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Chemistry Semester 2 > Semester reviews extras > Flashcards

Semester reviews extras Flashcards

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1
Q

What do the names of all binary compounds, both ionic and molecular, end in

A

-ide

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2
Q

When naming acids, the prefix hydro- is used when the name of the acid ends in

A

-ide

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3
Q

What subatomic particle plays the greatest part in determining the physical and chemical properties of an element

A

Electron

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4
Q

How many energy sublevels are there in the second principal energy level

A

2

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5
Q

What is the maximum number of orbitals in th ep sublevel

A

3

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6
Q

What is the maximum of d orbitals in a given principal energy level

A

5

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7
Q

What types of atomic orbitals are in the htird principal energy level

A

S, P, and D only

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8
Q

Emission of light from an atom occurs when the electon…

A

Drops from a higher to a lower energy level

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9
Q

Each period number in the periodic table corresponds to…

A

A principal energy level

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10
Q

What criterion is used to arrange the elements i rows and columns on the periodic table

A

SImilarity in properties

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11
Q

The periodic law states that there is a periodic repetition of the physical and chemical properties of elements

A

When they are arranged in order of increasing atomic number

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12
Q

Why is the radius of a positive ion always less than the radius of its neutral atom

A

The nucleus pulls the remaining electrons closer

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13
Q

Why is the radius of a negative ion always greater than the radius of its neutral atom

A

Because the repulsion of electrons increases

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14
Q

What term is used to describe an atom’s tendency to attract electrons to itself when it is chemically combined with another element

A

Electronegativity

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15
Q

When do cations form

A

When an atom loses electrons

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16
Q

What kind of ion does sulfur become when it combines with a metal

A

Anion

17
Q

What is the electrical charge of a cation

A

Positive

18
Q

What does the octect rule say

A

Eight electrons in their principal energy level

19
Q

What is the name given to the energy required to break a covalent single bond

A

Bond energy

20
Q

How many valence electrons does an atom of halogen have

A

7

21
Q

According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible

A

Pairs of valence electrons

22
Q

What are the components of binary molecular compounds

A

Two metallic elements

23
Q

What is not true about all chemical reactions

A

New atoms are formed as products

24
Q

What is a driving force in a dr reaction

A

A precipitate is formed

25
Q

What is a false statement about yield

A

TAhe actual yeild may be different from the theoretical yeild because insufficent limiting reactant was used

26
Q

Bohrs model

A
  • Energy levels
  • Electrons moves between energy levels when they gain and lose energy
  • Electrons emit light when they release energy and fall closer to the nucleus
27
Q

Bohr’s model how do electrons emit light

A
  • When energy comes in, the electron absorbs some enery and jumps away from the nucleus
  • The electron gives off that energy in the form of the light as the electron moves back towards the nucleus
28
Q

Why is silver always a plus 1 charge

A

5s^2 4d^9
One electon from s orbital moves to d so completely fille d and half filled s. It then loses the single electron from the s orbital

29
Q

Ionization energy

A

Amount of energy required to remove and electron

30
Q

Electron Affinity

A

Amount of energy released when an atom gains an electron

31
Q

Electronegativity

A

Amount of attraction an atom has for a bonded electron

32
Q

Lattice energy

A

AMount of energy reuiqred to separate a mole of ions in an ionic compound

33
Q

WHat are the types of IMF energies from weak to strong

A

LDF->DD->HB

34
Q

LDF

A
  • A temporary dipole caused by a momentary unequal charge

- Made stronger by more electrons bc more electrons the higher probability for and unequal distribiution of charge

35
Q

DD

A

A permenant partial positive and partial negative charge (dipole) cuased by polar bonds an an asymmetrical molcule
-The greater the EN dif, the greater the strength there is a larger difference in the sharing of electrons,, so a greater partial positive and negative charge

36
Q

HB

A

A very stong dipole caused by hydrogen being attached to nitrogen, flourine, or oxygen

37
Q

Spectator ion

A

Ions that don’t participate in the formation of solid, liquid, or gas, so they get crossed out

Chemistry Semester 2 (5 decks)

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