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FLASHCARDS > Science Summative Assessment 1 Reviewer > Flashcards

Science Summative Assessment 1 Reviewer Flashcards

1
Q

Who first discovered the atom?

A

Democritus

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2
Q

What are the 5 atomic models?

A

Atomic Model, Plum-Pudding Model, Nuclear Model, Planetary Model, Quantum Mechanical Model

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3
Q

Which model has these theories?

Atoms are small, indivisible. Atoms can’t be divided, created, destroyed. An element = identical. Different elements create different properties. Atoms of different elements can be combined to form compounds.

A

Atomic Model

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4
Q

Who created the Atomic Model?

A

John Dalton

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5
Q

Which model has these theories?

Atoms consists of a positive and negative charge. An atom is electrically neutral (positive = negative). Negatively charged electrons are fixed in the positive sphere.

A

Plum-Pudding Model

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6
Q

Who created the Plum-Pudding Model?

A

Joseph John Thomson (J.J Thomson)

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7
Q

Which model has these theories?

Atoms are mainly empty space. Positive charge is concentrated at the center of an atom. The center of an atom is called the nucleus. Electrons move around the nucleus.

A

Nuclear Model

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8
Q

Who created the Nuclear Model?

A

Ernest Rutherford

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9
Q

Who created the Planetary Model?

A

Niels Bohr

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10
Q

Which model has these theories?

Electrons move around the nucleus in ‘a cloud’ not orbits. Orbitals help us predict the area where we can find electrons. The closer position to the nucleus the higher chance to find electrons.

A

Quantum Mechanical Model (QMM)

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10
Q

Which model has these theories?

electrons orbit the nucleus. Orbits have a specific size and energy. The energy is related to the size of the orbit. Lowest energy is found in the smallest orbit. Electrons can move between each shell when gaining or losing energy.

A

Planetary Model

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11
Q

Who created the Quantum Mechanical Model?

A

Erwin Schrodinger

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11
Q

Electrons travel in fixed circular paths known as __. (Bohr’s Atomic Model)

A

Orbits

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12
Q

Substances emit their characteristic __. (Bohr’s Atomic Model)

A

Colors

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13
Q

The Bohr Atomic Model introduced the p________ e_____ l____,

A

principal energy level

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14
Q

What happens in Atomic Excitation and Atomic De-excitation?

A

In atomic excitation, the electron moves outward in orbits. In atomic de-excitation, the electron moves inward in orbits.

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14
Q

What theory proposes that all matter, including electrons can also exist as a wave. (theorized by Louie De Broglie)

A

wave-particle duality of matter

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14
Q

What are the basic parts of an atomic model?

A

Nucleus, Electrons, Orbits, Energy Levels

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15
Q

What theory states that it is impossible to know the exact position and momentum of an electron at the same time? (theorized by Werner Karl Heisenberg)

A

Uncertainty Principle (became the basis of quantum mechanics)

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15
Q

What ideas helped develop the quantum mechanical model (Schrodinger’s Model)

A

De Brogile’s ideas (wave-particle duality of matter) and Heisenberg’s ideas (Uncertainty Principle)

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15
Q

What are all the orbital types?

A

s orbital, p orbital, d orbital, f orbital

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15
Q

Electrons were thought to orbit around the nucleus in fixed paths. But was later discovered to move in a _____.

A

cloud

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16
Q

Method of arranging electrons by using orbital diagrams

A

Electron Population

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16
Q

Electrons are represented with ______. (Electron Population)

A

arrows

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17
Q

How many electrons can each box accommodate? (Electron Population)

A

two

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17
Q

How many boxes does the d orbital have? How many electrons can the d orbital have? (Electron Population)

A

It has 5 boxes and can accommodate 10 electrons.

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18
Q

How many boxes does the s orbital have? How many electrons can the s orbital have? (Electron Population)

A

It has 1 box and can accommodate 2 electrons.

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18
Q

How many boxes does the p orbital have? How many electrons can the p orbital have? (Electron Population)

A

It has 3 boxes and can accommodate 6 electrons.

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18
Q

States that electrons are distributed in increasing energy of orbitals.

A

Aufbau Principle

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19
Q

What are the ℓ values for each subshell?

A

s = 0, p = 1, d = 2, f= 3

19
Q

How many boxes does the f orbital have? How many electrons can the f orbital have? (Electron Population)

A

It has 7 boxes and can accommodate 14 electrons.

20
Q

What is Hund’s Rule?

A

When filling up electrons in degenerate orbitals, each orbital (1s, 2s, 2p, 3s, 3p, …) is filled with a single electron of the same spin before pairing it with the opposite spin.

20
Q

What is Pauli’s Exclusion Principle?

A

Each orbital can only contain a maximum of two electrons with opposite spins (up arrow or down arrow). No orbital diagram must be drawn with the same spin. ⬆️⬇️✅,⬇️⬇️❌,⬆️⬆️❌

20
Q

The principle energy level is based on the ___ that the element is in.

A

row (in periodic table)

21
Q

Longhand electron configuration steps

A

Determine number of electrons. for neutral atoms the number of electrons is equivalent to the atomic number (Z)

Distribute electrons from lowest energy level following the Aufbau Principle.

22
Q

Give me the chronological order of the Aufbau Principle subshells.

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s

23
Q

What is the longhand electron configuration of In?

A

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10, 5p1

24
Q

When starting to count in the d block subtract _ from the row it is in.

A

1

25
Q

When starting to count in the f block subtract _ from the row it is in.

A

2

26
Q

What are the row numbers of the f block?

A

4f and 5f

27
Q

Steps in doing shorthand electron configuration

A

Find the element. Find noble gas before that element (all noble gases are in column 18 on periodic table). Identify element location/the last subshell and electron of longhand electron configuration (Ex. I = 5p5). Add the noble gas and element location together. It should look something like this (for I): [Kr]5p5.

28
Q

Steps in dong electron configuration of ions or transition metals

A

An element, lets say, O when neutral has 8 electrons. When adding a negative charge O-, it will gain 1 electron making it 9 electrons, if positive charge O+, it will lose 1 electron making it 7 electrons.

For transition metals like Fe, we remove electrons from s orbitals first. Neutral Fe = 1s2 2s2 2p6 3s6 4s2 3d6. Fe2+ = 1s 2s2 2p6 3s2 3p6 4s0 3d6. Fe3+ = 1s 2s2 2p6 3s2 3p6 4s0 3d5.

29
Q

What are the 4 quantum numbers?

A

Principal, Azimuthal, Magnetic, Spin

30
Q

What is the symbol for Principal?

A

it is “n”

31
Q

What is the symbol for Angular Momentum/Azimuthal?

A

it is “ℓ”

32
Q

What is the symbol for Magnetic?

A

it is “mℓ”

33
Q

What is the symbol for Spin?

A

it is “ms”

34
Q

How do you find Angular momentum ℓ? (quantum numbers)

A

s=0, p=1, d=2, f=3

35
Q

How do you find Principal n? (quantum numbers)

A

The row the element is in is n. Subtract 1 if its in d block and subtract 2 if its in f block.

36
Q

How do you find Magnetic mℓ? (quantum numbers)

A

find element location (Ex. Sulfur = 3p4).
s: mℓ = 0
p: mℓ = -1, 0, or 1.
d: mℓ = -2, -1, 0 , 1, or 2
f: mℓ = -3, -2, -1, 0, 1, 2, or 3

The value beside orbital in element location determines what mℓ will be. For example, Sulfur is in p. There are 3 possible values for p orbital (1, 0, or 1), those are all boxes. The value beside the orbital in sulfur is 4. So draw 4 arrows in the 3 boxes and use the Hund’s rule. The last arrow lands in the 3rd box which is 1. The mℓ of sulfur is 1.

37
Q

How do you find Spin ms? (quantum numbers)

A

Do mℓ before this. Once you have the final arrow in mℓ, if it is an up arrow, it is +1/2, if it is a down arrow, it is -1/2.

38
Q

Find the 4 quantum numbers of Plutonium (5f6).

A

n=5
ℓ=3
mℓ=2
ms=+1/2

39
Q

What are molecules?

A

Group of 2 or more atoms held together by chemical bonds
Can be atoms of the same element or atoms of a different element.

40
Q

What is an element?

A

An element is a pure substance that cannot be broken down into any simpler substance through any physical or chemical means.
Most elements exist as solids at room temp
11 elements exists as gasses and 2 exists as liquids.

41
Q

What are Molecular Compounds?

A

Combination of different kinds of elements in fixed proportions by mass
Resulting compounds are completely different from the properties of the elements they are made of

42
Q

How do Ions from?

A

Ions are formed when an atom gains or loses one or more electrons
If a neutral atom loses an electron it will be positively charged, if it gains an electron it will be negatively charged.

43
Q

What are positively charged ions called?

A

Cations

44
Q

What are negatively charged ions called?

A

Anions

45
Q

Do metals form cations or anions?

A

cations

46
Q

Do non metals form cations or anions?

A

anions

47
Q

What are monoatomic ions?

A

ions that only have one atom (Ex. Na+ and Cl-)

48
Q

What do lewis electron dot symbols consist of?

A

element’s chemical symbol and a dot for each of its valence electrons
position of the dots don’t matter as long as we fill out the 4 sides maximum of 2 each side
the amount of dots corresponds to the column number (subtract 10 when in p block. column 1 = 1 dot, column 17 = 7 dots.

48
Q

What are polyatomic ions?

A

group of atoms that have a net charge (Ex. OH-)

49
Q

What is Ionic bonding?

A

Occurs when there is a complete transfer of electrons between a metal and non metal
Results in formation of ions
Atoms MUST become isoelectric (same number of electrons) with the nearest noble gas

49
Q

What is the octet rule

A

To attain maximum stability, an atom needs to share, gain or lose electrons until eight valence electrons are found on its valence shells.

50
Q

What are the steps of ionic bonding with LEDs?

A
  1. Transfer the electron (add more of the same element to transfer completely)
  2. The metal becomes a cation because it gave the electron to the non-metal. Non-metal becomes an anion because it received electrons. Add brackets to the completed octet.
  3. Get the ionic formula.
51
Q

Naming cations (+ charge) with stock method

A

Stock method indicates positive charge using a roman numeral in parenthesis after name of the metal. (Ex. Fe2+ is Iron (II), Cu+ is copper (I)

52
Q

Naming cations (+ charge) with classical system

A

Use the suffix -ous for ions with lower charge (Ex. Fe2+ is Ferrous, Cu+ is Cuprous)
Use the suffix -ic for ions with higher charge (Ex. Fe3+ is Ferric, Cu2+ is Cupric)

53
Q

Naming monoatomic (single element) anions (- charge)

A

We replace the ending of element with -ide. (Ex. Hydrogen to Hydride, Oxygen to Oxide, Nitrogen to Nitride)

54
Q

Naming non-oxyanions polyatomic anions (- charge)

A

Some poly atomic anions have endings with -ide (Ex. Hydroxide, Cyanide, Peroxide)

55
Q

Naming Oxyanions (polyatomic with oxygen)

A

-ate is used for common anions
-per is added to -ate for anions with one more oxygen than -ate ions
-ite is used for anions with one less oxygen than -ate anions
-hypo is added to ite for anions with two less oxygen than -ate

56
Q

Naming binary ionic compounds

A

First, name the metal followed by the non-metal ending with -ide
Cation name first, then Anion name (Ex. Calcium Chloride, Aluminum Perchlorate, Cupric Nitrate)

57
Q

Writing chemical formulas for binary ionic compounds using the criss cross method

A

We write the charges then transfer them over to the other element and make it the amount below the element.
We can use Na and S for this example.
Na has a charge of 1+ and S has a charge of 2-
Na1+ S2-
Na2S

Cancel out the numbers below if both elements have the same

FLASHCARDS (6 decks)

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