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GRADE 11 FIRST SEM Midterms > CHEM 01 3 Periodicity > Flashcards

CHEM 01 3 Periodicity Flashcards

1
Q

A powerful tool for understanding and predicting the physical and chemical properties of elements

A

Periodic Table

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2
Q

-The number of protons in the nucleus of the atom

A

Atomic Number

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3
Q

-The average mass of the atoms in an element

A

Atomic Mass

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4
Q

-Usually from a Greek or Latin word for the element or a substance containing the element

A

Element Name

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5
Q

-Short-hand abbreviation for the element name

A

Symbol

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6
Q

-The person credited the most for the development of the periodic table
-He was not the first scientist who tried to arrange elements in a certain order
-Chemists mostly credit him
-Because he also used chemical properties to organize the table
-He left blanks for future elements
-Elements that would eventually be found
-Predicted some missing elements

A

Dmitri Mendeleev

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7
Q

-Had the same conclusions as Dmitri Mendeleev

A

Lothar Meyer

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8
Q

-Dmitri Mendeleev and Lothar Meyer independently came to the same conclusion about how elements should be grouped

True or False

A

True

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9
Q

-The chemical reactivity of the elements is largely determined by their ….
-Are the outermost electrons

A

Valence Electrons

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10
Q

-Referred to as core electrons

A

Nonvalence Electrons

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11
Q

-Going across the periodic table
-Horizontal row
-Elements are arranged in these

A

Periods

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12
Q

-Going down a column, elements are arranged as these
-Vertical column
-All elements in a given …. Have the same number and type of valence electron

A

Groups

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13
Q

-The alkali mentals (Group 1A elements) all have the same electron configuration of ns¹
-The all tend to lose one electron to form the unipositive cation
-Hence, they share physical and chemical property

True or False

A

True

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14
Q

-Are soft, metallic solids
-They are found only in compounds in nature, not in their elemental forms
-Typical metallic properties (luster, conductivity) are seen in them

A

Alkali Metals

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15
Q

-Have higher densities and melting points than alkali metals
-They readily form +2 cations, losing the 2 valence electrons.

A

Alkaline Earth Metals

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16
Q

-Are typical nonmetals
-They have highly negative electron affinities, so they exist as anions in nature
-They react directly with metals to form metal halides

A

Halogens

17
Q

-Helium and neon are chemically inert (They have desired electrons)
-This lack of chemical reactivity is due to the completely filled ns and np subshells
-A condition that often correlates with great stability: Law of Octaves
-They are found as monatomic gases.

A

Noble Gases

18
Q

-Right to Left (Left is more Metallic)
-Top to Bottom (Bottom is more Metallic)

A

Metallic Character (Direction)

19
Q

-Most of the elements in nature are these
-The following are some properties these:
-Shiny luster
-Conduct heat and electricity
-Malleable and ductile
-Solids at room temperature (except mercury)
-Low ionization energies/form cations easily

A

Metals

20
Q

-Are found on the right-hand side of the periodic table.
-Properties of these include the following:
-Solid, liquid, or gas (depends on element)
-Solids are dull, brittle, poor conductors
-Large negative electron affinity, so they form anions readily

A

Non-Metals

21
Q

-Have some characteristics of metals and some of nonmetals
-Several are electrical semiconductors (computer chips)

A

Metalloids

22
Q

-Is the repetitive pattern of property for elements based on the atomic number.
-The following properties are discussed in this unit:
-Sizes of atoms and ions
-Ionization energy
-Electron affinity
-Electronegativity

A

Periodicity

23
Q
  • is a fundamental property that leads to many of the trends
    -Many properties of atoms depend on electron configuration and on how strongly the outer electrons in the atoms are attracted to the nucleus
    -The attractive force between an electron and the nucleus depends on the magnitude of the nuclear charge
    -And on the average distance between the nucleus and the electron
A

Effective nuclear charge

24
Q
  • It is tempting to think of atoms as hard, spherical objects
    -According to the quantum- mechanical model,
    -However, atoms do not have sharply defined boundaries at which the electron distribution becomes zero
    -Hence, we define the size of an atom in terms of its …
    -Which is one-half the distance between the two nuclei in two adjacent metal atoms or in a diatomic molecule
A

Atomic Radius

25
Q

-Is the radius of a cation or an anion

A

Ionic Radius

26
Q

-Are smaller than their parent atoms
-Removing one or more electrons from an atom reduces electron-electron repulsion but the nuclear charge remains the same
-So the electron cloud shrinks

A

Cations

27
Q

-Are larger than their parent atoms
-Because the nuclear charge remains the same but the repulsion resulting from the additional electron(s) enlarges the domain of the electron cloud

A

Anions

28
Q

-Group of ions all containing the same number of electrons in an ….,
-The more positive the charge, the smaller the ion

A

Isoelectric Series

29
Q

-Is the minimum energy required to remove an electron from the ground state of a gaseous atom or ion
-The first ionization energy is the energy required to remove the first electron
-The second ionization energy is the energy required to remove the second electron
-The higher the ionization energy, the more difficult it is to remove an electron

A

Ionization Energy

30
Q

-Is the energy required to remove the first electron

A

First Ionization Energy

31
Q

-Is the energy required to remove the second electron

A

Second Ionization Energy

32
Q

-Have higher ionization energy values

A

Smaller Atoms

33
Q

-Measures the energy change when an atom gains an electron
-Measures the attraction, or affinity
-Of the atom for the added electron
-For most elements, it is negative in value
-Indicates that an atom easily accepts electrons

A

Electron Affinity

34
Q

-Is the ability of an atom in a molecule to attract shared electrons to itself
-Elements with higher ……. have a greater tendency to attract electrons than do elements with low …….

A

Electronegativity

35
Q

-Elements that exist as individual atoms
-Noble gases

A

Monoatomic Gases

36
Q

-Elements that appear in pairs

A

Diatomic Gases

37
Q

-An atom having a positive 1 charge that is a cation with +1 charge
-Has donated one of its electrons to form a unipositive cation
-The all tend to lose one electron to form the unipositive cation
-Only one valence electron

A

Unipositive Cation

38
Q

-An atom having a negative 1 charge
-Anions with a charge of -1
-Gaining one electron

A

Uninegative Anion

GRADE 11 FIRST SEM Midterms (15 decks)

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