rule

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

4 parts of electrons address

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)

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

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

Electron configuration Ex: Carbon 6

How electrons are arranged1s2 2s2 2p2

Electron configuration for nitrogen (7 electrons)

1s2 2s2 2p3

What does [He] mean in electron configuration

Helium 1s2

Isotopes

Elements with different numbers of neutrons

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

Protons Neutrons

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

42 protons 56 neutrons

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

Positive

If Carbon gains 1 electron what charge will it have

Negaitive

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

Ion

Wavelength

Distance between 2 peaks or troughs in a wave

Frequency

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

What is relationship between frequency and wavelength

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

What are units of frequency and wavelength

Hertz

What is h in c= hv

Wavelength

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

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

What did Newlands discover

Law of octaves

Connection with atomic mass and chemical properties

What did Mendeleev do for creating periodic table

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

Lustrous

metallic

Alkali metals How many electrons do they lose or gain

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

Alkali earth metals How many electrons do they lose or gain

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

Halogens

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

Noble gases

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

Metalloids

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

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

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

Ionization energy

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

Atomic radius

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

Ion size

Cation-bigger Anion- smaller

Electron affinity

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

Electronegativity

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

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

Lose energy Gain stability Valence electron

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

Noble gases

Polarity of a bond btwn 2 atoms depend on what

Electronegativity

What does deltaEN mean

Electronegativity

What kind of bond would exist between Na and F

Ionic

What is electrostatic force

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

What does the single dash btwn 2 atoms mean

2 electrons shared

What does double dash btwn 2 atoms mean

2 pairs of 2 electrons shared

What does triple dash btwn 2 atoms mean

3 pairs of 2 electrons shared

Electron sea theory

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

Which does electron sea theory explain regarding metals

Luster, conductivity, ductility

Ionic compounds

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

Ionic compounds are they good at electrical conductivity

Yes

Are ionic compounds easily broken as crystals

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

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

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

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

Which bond type is stronger sigma or pi

Sigma

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

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

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

Triple

Resonance

No single Lewis structure can totally describe how electrons are distributed

What makes a good graph

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

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

To protect your eyes

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

To protect from chemicals

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

So hair doesn't catch on fire

Why use tongs when working with glass beaker

To safely grab very hot items

What is purpose of wire gauze

Place between beaker or dish and lab burner

Inductive vs Deductive reasoning

Inductive- Begins with observation Deductive- Begins with theory

Bonds sigma and pi

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