Chemistry Midterm Review

studied byStudied by 4 people
5.0(3)
Get a hint
Hint

How and where did the natural elements form?

1 / 139

flashcard set

Earn XP

Description and Tags

140 Terms

1

How and where did the natural elements form?

They formed in stars. Smaller stars formed smaller elements. Larger stars formed larger elements. Supernovas and massive stars form elements heavier than iron.

New cards
2

What elements are produced by more massive stars?

Elements heavier than iron,.

New cards
3

How did larger elements (beyond iron) form?

Through supernovas

New cards
4

What is the relationship between the life cycle of a star and its mass?

The path the star follows depends on its mass. The larger the mass, the shorter the life cycle.

New cards
5

What element is the building block for all other natural elements?

Hydrogen

New cards
6

What is the difference between chemical and physical changes?

Physical changes affect physical properties w/ no new change in chemical composition. Chemical changes is when entirely new substances form with different properties.

New cards
7

What are physical properties?

Physical properties are characteristics observed without changing the identity of the substance. Ex. color, density, melting points.

New cards
8

What are chemical properties?

A characteristic of a substance observed through a chemical reaction. Ex. flammability, heat of combustion, acidity.

New cards
9

What is the difference between reactants and products in chemical reactions?

A reactant is is the original substance in a chemical reaction. A product is a new substance created through a chemical reaction.

New cards
10

What are the particles like in solids?

The particles vibrate and are tightly packed.

New cards
11

What are the particles like in liquids?

The particles are lightly held together and can slip past each other.

New cards
12

What are the particles like in gases?

The particles are slightly held together and can move independently at higher speeds.

New cards
13

What is the difference between pure substances and mixtures?

Pure substances have definitive characteristics and are elements and compounds. Mixtures have properties that reflect those in pure substances. The composition can vary by proportion.

New cards
14

What are some methods for separating mixtures?

Filtration, magnetism, evaporation, by hand, dissolving, condensation

New cards
15

Which state of matter has the highest kinetic energy and why?

Gas; the particles are slightly held together, so it can move independently at higher speeds

New cards
16

Why does a given quantity of water heated at a constant rate take longer to change from liquid to gas than from solid to liquid?

A greater amount of potential energy is stored in the particles of a gas.

New cards
17

What are 4 naturally occurring diatomic elements?

Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Chlorine, Bromine (Have No Fear Of Ice Cold Beer)

New cards
18

What are three forms of energy?

Kinetic energy, Potential energy, Heat energy

New cards
19

What is the boiling point of water on the Kelvin scale?

373 Kelvin

New cards
20

What is the boiling point of water on the Celsius scale?

100 degrees Celsius

New cards
21

What subatomic particles are found in an atom’s nucleus?

Protons and Neutrons

New cards
22

Where are electrons found in an atom?

In electron clouds and orbitals

New cards
23

What is bright line spectra?

Bright line spectra is the light emitted when electrons move between energy levels.

New cards
24

How can an element’s bright line spectra be used identify elements in unknown materials?

Each element has a unique line spectra.

New cards
25

Which has a longer wavelength, orange or violet light?

Orange Light

New cards
26

Which has a higher energy, x-rays or gamma rays?

Gamma Rays

New cards
27

Which has a lower energy, infrared light or x-rays?

Infrared Light

New cards
28

Do atoms release energy when electrons jump to higher energy levels?

No

New cards
29

What is an electron cloud?

The space around the nucleus where electrons are located.

New cards
30

What letter represents the principal quantum number?

n

New cards
31

All electromagnetic radiation can be thought of as moving ….

waves

New cards
32

As the frequency of a wave increases, the wavelength…

decreases

New cards
33

Why can protons exist so close together within the nucleus of the atom?

The strong force holds together the subatomic particles of the nucleus.

New cards
34

What determines the type of bond an atom can form?

The valence electrons

New cards
35

Why can properties of elements in the same group be predicted?

They have the same number of valence electrons so they act similarly.

New cards
36

Why did Mendeleev have gaps in his table?

Predicted the properties of undiscovered elements when he grouped the elements by similar properties and increasing atomic mass.

New cards
37

How did Mendeleev use the gaps in the periodic table?

He used it predict undiscovered elements.

New cards
38

What is the importance of valence electrons?

They are the only electrons that partake in chemical reaction.

New cards
39

How is the electron configuration similar for each element in a group?

They have the same number of valence electrons and the same ending sublevel.

New cards
40

Where are metals located on the periodic table?

Located to the left of the red staircase.

New cards
41

Where are metalloids located on the periodic table?

Metalloids are bordering the red staircase.

New cards
42

Where are nonmetals located on the periodic table?

Located to the right of the red staircase.

New cards
43

Where are noble gases located on the periodic table?

Group 18

New cards
44

Where are the halogens located on the periodic table?

Group 17

New cards
45

Where are the alkali metals located on the periodic table?

Group 1

New cards
46

Where are the alkaline earth metals located on the periodic table?

Group 2

New cards
47

Identify a group of inert elements.

Noble Gases

New cards
48

Which sublevel do transition elements fill?

The d sublevel

New cards
49

What trend in atomic radius do you see as you go down a group?

It increases due to electrons occupying additional energyy levels.

New cards
50

What trend in atomic radius do you see as you go across a period?

It decreases across a period because additional protons pull the electrons closer.

New cards
51

Ionization Energy

Energy needed to remove an electron from a neutral atom or an ion.

New cards
52

What trend in ionization energy do you see as you go down a group?

It decreases due to occupied energy levels and electron shielding.

New cards
53

What trend in ionization energy do you see as you go across a period?

Increases across a period because of additional protons pull the electrons closer.

New cards
54

Electronegativity

An atom’s attraction for electrons when bonded to another atom.

New cards
55

What trend in electronegativity do you see as you go down a group?

Decreases down groups due to additional energy levels and electron shielding.

New cards
56

What trend in electronegativity do you see as you go across a period?

Increases across a period due to additional protons.

New cards
57

What is the most reactive metal?

Francium

New cards
58

What is the most reactive nonmetal?

Fluorine

New cards
59

How do you express specific heat?

joules per gram Kelvin (J/gK)

New cards
60

What is the SI unit for energy?

joules (J)

New cards
61

What is the equation for specific heat capacity?

Cp=q/mT ( q=energy, m=mass, T=change in temp)

New cards
62

What units do you use for heat of fusion?

J/g

New cards
63

How do you calculate percent error?

( I Your Answer - Accepted Value I / Accepted Value ) times 100

New cards
64

Dalton's Atomic Theory

  1. Matter composed of indivisible particles called atoms.

  2. Each element's atoms are alike.

  3. Atoms of different elements have different masses.

  4. Atoms of different elements combine in whole numbers to form compounds.

  5. In chemical reactions, atoms are rearranged, not created nor destroyed.

New cards
65

Which principles of Dalton's Atomic Theory are no longer true?

  1. Matter composed of indivisible particles called atoms.

  2. Each element's atoms are alike.

New cards
66

JJ Thomson

Experimented with cathode ray tube; Discovered electrons

New cards
67

Strong Force

Holds the protons and neutrons together in the nucleus of an atom. The closely packs neutrons and protons creates the strong force which is stronger than the repulsive force.

New cards
68

What unit is atomic mass measured in?

amu (atomic mass units); 1 amu is 1/12th the mass of one carbon atom

New cards
69

How do you find the atomic mass?

Add the number of protons and neutrons.

New cards
70

Isotope

Atoms of the same element with different number of neutrons.

New cards
71

Equation for Mass Number

Mass Number = protons + neutrons

New cards
72

Alpha Particle

A small, positively charge particle, which Rutherford directed at thin, gold foil

New cards
73

Anode

The electrode attached to the positive terminal of a voltage source

New cards
74

Cathode

The electrode attached to the negative terminal of a voltage source

New cards
75

Anion

Negatively charged atom with more electrons than protons

New cards
76

Ernest Rutherford

Experimented with gold foil; Discovered atom is mostly empty space and the nucleus contains most of the atom's mass

New cards
77

Which 2 subatomic particles have significant masses?

Protons & Neutrons

New cards
78

Cations

Positively charged particles that have lost electrons.

New cards
79

How can you calculate the charge of an atom?

Protons - Electrons = Charge

New cards
80

Equation for Average Atomic Mass

Average Atomic Mass = (mass of isotope 1 x abundance) + ( mass of isotope 2 x abundance)

New cards
81

Photon

When an electron releases energy in the form of light.

New cards
82

What is the speed of light?

2.988 x 10^8 m/s or 3.00 x 10^8 m/s

New cards
83

In the equation c = λ x v, what does c represent?

Speed of Light

New cards
84

In the equation c = λ x v, what does λ represent?

Wavelength

New cards
85

In the equation c = λ x v, what does v represent?

Frequency

New cards
86

In the equation E = h x v, what does h represent?

Planck's Constant

New cards
87

In the equation E = h x v, what does e represent?

Energy

New cards
88

In the equation c = λ x v, are λ and v inversely or directly proportional?

Inversely

New cards
89

Do all wavelengths on the electromagnetic spectrum travel at the same speed?

Yes

New cards
90

What does quantum # n describe about an electron?

The electrons distance from the nucleus aka what energy level it's in.

New cards
91

What are the four sublevels in order of energy?

s,p,d,f

New cards
92

How many orbitals does sublevel s have?

1 orbital

New cards
93

How many orbitals does sublevel p have?

3 orbitals

New cards
94

How many orbitals does sublevel d have?

5 orbitals

New cards
95

How many orbitals does sublevel f have?

7 orbitals

New cards
96

How many electrons can each orbital hold?

2 electrons

New cards
97

Pauli Exclusion Principle

Within each orbital, electrons spin in opposite directions. Two electrons in one orbital can't be spinning the same way.

New cards
98

Aufbau Principle

Electrons fill the lowest energy levels first.

New cards
99

Hund's Rule

P orbital fill with one electron at a time; no pairing until each p orbital has one electron.

New cards
100

Electromagnetic Spectrum

All of the frequencies or wavelengths of electromagnetic radiation.

New cards

Explore top notes

note Note
studied byStudied by 10 people
Updated ... ago
5.0 Stars(1)
note Note
studied byStudied by 22 people
Updated ... ago
4.0 Stars(1)
note Note
studied byStudied by 31 people
Updated ... ago
5.0 Stars(1)
note Note
studied byStudied by 9 people
Updated ... ago
5.0 Stars(1)
note Note
studied byStudied by 16 people
Updated ... ago
4.0 Stars(1)
note Note
studied byStudied by 4 people
Updated ... ago
5.0 Stars(1)
note Note
studied byStudied by 10 people
Updated ... ago
5.0 Stars(1)
note Note
studied byStudied by 36 people
Updated ... ago
5.0 Stars(1)

Explore top flashcards

flashcards Flashcard24 terms
studied byStudied by 77 people
Updated ... ago
5.0 Stars(1)
flashcards Flashcard34 terms
studied byStudied by 5 people
Updated ... ago
4.0 Stars(1)
flashcards Flashcard101 terms
studied byStudied by 4 people
Updated ... ago
5.0 Stars(1)
flashcards Flashcard37 terms
studied byStudied by 1 person
Updated ... ago
5.0 Stars(1)
flashcards Flashcard41 terms
studied byStudied by 2 people
Updated ... ago
5.0 Stars(1)
flashcards Flashcard45 terms
studied byStudied by 2 people
Updated ... ago
5.0 Stars(1)
flashcards Flashcard36 terms
studied byStudied by 1 person
Updated ... ago
5.0 Stars(1)
flashcards Flashcard50 terms
studied byStudied by 13 people
Updated ... ago
5.0 Stars(1)