Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Science 10 AP: Chemistry > History, Atoms, Elements, Ions > Flashcards

History, Atoms, Elements, Ions Flashcards

1
Q

What is matter?

A

Anything that has mass and occupies space. It is also a form of energy. Can be a solid, liquid, or gas.

Mass is the quantity of matter present in a body. There are several ways to classify matter.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is matter split into?

A
  • Mixtures (combinations of matter that can be separated by physical means). No fixed composition.
  • Pure Substance (matter that has a definite composition, as they always look consistent throughout).
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are mixtures split into?

A
  • Heterogenous Mixtures (different components are visible within the mixture)
  • Homogenous Mixtures (different components are not visible)

(FYI: technically homogenous then into suspensions and colloids.)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are pure substances split into?

A
  • Compounds (two or more elements chemically bonded together and can be chemically separated)
  • Elements (cannot be broken down into simpler substances by chemical means—they are on the Periodic Table)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

(Just in case) What are the two earliest atomic models?

A

(Both around 400 BC)
- Aristotle/Plato: 4 element model
- Democritus: “indivisible” atomos

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What was the first “modern atomic theory” (1803)?

A

John Dalton’s Theory (founder of modern chemistry):
- indivisible atoms
- no knowledge of subatomic atoms (atoms are neutral)
- analogous to billard balls that bounce off of each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What was the second atomic theory (1897+)?

A

J.J. Thomson’s Theory:
- positive sphere with embedded elections (atoms are overall neutral)
- atoms are divisible and smaller had to exist
- discovered elections; elections contain charged particles
- you can pull electrons out; but does not know about protons
- analogous to plum pudding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What was the third atomic theory (1914)?

A

Ernest Rutherford’s Theory:
- small positive (dense) nucleus surrounded by electrons
- mostly open space
- Gold Foil Experiment
- could not explain why the electrons do not spiral into the nucleus
- analogous to a beehive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What was the last atomic theory (1921)?

A

Niels Bohr’s Theory:
- magic number of (periods, energy packets, rings) elections in quantized/discrete (smallest amount of something) energy levels
(TLDR) elections are found in specific energy levels/orbitals
- analogous to planets orbiting around the Sun

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

(Just in case) What are the three important theories we missed?

A
  • 1904: H. Nagaoka (A positive sphere with a ring of electrons)
  • 1926: Erwin Schrodinger (Quantum Mechanics Theory)
  • 1935: Sir James Chadwick (Neutron)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are the five main points of Dalton’s Atomic Theory? Which are actually 100% correct?

A
  1. All matter is made up of small particles called atoms (correct)
  2. Atoms can’t be created or destroyed or divided into smaller particles (subatomic particles exist)
  3. All atoms of the same element are identical in mass and size but differ in mass and size from the atoms of other elements (some are more similar, some are not).
  4. Compounds are formed when atoms of different elements combine in fixed proportions. The smallest particles of any compound always contain the same type and relative numbers of atoms (correct)
  5. Chemical reactions change the way atoms are grouped but the atoms themselves are not changed (correct, nuclear change the atoms)

A, C, D, C, R

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are subatomic particles?

A

Particles that make up the atom: protons, neutrons, electrions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are protons?

A

Positively charged particles. Bigger than electrons. By a lot. Found in the nucleus.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are neutrons?

A

Particles with no electric charge. Same mass as protons. Found in the nucleus.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are electrons?

A

Negatively charged particles. Located in the outer region of the atoms. Move in the shells.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the nucleus?

A

The small, positively charged central region of the atom.
- Most mass of an atom is here
- Contains protons and neutrons
- Same number of protons/electrons but different number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is an energy level?

A

A specific allowed energy for electrons
- Thought of as a space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What are quarks?

A

Smaller particles make up neutrons and protons. Not electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is the nucleon?

A

Protons and neutrons.
- The generic term for particles inside the nucleus.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is the atomic number?

A

The number of protons in the nucleus. It identifies the element.
- Found on Periodic Tables
- Since all atoms are neutral, the number of protons is equal to the number of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is the atomic mass?

A

The total number of protons and neutrons in an atom. It is the total mass of an element.
- Found on Periodic Tables

  • Atomic mass = # of protons + # of all neutrons (rounded atomic mass)
  • # of neutrons = Atomic mass - # of protons (r.a.m.)
22
Q

What are atomic isotopes?

A

Atoms of the same element that differ in mass. They have the same number of protons, but different numbers of neutrons.

Notation:
M (mass #, p+ + n0, do not refer to Periodic Tables)
X (symbol)
A (atomic #, p+ #)

Naming: (element) (dash) (mass number)

Example: Carbon-14
14
C
6

23
Q

(Just in case) What is hydrogen-2 and hydrogen-3 called?

A

Deuterium and Tritium

24
Q

Who organized the Periodic Table?

A

Dmitri Mendeleev

25
Q

What are periods on the Periodic Table?

A
  • Horizontal rows
  • Elements arranged from lowest to highest atomic #
  • Tells you the number of occupied energy levels.
26
Q

What are groups on the Periodic Table?

A
  • Vertical columns
  • Elements arranged into families based on properties
  • Valence electron (number of) placement
27
Q

What are the Alkali metals?

A
  • Group 1 elements, excluding Hydrogen
  • Very reactive to water
  • Shiny, solids, and silvery looking
  • Very soft
  • Soft, malleable, ductile
28
Q

What are the Alkaline-earth metals?

A
  • Group 2 elements
  • React with the Halogens, including Oxygen
  • Shiny solids (not as soft)
  • Malleable, ductile
29
Q

What are the Halogens?

A
  • Group 17 elements
  • React with the (Alkaline-earth) metals to form salts
  • Vary greatly in appearance and state
30
Q

What are the Noble gases?

A
  • Group 18 elements
  • Inert and non-reactive
  • Full outer shell
  • Colorless gases of varying weights
31
Q

What is the “staircase” on the Periodic Table?

A

A line that separates the metals on the left from the non-metals on the right. The metalloids are on it.

32
Q

What is the state, appearance, conductivity, malleability, and ductility of metals?

A
  • Solid (except Hg)
  • Shiny
  • Good heat and electric conductor
  • Yes, both
33
Q

What is the state, appearance, conductivity, malleability, and ductility of non-metals?

A
  • Varying
  • Dull
  • Poor conductors of heat/electricity: insulators
  • Brittle (not malleable), nor ductile
34
Q

What is the state, appearance, conductivity, malleability, and ductility of metalloids?

A
  • All solids
  • Some dull, some shiny
  • Some conduct electricity, but most do not conduct heat
  • Brittle (not malleable), nor ductile

These contain properties of both metals and non-metals.

35
Q

Define malleability.

A

Bendable; able to be worked into a shape. Hammered into sheets.

36
Q

Define ductility.

A

Can be stretched into wires.

37
Q

Electron placement: electrons orbit in fixed energy levels. The maximum number of electrons held by each of the following energy levels is…
First e-: __
Second e-: __
Third e-: __

A

2
8
8

38
Q

What is a stable octet?

A

(in the valence energy level) An arrangement of 8 electrons in the outermost occupied energy level. Like the noble gases.

39
Q

What does the period number tell us?

A

Tells you the number of occupied energy levels.

40
Q

What is the valence energy level?

A

The outermost occupied energy levels (actually will do stuff).
- The electrons in the valence energy level are called valence electrons.
- Elements in the same group on the Periodic Table have atoms with the same number of valence electrons

41
Q

What does the group number tell us?

A

The number of valence electrons in an atom.

42
Q

How to figure out the number of valence electrons?

A

Group number. For 13-18, just look at the second number.

43
Q

What are energy levels?

A

A region of space near the nucleus that may contain electrons.

44
Q

How do you make energy level diagrams?

A
  • write the appropriate symbol
  • make a circle (nucleus) above the symbol
  • indicate the correct number of p+ and n0 in the circle
  • indicate the correct number of electrons one each energy level, starting at the level closest to the nucleus
  • works up to Calcium
  • used since the Bohr model is kinda hard to read
45
Q

How does the amount of energy in electrons differ as you move away from the nucleus?

A

Near the nucleus: lowest energy, strongest attraction to the nucleus

As you move farther away there will be more energy

46
Q

What are electron dot diagrams? How do you make them?

A

They represent the valence electrons of an atom.

The symbol of the element in the center, the valence electrons are represented as dots.

Electrons want to spread out as far away from each other as possible. Dots are placed in a clockwise fashion.

Elements of the same group will have the same dot diagram!

Helium’s two have to be paired since its valence is 2.

47
Q

What are lone pairs?

A

Stable!

48
Q

What are ions?

A

A neutral atom has the same number of protons as electrons.
It is possible for an atom to gain or lose electrons and become charged: IONS.

The gaining/losing of electrons: ionization

49
Q

What are positively charged ions?

A
  • They have fewer electrons than protons. They lose electrons.
  • Metals tend to form these CATIONS
  • Naming: element name + “ion”
  • Lithium ion
  • Na+
50
Q

What are negatively charged ions?

A
  • They have more electrons than protons. They gain electrons.
  • Non-metals tend to form these ANIONS
  • Naming: element name (replaced with “-ide) + “ion”
  • Oxide ion
  • S2-
51
Q

Why are ions formed?

A
  • to obtain a full valence energy level (full outer shell), to become stable, like the noble gases
  • having a full shell (stable but charged) is better than being unbalanced but neutral

Science 10 AP: Chemistry (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions