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A. 1. What's the matter? > Notes > Flashcards

Notes Flashcards

1
Q

What is matter?

A

EVERYTHING around us in all its states. it has to have at least some tiny mas and take up at least some space.

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2
Q

What is matter made up of?

A

Atoms and molecules

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3
Q

What are sub atomic particles (made up of)?

A

Protons, electrons, neutrons

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4
Q

The unit of stuff has to be able to do what while having the same composition and unit?

A

Change state

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5
Q

What are atoms?

A

The building blocks to make up all the stuff we see

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6
Q

What are elements?

A

How we find atoms in their pure form in nature

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7
Q

What is a molecule?

A

Two of the same type of atom bonded toghether(O2)

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8
Q

What is a compound?

A

Two or more different elements bonded together. An energy provider molecule.

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9
Q

Difference between an element and an atom.

A

An atom is only one single unit.

An element can be more 1 or more of the pure atom together/bonded.

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10
Q

What does the RUTHERFORD model allow?

A

To see how elements orbit around an atom in 3D.

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11
Q

What does the BOHR model allow us to see?

A

The orbital shells/energy level in 2D

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12
Q

Describe the Bohr-Rutherford

A

Shows nucleus with protons/orbitals only and electrons per shell. May or may not show neutrons. Fills electron shells using 2, 8, 8, 2.

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13
Q

Describe the Simplified Atomic Model (SAM)

A

Shows protons and neutrons in nucleus and electrons per energy level. Fills electron shells using 2, 8, 8, 2.

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14
Q

Name the negatively charged, positively charged, and neutral parts of an atom.

A

Electrons
Protons
Neutrons

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15
Q

Describe protons

A

Positively charged and located at the center of the atom (nucleus)

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16
Q

Describe neutrons

A

Neutrons are neutral and located at the center of the atom (nucleus)

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17
Q

Electrons

A

The tiniest particle, negatively charged and located very far away from the nucleus of the atom

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18
Q

Most of the atom is actually what?

A

Empty space

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19
Q

Where does most of the mass of an atom come from?

A

The nucleus (protons and neutrons)

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20
Q

Which sub atomic particles contribute to mass of an atom?

A

Protons and neutrons

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21
Q

What is the atomic number?

A

Number of protons

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22
Q

What is the atomic mass?

A

Average mass of the atoms in an element (protons + neutrons)

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23
Q

The bigger number of an element on a periodic table is what?

A

The atomic mass

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24
Q

What does each letter in A, Z, E notation indicate?

A 
A= Atomic mass
Z= Atomic number
E= Chemical symbol for the element
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25
Q

Study AZE

A

idk, do it

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26
Q

Which sub atomic particles determine the element?

A

Protons

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27
Q

Which sub atomic particles determine the atomic number?

A

Protons

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28
Q

Which sub atomic particles determine the atomic mass?

A

Protons and neutrons

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29
Q

Which sub atomic particles must be equal to have a stable atom (not an isotope)

A

Protons and neutrons

30
Q

What makes an atom of neutral charge?

A

Equal number of electrons and protons

31
Q

What determines if an element is a +ion?

A

More protons than electrons

32
Q

What determines if an element is a -ion?

A

More electrons than protons

33
Q

What is an ion? How does it happen?

A

A positively or negatively charged particle

Either having more or less protons than electrons.

34
Q

Describe a +ion

A

More protons than electrons

35
Q

Describe a -ion

A

More electrons than protons

36
Q

STUDY “Determine The Rules & Patterns of the Periodic Table To identify Each Element”

A

idk

37
Q

What is an isotope?

A

An atom of the same element (same number of protons) but a varying number of neutrons

protons stay the same, neutrons change

38
Q

Its radioactive if what?

A

The number of protons are not equal to the number of neutrons

39
Q

What is relative atomic mass?

A

An average based on the relative abundance (the abundance of each isotope of an element varies and can be described as a % to calculate the relative atomic mass). This is why you see decimals on the periodic table.

40
Q

Name a radioactive isotope and its uses.

A

C14
Carbon dating as C14 being unstable over time. See how much is left and can guess age of fossil if its not too old, otherwise no C14 left.
As a cancer treatment as certain radioactive substances can be targeted and will kill cells (both cancerous and not)

41
Q

What are valence electrons used to describe?

A

Atoms of the same group that share the same number of electrons on their outermost electron shell

42
Q

What do valence electrons determine?

A

How an atom will chemically interact

43
Q

When is an atom considered unreactive?

A

When the outermost electron shell is full for that level (2, 8, 8, 2)

44
Q

Which group is not chemically reactive?

A

Noble gasses

45
Q

Which are the most and second most reactive groups?

A

Alkali metals

Halogens

46
Q

What is the second group named?

A

Alkali Earth Metals

47
Q

Which element is not technically part of its group? Why?

A

H (Hydrogen)
It is a gas in a group of metals
(but it still needs one more electron for perfection so its there anyways)

48
Q

What is the name for the lines on the periodic tables that are horizontal?

A

PERIODS or rows

49
Q

What is the name for the lines on the periodic tables that are vertical?

A

GROUPS or columns

50
Q

What do the elements in a period have in common?

A

The same number of orbital shells

51
Q

What do the elements in a group have in common?

A

The number of valence electrons

52
Q

PRACTICE DRAWING B-R, AZE, SAM, LEWIS

A

art.

53
Q

Describe Alkali Metals

A

Column 1, 1 valence electron, includes H, very reactive (psycho)

54
Q

Describe Alkali Earth Metals

A

Column 2, 2 valence electrons, reactive

55
Q

Describe Halogens

A

Column 7, 7 valence electrons, very reactive (psycho)

56
Q

Describe Noble Gases

A

Column, 8, 8 valence electrons, includes He(2 ve-), “perfect”/STABLE

57
Q

Where are the metals on the periodic table?

A

To the left of the staircase

58
Q

Describe metals

A 
To the left of the sc.
Malleable
Conduct electricity
Conduct heat
Often shiny
Many react chemically with acids to produce a gas
59
Q

Where are non metals on the periodic table?

A

To the right of the staircase except for H.

Many are red at rm temp

60
Q

Describe non metals.

A

Opposite of metals

61
Q

Where are metalloids on the periodic table?

A

Along the staircase

62
Q

Describe metalloids

A

At least one characteristic from non metals and metals

63
Q

What does the Lewis structure show?

A

The element symbol and valence electrons (shown as dots around the symbol)

64
Q

When is the Lewis structure useful?

A

When we want to see which element would like to group or family would have their outermost electron shell filled if they bonded

65
Q

What is atomic radius?

A

Size of the atom

66
Q

Across a period/from left to right. how does atomic radius change? Why?

A

It decreases

When atomic number increases there is more electrostatic charges (more protons and electrons so there is more pull shrinking the overall size of the atom)

67
Q

What is the periodicity of electronegativity?

A

A measure of the ability of an atom to attract electrons to itself when forming a chemical bond

68
Q

How does the periodicity of electronegativity change from left to right?

A

It increases

69
Q

What makes an atom very reactive

A

When it is very close to having a full outer shell

70
Q

Is it easier to give away a ve or get one?

A

Give away

71
Q

from the middle to the right, and from the middle to the left what happens to the periodicity of chemical reactivity?

A

It increases

72
Q

What is the periodicity of chemical reactivity?

A

How reactive an element is

A. 1. What's the matter? (1 decks)

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